04:22What Makes Something Acidic? | Acids, Bases & Alkali's | Chemistry | FuseSchoolFuseSchool - Global Education343views
Multiple ChoiceWhich of the following compound(s) cannot be classified as an acid?A. H2SB. HCNC. H2D. C2H6E. All are acids1098views2rank5commentsHas a video solution.
Multiple ChoiceWhich is the weakest acid from the following?1287views5rank2commentsHas a video solution.
Multiple ChoiceWhich of the following acids would be classified as the strongest?1493views3rank5commentsHas a video solution.
Multiple ChoiceRank the following oxyacids in terms of increasing acidity. a) HClO3b) HBrO4c) HBrO3d) HClO41416views3rank1commentsHas a video solution.
Multiple ChoiceClassify each of the following as a strong acid, weak acid, strong base or weak base.1111views2rank3commentsHas a video solution.
Multiple ChoiceClassify each of the following as a strong acid, weak acid, Strong base, or weak base. 621views1rank2commentsHas a video solution.
Multiple ChoiceClassify each of the following as a strong acid, weak acid, strong base or weak base.708views4rank5commentsHas a video solution.
Multiple ChoiceWhich of the following is true in regards to HNO3? a) It has a bitter taste. b) It produces H+ ions in water.c) It exists as only molecules when dissolved in H2O. d) It decreases the acidity of the solution.171views4rankHas a video solution.
Textbook QuestionThe following pictures represent equal volumes of aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity. Which is the strongest acid? (a) HX (b) HY (c) HZ (d) All three acids are strong acids and have equal strength.471viewsHas a video solution.
Textbook QuestionConsider the conjugate bases, 1X-, Y-, Z-2 in Problem 2. If you mix equal concentrations of reactants and products, which of the following reactions will proceed to the left? (LO 16.3) (a) HX + Y- HY + X- (b) HX + Z- HZ + X- (c) HY + X- HX + Y- (d) HZ + Y- HY + Z-154viewsHas a video solution.
Textbook QuestionWhich is the strongest acid? (LO 16.4) (a) HClO3 (b) HBrO3 (c) H2SO3 (d) H2TeO31941viewsHas a video solution.
Textbook QuestionThe probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. (c) Why is the temperature given on the pH meter? 225viewsHas a video solution.
Textbook QuestionWhat is the concentration of hydroxide ions 3OH-4 in a glass of wine with pH = 3.64? (LO 16.5, 16.6) (a) 2.3 * 10-4 M (b) 6.4 * 10-3 M (c) 6.8 * 10-9 M (d) 4.4 * 10-11 M312viewsHas a video solution.
Textbook QuestionThe following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+.(c) Which solution would have the highest pH? 1418views1rankHas a video solution.
Textbook QuestionThe following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+. (a) Which of the acids is a strong acid? Explain. 364viewsHas a video solution.
Textbook QuestionAn acid solution with a concentration of 0.500 M has a pH = 3.21. What is the Ka of the acid? (LO 16.8) (a) 1.2 * 10-5 (b) 1.7 * 10-6 (c) 7.6 * 10-7 (d) 5.4 * 10-3362viewsHas a video solution.
Textbook QuestionEach of the three molecules shown here contains an OH group, but one molecule acts as a base, one as an acid, and the third is neither acid nor base. (c) Which one is neither acidic nor basic? 470viewsHas a video solution.
Textbook QuestionPhenylephrine, an organic substance with molecular formula C9H13NO2, is used as a nasal decongenstant in over-thecounter medications. The molecular structure of phenylephrine is shown below using the usual shortcut organic structure. (c) Would you expect a solution of phenylephrine hydrochloride to be acidic, neutral, or basic? 271viewsHas a video solution.
Textbook QuestionPhenylephrine, an organic substance with molecular formula C9H13NO2, is used as a nasal decongenstant in over-thecounter medications. The molecular structure of phenylephrine is shown below using the usual shortcut organic structure. (a) Would you expect a solution of phenylephrine to be acidic, neutral, or basic? 650viewsHas a video solution.
Textbook QuestionAmmonia 1NH32 has base dissociation constant 1Kb2 of 1.8 * 10-5. What is the concentration of an aqueous ammonia solution that has a pH of 11.68? (LO 16.11) (a) 0.28 M (b) 3.6 M (c) 9.0 * 10-3 M (d) 1.3 M472viewsHas a video solution.
Textbook QuestionConsider the molecular models shown here, where X represents a halogen atom. (b) Does the acidity of each molecule increase or decrease as the electronegativity of the atom X increases?186viewsHas a video solution.
Textbook QuestionConsider the molecular models shown here, where X represents a halogen atom. (a) If X is the same atom in both molecules, which molecule will be more acidic? 258viewsHas a video solution.
Textbook QuestionWhich of the following statements is false? (a) An Arrhenius base increases the concentration of OH- in water. (b) A Brønsted-Lowry base is a proton acceptor. (c) Water can act as a Brønsted–Lowry acid. (d) Water can act as a Brønsted–Lowry base. (e) Any compound that contains an –OH group acts as a Brønsted-Lowry base.356viewsHas a video solution.
Textbook QuestionGive the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+.271viewsHas a video solution.
Textbook QuestionGive the conjugate base of the following Brønsted–Lowry acids: (i) HCOOH, (ii) HPO42-.344viewsHas a video solution.
Textbook QuestionGive the conjugate acid of the following Brønsted–Lowry bases: (i) SO42-, (ii) CH3NH2.417viewsHas a video solution.
Textbook Question(a) Calculate the percent ionization of 0.0075 M butanoic acid 1Ka = 1.5 * 10-52.428viewsHas a video solution.
Textbook Question(b) Calculate the percent ionization of 0.0075 M butanoic acid in a solution containing 0.085 M sodium butanoate.359views1commentsHas a video solution.
Textbook QuestionIdentify the Brønsted–Lowry acid and the Brønsted–Lowry base on the left side of each of the following equations, and also identify the conjugate acid and conjugate base of each on the right side: (b) 1CH323N1aq2 + H2O1l2Δ1CH323NH +1aq2 + OH -1aq2166viewsHas a video solution.
Textbook Question(a) Calculate the percent ionization of 0.125 M lactic acid 1Ka = 1.4 * 10-42.652viewsHas a video solution.
Textbook QuestionIdentify the Brønsted–Lowry acid and the Brønsted– Lowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side. (a) HBrO1aq2 + H2O1l2ΔH3O+1aq2 + BrO-1aq2216viewsHas a video solution.
Textbook QuestionWhat is the conjugate acid of HSO3-? What is its conjugate base?860views1rankHas a video solution.
Textbook QuestionLabel each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (e) NH3.179viewsHas a video solution.
Textbook QuestionLabel each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (d) Cl-163viewsHas a video solution.
Textbook QuestionLabel each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (c) O2-207viewsHas a video solution.
Textbook QuestionLabel each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (b) HCO3-281viewsHas a video solution.
Textbook QuestionLabel each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (a) CH3COO-456viewsHas a video solution.
Textbook QuestionLabel each of the following as being a strong acid, a weak acid, or a species with negligible acidity. In each case write the formula of its conjugate base, and indicate whether the conjugate base is a strong base, a weak base, or a species with negligible basicity: (a) HCOOH185viewsHas a video solution.
Textbook QuestionPredict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow: (c) NO2-1aq2 + H2O1l2 Δ787viewsHas a video solution.
Textbook QuestionYou are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and any amount you need of sodium fluoride (NaF). (a) What is the pH of the hydrofluoric acid solution prior to adding sodium fluoride?175viewsHas a video solution.
Textbook QuestionYou are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid 1C6H5COOH2 and any amount you need of sodium benzoate 1C6H5COONa2. (a) What is the pH of the benzoic acid solution prior to adding sodium benzoate?183viewsHas a video solution.
Textbook QuestionPredict the products of the following acid–base reactions, and predict whether the equilibrium lies to the left or to the right of the reaction arrow: (c) HCO3-1aq2 + F-1aq2 Δ694viewsHas a video solution.
Textbook QuestionA formic acid solution has a pH of 3.25. Which of these substances will raise the pH of the solution upon addition? Explain your answer. a. HCl b. NaBr c. NaCHO2 d. KCl2402views1rankHas a video solution.
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. a solution that is 0.16 M in NH3 and 0.22 M in NH4Cl679viewsHas a video solution.
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. a solution that is 0.20 M in HCHO2 and 0.15 M in NaCHO21548views1rankHas a video solution.
Textbook QuestionCalculate 3H+4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3OH-4 = 8.8 * 10-9 M222viewsHas a video solution.
Textbook QuestionCalculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M253viewsHas a video solution.
Textbook QuestionCalculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.196viewsHas a video solution.
Textbook QuestionCalculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M275viewsHas a video solution.
Textbook QuestionCalculate the percent ionization of a 0.15 M benzoic acid solution in pure water and in a solution containing 0.10 M sodium benzoate. Why does the percent ionization differ significantly in the two solutions?1665viewsHas a video solution.
Textbook QuestionWhich of the following solutions is the most acidic? (a) 0.2 M Ba(OH)2, (b) 0.2 M H2SO3, (c) 1.0 M glucose 1C6H12O6).1326views2rankHas a video solution.
Textbook QuestionWhich of the following solutions is the most basic? (a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.747viewsHas a video solution.
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. c. a mixture that is 0.15 M in HF and 0.15 M in NaF1415viewsHas a video solution.
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. 0.15 M NaF324viewsHas a video solution.
Textbook QuestionSolve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a. 0.15 M HF944viewsHas a video solution.
Textbook QuestionBy what factor does 3H+4 change for a pH change of (a) 2.00 units?216viewsHas a video solution.
Textbook QuestionState whether each of the following statements is true or false. Justify your answer in each case. (c) Methanol is a base.230viewsHas a video solution.
Textbook QuestionState whether each of the following statements is true or false. Justify your answer in each case. (b) HCl is a weak acid.201viewsHas a video solution.
Textbook QuestionIn each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. d. C5H5N(aq) + H2O(l )C5H5NH+(aq) + OH-(aq)606views1rankHas a video solution.
Textbook QuestionIn each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. NH3(aq) + H2O(l )NH4+(aq) + OH-(aq)685viewsHas a video solution.
Textbook QuestionLabel each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (d) Ba1OH22.736viewsHas a video solution.
Textbook QuestionLabel each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (b) acetonitrile, CH3CN409viewsHas a video solution.
Textbook QuestionLabel each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. (a) HF275viewsHas a video solution.
Textbook QuestionIn each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. c. CO32 - (aq) + H2O(l )HCO3-(aq) + OH-(aq)840viewsHas a video solution.
Textbook QuestionIn each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. CH3NH2(aq) + H2O(l )CH3NH3+(aq) + OH-(aq)304viewsHas a video solution.
Textbook QuestionWrite the formula for the conjugate base of each acid. d. HF262viewsHas a video solution.
Textbook QuestionWrite the formula for the conjugate base of each acid. c. HCHO2718viewsHas a video solution.
Textbook QuestionWrite the formula for the conjugate base of each acid. b. H2SO3565viewsHas a video solution.
Textbook QuestionThe average pH of normal arterial blood is 7.40. At normal body temperature 137 °C2, Kw = 2.4 * 10-14. Calculate 3H+4, 3OH-4, and pOH for blood at this temperature.1847views1rankHas a video solution.
Textbook QuestionWrite the formula for the conjugate base of each acid. a. HCl1060viewsHas a video solution.
Textbook QuestionWrite the formula for the conjugate acid of each base. c. HSO4383viewsHas a video solution.
Textbook QuestionThe following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have been omitted for clarity. (e) What is the percent dissociation in the solution of HZ?288viewsHas a video solution.
Textbook QuestionThe following pictures represent aqueous solutions of three acids HA1A = X, Y, or Z2; water molecules have been omitted for clarity. (c) Which acid, if any, is a strong acid?599viewsHas a video solution.
Textbook QuestionLocate sulfur, selenium, chlorine, and bromine in the periodic table: (a) Which binary acid 1H2S, H2Se, HCl, or HBr2 is the strongest? Which is the weakest? Explain.148viewsHas a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). c. HBr472viewsHas a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). b. HCl214viewsHas a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). a. HNO3338viewsHas a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). H2SO3516viewsHas a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). c. H2SO4235viewsHas a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). b. HCHO2384viewsHas a video solution.
Textbook QuestionClassify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). a. HF667viewsHas a video solution.
Textbook QuestionThe following pictures represent solutions of three salts NaA (A- = X-, Y-, or Z-); water molecules and Na+ ions have been omitted for clarity. (a) Arrange the three A- anions in order of increasing base strength.268viewsHas a video solution.
Textbook QuestionThe following pictures represent solutions of three salts NaA (A- = X-, Y-, or Z-); water molecules and Na+ ions have been omitted for clarity. (b) Which A- anion has the strongest conjugate acid?174viewsHas a video solution.
Textbook QuestionThe following picture represents the hydrated metal cation M1H2O26 n + , where n = 1, 2, or 3. (c) Which M1H2O26n + ion 1n = 1,2, or 32 is the strongest acid, and which has the strongest conjugate base?137viewsHas a video solution.
Textbook QuestionCalculate [H3O+] and [OH-] for each solution at 25 °C. b. pH = 11.23433viewsHas a video solution.
Textbook QuestionCalculate [H3O+] and [OH-] for each solution at 25 °C. a. pH = 8.551498viewsHas a video solution.
Textbook QuestionPhenylacetic acid 1C6H5CH2COOH2 is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. A 0.085 M solution of C6H5CH2COOH has a pH of 2.68. Calculate the Ka value for this acid.919viewsHas a video solution.
Textbook QuestionA 0.100 M solution of chloroacetic acid 1ClCH2COOH2 is 11.0% ionized. Using this information, calculate 3ClCH2COO-4, 3H+4, 3ClCH2COOH4, and Ka for chloroacetic acid.575viewsHas a video solution.
Textbook QuestionA 0.100 M solution of bromoacetic acid 1BrCH2COOH2 is 13.2% ionized. Calculate 3H+4, 3BrCH2COO-4, 3BrCH2COOH4 and Ka for bromoacetic acid.631viewsHas a video solution.
Textbook QuestionThe hydronium ion H3O+ is the strongest acid that can exist in aqueous solution because stronger acids dissociate by transferring a proton to water. What is the strongest base that can exist in aqueous solution?3375views1rankHas a video solution.
Textbook QuestionCalculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H3O+] = 0.044 M [H3O+] = 0.045 M [H3O+] = 0.046 M993viewsHas a video solution.
Textbook QuestionIf a solution of HF 1Ka = 6.8 * 10-42 has a pH of 3.65, calculate the concentration of hydrofluoric acid.260viewsHas a video solution.
Textbook QuestionDetermine the concentration of H3O+ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.521654viewsHas a video solution.
Textbook QuestionWhich acid in each of the following pairs has the stronger conjugate base? See Table 16.1 to compare the relative strengths of conjugate acid-base pairs. (a) HCl or HF403viewsHas a video solution.
Textbook QuestionThe acid-dissociation constant for chlorous acid 1HClO22 is 1.1 * 10-2. Calculate the concentrations of H3O+, ClO2-, and HClO2 at equilibrium if the initial concentration of HClO2 is 0.0125 M.822viewsHas a video solution.
Textbook QuestionWhich base in each of the following pairs has the stronger conjugate acid? See Table 16.1 to compare the relative strengths of conjugate acid-base pairs. (a) Cl- or CO32-217viewsHas a video solution.
Textbook QuestionArrange each group of compounds in order of increasing acid strength. Explain your reasoning. (a) HCl, H2S, PH3633viewsHas a video solution.
Textbook QuestionDetermine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (c) 0.165 M hydroxylamine.873viewsHas a video solution.
Textbook QuestionThe pH of a solution of NH3 and NH4Br is 8.90. What is the molarity of NH4Br if the molarity of NH3 is 0.016 M?646viewsHas a video solution.
Textbook QuestionCalculate the percent dissociation of 0.10 M hydrazoic acid (HN3, Ka = 1.9 X 10^-5). Recalculate the percent dissociation of 0.10 M HN3 in the presence of 0.10 M HCl, and explain the change.703viewsHas a video solution.
Textbook QuestionWould you expect zirconium(II) oxide, ZrO, to react more readily with HCl(aq) or NaOH(aq)?151viewsHas a video solution.
Textbook QuestionCalculate the pH of 100.0 mL of 0.30 M NH3 before and after the addition of 4.0 g of NH4NO3, and account for the change. Assume that the volume remains constant.403viewsHas a video solution.
Textbook QuestionArrange the following oxides in order of increasing acidity: K2O, BaO, ZnO, H2O, CO2, SO2.491viewsHas a video solution.
Textbook QuestionIdentify the weakest acid in each of the following sets. Explain your reasoning. (b) NH3, H2O, H2S278viewsHas a video solution.
Textbook QuestionIdentify the weakest acid in each of the following sets. Explain your reasoning. (a) H2SO3, HClO3, HClO41104views1rankHas a video solution.
Textbook QuestionChlorine reacts with oxygen to form Cl2O7. (c) Would you expect Cl2O7 to be more reactive toward H+1aq2 or OH-1aq2?354views1rankHas a video solution.
Textbook QuestionCalculate the percent ionization of propionic acid 1C2H5COOH2 in solutions of each of the following concentrations 1Ka is given in Appendix D): (a) 0.250 M435viewsHas a video solution.
Textbook QuestionAn element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl4 is a colorless liquid with a boiling point of 58 °C. (b) Do you think that element X is a metal, nonmetal, or metalloid?183viewsHas a video solution.
Textbook QuestionAn element X reacts with oxygen to form XO2 and with chlorine to form XCl4. XO2 is a white solid that melts at high temperatures (above 1000 °C). Under usual conditions, XCl4 is a colorless liquid with a boiling point of 58 °C. (a) XCl4 reacts with water to form XO2 and another product. What is the likely identity of the other product?458viewsHas a video solution.
Textbook QuestionIdentify the stronger acid in each of the following pairs. Explain your reasoning. (b) H3PO4 or H3AsO4104viewsHas a video solution.
Textbook QuestionCitric acid, which is present in citrus fruits, is a triprotic acid (Table 16.3). (a) Calculate the pH of a 0.040 M solution of citric acid. (b) Did you have to make any approximations or assumptions in completing your calculations? (c) Is the concentration of citrate ion 1C6H5O7 3-2 equal to, less than, or greater than the H+ ion concentration?1297viewsHas a video solution.
Textbook QuestionDetermine the pH of an HNO2 solution of each concentration. In which cases can you not make the simplifying assumption that x is small? a. 0.500 M b. 0.100 M c. 0.0100 M1494views1commentsHas a video solution.
Textbook QuestionWrite balanced equations for the following reactions: (a) boron trichloride with water217viewsHas a video solution.
Textbook QuestionWrite balanced equations for the following reactions: (c) phosphorus pentoxide with water139viewsHas a video solution.
Textbook QuestionDetermine the pH of an HF solution of each concentration. In which cases can you not make the simplifying assumption that x is small? (Ka for HF is 6.8 * 10-4.) a. 0.250 M b. 0.0500 M c. 0.0250 M1607views1commentsHas a video solution.
Textbook QuestionWrite balanced equations for the following reactions: (d) arsenic trioxide with aqueous potassium hydroxide.215viewsHas a video solution.
Textbook QuestionConsider the base hydroxylamine, NH2OH. (a) What is the conjugate acid of hydroxylamine?930viewsHas a video solution.
Textbook QuestionDetermine the percent ionization of a 0.125 M HCN solution.1292views1commentsHas a video solution.
Textbook QuestionDetermine the percent ionization of a 0.225 M solution of benzoic acid.1145viewsHas a video solution.
Textbook QuestionEphedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2 A 0.035 M solution of ephedrine has a pH of 11.33. (a) What are the equilibrium concentrations of C10H15ON, C10H15ONH+, and OH-?936viewsHas a video solution.
Textbook QuestionEphedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base: C10H15ON1aq2 + H2O1l2 Δ C10H15ONH+1aq2 + OH-1aq2 A 0.035 M solution of ephedrine has a pH of 11.33. (b) Calculate Kb for ephedrine.294viewsHas a video solution.
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M260viewsHas a video solution.
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M192viewsHas a video solution.
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. b. 0.500 M692viewsHas a video solution.
Textbook QuestionCalculate the percent ionization of a formic acid solution having the given concentration. a. 1.00 M887viewsHas a video solution.
Textbook QuestionA 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.2417views1rank1commentsHas a video solution.
Textbook QuestionCalculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (e) -1.0485viewsHas a video solution.
Textbook QuestionCalculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25475viewsHas a video solution.
Textbook QuestionFind the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO21499viewsHas a video solution.
Textbook QuestionWhich of the following species behave as strong acids or as strong bases in aqueous solution? (a) HNO2 (b) HNO3(c) NH4+ (d) Cl-672viewsHas a video solution.
Textbook QuestionUsing data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (b) 0.035 M Na2S433viewsHas a video solution.
Textbook QuestionPyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (a) Write out the reaction that leads to this acidic pH.582views1rankHas a video solution.
Textbook QuestionPyridinium bromide 1C5H5NHBr2 is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. An aqueous solution of pyridinium bromide has a pH of 2.95. (c) A solution of pyridinium bromide has a pH of 2.95. What is the concentration of the pyridinium cation at equilibrium, in units of molarity?311viewsHas a video solution.
Textbook QuestionThe value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (a) Write the chemical equation for the equilibrium that corresponds to Ka.408viewsHas a video solution.
Textbook QuestionPredict the stronger acid in each pair: (e) benzoic acid (C6H5COOH) or phenol (C6H5OH).959viewsHas a video solution.
Textbook QuestionPredict the stronger acid in each pair: (c) HBrO3 or HBrO21251viewsHas a video solution.
Textbook QuestionLook up the values of Ka in Appendix C for C6H5OH, HNO3, CH3CO2H, and HOCl, and arrange these acids in order of: (b) Decreasing percent dissociation.414viewsHas a video solution.
Textbook QuestionDetermine the [OH-], pH, and pOH of a 0.15 M ammonia solution.1245viewsHas a video solution.
Textbook QuestionBased on their compositions and structures and on conjugate acid–base relationships, select the stronger base in each of the following pairs: (b) BrO- or BrO2-730viewsHas a video solution.
Textbook QuestionBased on their compositions and structures and on conjugate acid–base relationships, select the stronger base in each of the following pairs: (b) PO43- or AsO43-537views2rankHas a video solution.
Textbook QuestionIndicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) In general, the acidity of binary acids increases from left to right in a given row of the periodic table. (b) In a series of acids that have the same central atom, acid strength increases with the number of hydrogen atoms bonded to the central atom. (c) Hydrotelluric acid 1H2Te2 is a stronger acid than H2S because Te is more electronegative than S.482viewsHas a video solution.
Textbook QuestionCaffeine (C8H10N4O2) is a weak base with a pKb of 10.4. Calculate the pH of a solution containing a caffeine concentration of 455 mg>L.2609views4rankHas a video solution.
Textbook QuestionAmphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 225 mg>L.1999viewsHas a video solution.
Textbook QuestionIndicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) Acid strength in a series of H¬A molecules increases with increasing size of A. (b) For acids of the same general structure but differing electronegativities of the central atoms, acid strength decreases with increasing electronegativity of the central atom. (c) The strongest acid known is HF because fluorine is the most electronegative element.518viewsHas a video solution.
Textbook QuestionA vitamin C tablet containing 250 mg of ascorbic acid 1C6H8O6; Ka = 8.0 * 10-52 is dissolved in a 250 mL glass of water. What is the pH of the solution?1145viewsHas a video solution.
Textbook QuestionAcetic acid 1CH3COOH; Ka = 1.8 * 10-52 has a concentration in vinegar of 3.50% by mass. What is the pH of vinegar? (The density of vinegar is 1.02 g/mL.)1056viewsHas a video solution.
Textbook QuestionDetermine the [OH-] and pH of a solution that is 0.140 M in F-.1348viewsHas a video solution.
Textbook QuestionIndicate whether each of the following statements is correct or incorrect. (c) Conjugate acids of weak bases produce more acidic solutions than conjugate acids of strong bases.158viewsHas a video solution.
Textbook QuestionA typical aspirin tablet contains 324 mg of aspirin (acetylsalicylic acid, C9H8O4), a monoprotic acid having Ka = 3.0 * 10-4. If you dissolve two aspirin tablets in a 300 mL glass of water, what is the pH of the solution and the percent dissociation? 1334views1rankHas a video solution.
Textbook QuestionWrite balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation of the triprotic acid H3PO4.200viewsHas a video solution.
Textbook QuestionCalculate the concentration of all species in a 0.15 M KF solution.1358views1rankHas a video solution.
Textbook QuestionCalculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.1306viewsHas a video solution.
Textbook QuestionWrite chemical equations and corresponding equilibrium expressions for each of the three ionization steps of phosphoric acid.412viewsHas a video solution.
Textbook QuestionButyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (c) Calculate the pH of a 0.050 M solution of sodium butyrate.756viewsHas a video solution.
Textbook QuestionButyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (b) Calculate the pH of a 0.050 M solution of butyric acid.656views1rankHas a video solution.
Textbook QuestionRitalin is the trade name of a drug, methylphenidate, used to treat attention-deficit/hyperactivity disorder in young adults. The chemical structure of methylphenidate is (a) Is Ritalin an acid or a base? An electrolyte or a nonelectrolyte?563viewsHas a video solution.
Textbook QuestionStrychnine 1C21H22N2O22, a deadly poison used for killing rodents, is a weak base having Kb = 1.8 * 10-6. Calculate the pH of a saturated solution of strychnine (16 mg/100 mL).360viewsHas a video solution.
Textbook QuestionWhat is the pH at 25 C of water saturated with CO2 at a partial pressure of 1.10 atm? The Henry's law constant for CO2 at 25 C is 3.1 * 10-2 mol>L@atm.580viewsHas a video solution.
Textbook QuestionThe amino acid glycine 1H2N¬CH2¬COOH2 can participate in the following equilibria in water: H2N¬CH2¬COOH + H2OΔ H2N¬CH2¬COO- + H3O+ Ka = 4.3 * 10-3 H2N¬CH2¬COOH + H2OΔ+H3N¬CH2¬COOH + OH- Kb = 6.0 * 10-5 (b) What is the pH of a 0.050 M aqueous solution of glycine?290viewsHas a video solution.
Textbook QuestionBased on molecular structure, arrange the binary compounds in order of increasing acid strength. Explain your choice. H2Te, HI, H2S, NaH695viewsHas a video solution.
Textbook QuestionIn nonaqueous solvents, it is possible to react HF to create H2F+. Which of these statements follows from this observation? (a) HF can act like a strong acid in nonaqueous solvents, (b) HF can act like a base in nonaqueous solvents, (c) HF is thermodynamically unstable, (d) There is an acid in the nonaqueous medium that is a stronger acid than HF.430viewsHas a video solution.
Textbook QuestionBased on molecular structure, arrange the oxyacids in order of increasing acid strength. Explain your choice. HClO3, HIO3, HBrO3578viewsHas a video solution.
Textbook QuestionWrite a balanced net ionic equation for the reaction of each of the following ions with water. In each case, identify the Brønsted–Lowry acids and bases and the conjugate acid– base pairs. (a) CH3NH3+368viewsHas a video solution.
Textbook QuestionBased on these molecular views, determine whether each pictured acid is weak or strong. 438viewsHas a video solution.
Textbook QuestionCalculate the concentrations of all species present and the pH in 0.10 M solutions of the following substances. See Appendix C for values of equilibrium constants. (b) Sodium acetate, Na1CH3CO22504viewsHas a video solution.
Textbook QuestionCalculate the pH and the percent dissociation of the hydrated cation in 0.020 M solutions of the following substances. See Appendix C for values of equilibrium constants. (a) Fe1NO322249viewsHas a video solution.
Textbook QuestionCalculate the pH and the percent dissociation of the hydrated cation in the following solutions. See Appendix C for the value of the equilibrium constant. (a) 0.010 M Cr1NO323468viewsHas a video solution.
Textbook QuestionThe AIDS drug zalcitabine (also known as ddC) is a weak base with a pKb of 9.8. What percentage of the base is protonated in an aqueous zalcitabine solution containing 565 mg>L?308viewsHas a video solution.
Textbook QuestionThe pH of a 1.00 M solution of urea, a weak organic base, is 7.050. Calculate the Ka of protonated urea.1460viewsHas a video solution.
Textbook QuestionLactic acid is a weak acid found in milk. Its calcium salt is a source of calcium for growing animals. A saturated solution of this salt, which we can represent as Ca(Lact)2, has a [Ca2 + ] = 0.26 M and a pH = 8.78. Assuming the salt is completely dissociated, calculate the Ka of lactic acid.2098viewsHas a video solution.
Textbook QuestionCalculate the pH and the concentrations of all species present (H3O+ , F-, HF, Cl-, and OH-) in a solution that contains 0.10 M HF 1Ka = 3.5 * 10-42 and 0.10 M HCl.490viewsHas a video solution.
Textbook QuestionWhen NO2 is bubbled into water, it is completely converted to HNO3 and HNO2: 2 NO21g2 + H2O1l2S HNO31aq2 + HNO21aq2 Calculate the pH and the concentrations of all species present (H3O+ , OH-, HNO2, NO2 -, and NO3 -) in a solution prepared by dissolving 0.0500 mol of NO2 in 1.00 L of water. Ka for HNO2 is 4.5 * 10-4.735viewsHas a video solution.
Textbook QuestionAcid and base behavior can be observed in solvents other than water. One commonly used solvent is dimethyl sulfoxide (DMSO), which can be treated as a monoprotic acid 'HSol.' Just as water can behave either as an acid or a base, so HSol can behave either as a Brønsted–Lowry acid or base. (b) The weak acid HCN has an acid dissociation constant Ka = 1.3 * 10-13 in the solvent HSol. If 0.010 mol of NaCN is dissolved in 1.00 L of HSol, what is the equilibrium concentration of H2Sol + ?674viewsHas a video solution.
Textbook QuestionA 7.0 mass % solution of H3PO4 in water has a density of 1.0353 g/mL. Calculate the pH and the molar concentrations of all species present (H3PO4, H2PO4-, PO43-, H3O+ , and OH-) in the solution. Values of equilibrium constants are listed in Appendix C.362views1rankHas a video solution.
Textbook QuestionIn qualitative analysis, Ca2+ and Ba2+ are seperated from Na+, K+, Mg2+ by adding aqueous (NH4)2CO3 to a solution that also contains aqueous NH3 (Figure 17.18). Assume that the concentrations after mixing are 0.080 M (NH4)2CO3 and 0.16 M NH3. (a) List all the Bronsted-Lowry acids and based present initially, and identify the principal reaction.334viewsHas a video solution.
Textbook QuestionIn the case of very weak acids, 3H3O+ 4 from the dissociation of water is significant compared with 3H3O+ 4 from the dissociation of the weak acid. The sugar substitute saccharin 1C7H5NO3S2, for example, is a very weak acid having Ka = 2.1 * 10-12 and a solubility in water of 348 mg/100 mL. Calculate 3H3O+ 4 in a saturated solution of saccharin. (Hint: Equilibrium equations for the dissociation of saccharin and water must be solved simultaneously.)301viewsHas a video solution.
Textbook QuestionIn aqueous solution, sodium acetate behaves as a strong electrolyte, yielding Na+ cations and CH3CO2 - anions. A particular solution of sodium acetate has a pH of 9.07 and a density of 1.0085 g/mL. What is the molality of this solution, and what is its freezing point?1057viewsHas a video solution.
Textbook QuestionA 1.000 L sample of HF gas at 20.0 °C and 0.601 atm pressure was dissolved in enough water to make 50.0 mL of hydrofluoric acid. (a) What is the pH of the solution?146viewsHas a video solution.
Textbook QuestionA 1.000 L sample of HF gas at 20.0 °C and 0.601 atm pressure was dissolved in enough water to make 50.0 mL of hydrofluoric acid. (b) To what volume must you dilute the solution to triple the percent dissociation?237viewsHas a video solution.
Textbook QuestionYou may have been told not to mix bleach and ammonia. The reason is that bleach (sodium hypochlorite) reacts with ammonia to produce toxic chloramines, such as NH2Cl. For example, in basic solution: OCl-1aq2 + NH31aq2S OH-1aq2 + NH2Cl1aq2 (b) The following mechanism has been proposed for this reaction in basic solution: H2O + OCl-HOCl + OH- Fast, equilibrium constantK1 HOCl + NH3 S H2O + NH2Cl Slow, rate constantk2 Assuming that the first step is in equilibrium and the second step is rate-determining, calculate the value of the rate constant k2 for the second step. Ka for HOCl is 3.5 * 10-8.267viewsHas a video solution.
Open QuestionWhich of these substances contributes to soap's slippery texture: an acid, a base, carbonate, or water?48viewsHas a video solution.
Open QuestionAccording to the Arrhenius concept, if HNO3 were dissolved in water, it would act as33viewsHas a video solution.
Open QuestionThe pH of 2.65 m CH3NH2(aq) is 12.54. determine the value of Kb for methylamine.349viewsHas a video solution.