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Problem 20a1
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of CH3COCH3?
Problem 20b
Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (b) If 0.1 mol of each compound is dissolved in solution, which one contains 0.2 mol of solute particles, which contains 0.1 mol of solute particles, and which contains somewhere between 0.1 and 0.2 mol of solute particles?
Problem 21
Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) MgBr2 (b) NH4OH (c) Ni(CH3COO)2 (d) AgNO3 (e) FeCO3.
Problem 22
Predict whether each of the following compounds is soluble in water: (a) MgS (b) Cr(OH)3 (c) ZnCl2 (d) Pb3(PO4)2 (e) Sr(CH3COO)2.
Problem 23
Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) Ca(CH3COO)2 and NaOH (b) K2CO3 and NH4NO3, (c) Na2S and FeCl3.
Problem 24
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) NH4I and CuCl2 (b) LiOH and MnCl2 (c) K3PO4 and CoSO4
Problem 25a
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate
Problem 25c
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (c) ammonium phosphate and calcium chloride
Problem 26a,b
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction.
(a) Ba(OH)2(aq) + FeCl3(aq) →
(b) ZnCl2(aq) + Cs2CO3(aq) →
Problem 28
Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb1NO322, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br-, CO32-, NO3-?
- You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3, CaCl2, or Al21SO423. A friend suggests that you test a portion of the solution with Ba1NO322 and then with NaCl solutions. According to your friend's logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle? (a) Barium sulfate could precipitate. (b) Silver chloride could precipitate. (c) Silver sulfate could precipitate. (d) More than one, but not all, of the reactions described in answers a–c could occur. (e) All three reactions described in answers a–c could occur.
Problem 29
Problem 33a
State whether each of the following statements is true or false. Justify your answer in each case. (a) Sulfuric acid is a monoprotic acid.
Problem 33b
State whether each of the following statements is true or false. Justify your answer in each case. (b) HCl is a weak acid.
Problem 33c
State whether each of the following statements is true or false. Justify your answer in each case. (c) Methanol is a base.
Problem 34c
State whether each of the following statements is true or false. Justify your answer in each case.
(c) Although sulfuric acid is a strong electrolyte, an aqueous solution of H2SO4 contains more HSO4- ions than SO42- ions.
Problem 35a
Label 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) HF
Problem 35b
Label 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, CH3CN
Problem 35d
Label 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.
- Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) PbCl2 (b) N(CH3)3 (c) CsOH (d) H2S (e) CrCl2 (f) Ni(CH3COO)2.
Problem 38
Problem 40a
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous barium hydroxide
Problem 40b
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (b) Solid chromium(III) hydroxide reacts with nitrous acid.
Problem 40c
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (c) Aqueous nitric acid and aqueous ammonia react.
Problem 41a,b
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each: (a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid (b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.
Problem 42a,b
Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: FeO(s) + 2 HClO4(aq) → Fe(ClO4)2(aq) + H2O(l) (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between NiO(s) and an aqueous solution of nitric acid.
- Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions. (a) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when each substance reacts with a hydrochloric acid solution. (b) By observing the reactions in part (a), how could you distinguish any of the three magnesium substances from the other two?
Problem 43
- As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. (a) Write the molecular and net ionic equations for this reaction. (b) Based on the definitions of acid and base, what ion is the base in this reaction? (c) What is the acid in the reaction? (d) What is the spectator ion in the reaction?
Problem 44
- True or false: (a) If a substance is oxidized, there must be more oxygen in the substance.
Problem 45
- True or false: (a) Reduction occurs if the oxidation number of an element increases
Problem 46
Problem 47b
(a) Which region of the periodic table shown here contains elements that are easiest to oxidize? (b) Which region contains the least readily oxidized elements?
Problem 48a,b,c
Determine the oxidation number of sulfur in each of the following substances: (a) barium sulfate, BaSO4 (b) sulfurous acid, H2SO3 (c) strontium sulfide, SrS