6. Chemical Quantities & Aqueous Reactions

Which of the following compounds is insoluble in water?

You are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next an Na2SO41aq2 solution is added and a white precipitate forms. What is the identity of the unknown white solid?

Which of the following solutions will not form a precipitate when added to 10 mL of 0.10 M KOH? (LO 4.10, 4.11) (a) 10 mL of 0.10 NH4Cl (b) 10 mL of 0.10 M PbSO4 (c) 10 mL of 0.10 M Fe(NO3)3 (d) 10 mL of 0.10 M AgCH3CO2

What kind of reaction is the 'water-splitting' reaction? H2O(l)¡H2(g) + ½ O2(g) (a) an acid-base reaction (b) a metathesis reaction (c) a redox reaction (d) a precipitation reaction

Three cations, Ni2 + , Cu2 + , and Ag+, are separated using two different precipitating agents. Based on Figure 17.23, what two precipitating agents could be used? Using these agents, indicate which of the cations is A, which is B, and which is C.

Write a balanced chemical equation for the reaction that occurs when (a) Mg(s) reacts with Cl21g2

Write a balanced chemical equation for the reaction that occurs when (a) titanium metal reacts with O21g2

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (b) Li3N1s2 + BN1s2 ¡Li3BN21s2

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) C7H161s2 + O21g2 ¡CO21g2 + H2O1l2

Balance the following equations and indicate whether they are combination, decomposition, or combustion reactions: (a) NaClO31s2¡NaCl1s2 + O2(g)

Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (c) Na2S and FeCl3.

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction.(b) LiOH and MnCl2

(a) When chlorine atoms react with atmospheric ozone, what are the products of the reaction?

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.

Three solutions are mixed together to form a single solution; in the final solution, there are 0.2 mol Pb1CH3COO)2, 0.1 mol Na2S, and 0.1 mol CaCl2 present. What solid(s) will precipitate?

Assume that an aqueous solution of a cation, represented as a red sphere, is allowed to mix with a solution of an anion, represented as a yellow sphere. Three possible outcomes are represented by boxes (1)–(3):

Which outcome corresponds to each of the following reactions? (a) 2 Na+(aq) + CO32-(aq) S (b) Ba2+(aq) + CrO42-(aq) S (c) 2 Ag+(aq) + SO32-(aq) S

Assume that an aqueous solution of a cation, represented as a blue sphere, is allowed to mix with a solution of an anion, repre-sented as a red sphere, and that the following result is obtained: Which combinations of cation and anion, chosen from the fol-lowing lists, are compatible with the observed results? Explain Cations: Na+, Ca2+, Ag+, Ni2+ Anions: Cl-, CO3 2-, CrO4 2-, NO3

Assume that an aqueous solution of OH-, represented as a blue sphere, is allowed to mix with a solution of an acid HnA, represented as a red sphere. Three possible outcomes are depicted by boxes (1)–(3), where the green spheres represent An-, the anion of the acid: Which outcome corresponds to each of the following reactions? (a) (b) (c)

Magnesium ions are removed in water treatment by the addition of slaked lime, Ca(OH)2. Write a balanced chemical equation to describe what occurs in this process

Natural gas consists primarily of methane, CH4(g). (b) Write a balanced chemical equation for the incomplete combustion of methane to product CO(g) as the only carbon-containg product.

Write a balanced equation for the reaction that occurs in each of the following cases: (c) A fresh surface of lithium metal is exposed to oxygen gas.

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal is exposed to an atmosphere of chlorine gas.

Write a balanced equation for the reaction that occurs in each of the following cases: (c) Potassium reacts with chlorine gas.

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Lithium is added to water.

Classify each of the following reactions as a precipitation, acid–base neutralization, or oxidation–reduction. (a) (b) (c)

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' c. CrBr2(aq) + Na2CO3(aq)¡

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' b. KCl(aq) + CaS(aq)¡

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. LiI(aq) + BaS(aq)

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' d. NH4Cl(aq) + AgNO3(aq)¡

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. NaNO3(aq) + KCl(aq)¡

A solution containing several metal ions is treated with dilute HCl; no precipitate forms. The pH is adjusted to about 1, and H2S is bubbled through. Again, no precipitate forms. The pH of the solution is then adjusted to about 8. Again, H2S is bubbled through. This time a precipitate forms. The filtrate from this solution is treated with 1NH422HPO4. No precipitate forms. Which of these metal cations are either possibly present or definitely absent: Al3 +, Na +, Ag +, Mg2 +?

Write a balanced equation for the reaction that occurs in each of the following cases: (d) Aluminum trichloride reacts with aqueous sodium hydroxide.

Write a balanced equation for the reaction that occurs in each of the following cases: (c) Hydrogen bromide gas reacts with chlorine gas.

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' c. copper(II) nitrate and magnesium sulfide

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. potassium carbonate and lead(II) nitrate

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate

"In the course of various qualitative analysis procedures, the following mixtures are encountered: (d) Ag+ and Mn2 + . Suggest how each mixture might be separated."

In the course of various qualitative analysis procedures, the following mixtures are encountered: (a) Zn2 + and Cd2 + . Suggest how each mixture might be separated.

Which of the following solutions will not form a precipitate when added to 0.10 M BaCl2? (a) 0.10 M LiNO3 (b) 0.10 M K2SO4 (c) 0.10 M AgNO3

Suggest how the cations in each of the following solution mixtures can be separated: (c) Pb2 + and Al3 +.

Which of the following solutions will not form a precipitate when added to 0.10 M NaOH? (a) 0.10 M MgBr2 (b) 0.10 M NH4Br (c) 0.10 M FeCl2

How would you prepare the following substances by a precipitation reaction? (a) PbSO4

How would you prepare the following substances by a precipitation reaction? (b) Mg3(PO4)2

Complete and balance each acid–base equation. c. H2SO4(aq) + NaOH(aq)¡

Complete and balance each acid–base equation. b. HC2H3O2(aq) + Ca(OH)2(aq)¡

Assume that you have an aqueous mixture of NaNO3 and AgNO3. How could you use a precipitation reaction to separate the two metal ions?

A solution of 105.0 mL of 0.300 M NaOH is mixed with a solution of 150.0 mL of 0.060 M AlCl3. (b) What precipitate forms?

Assume that you have an aqueous mixture of BaCl2 and CuCl2. How could you use a precipitation reaction to sepa-rate the two metal ions?

Write balanced chemical equations for (c) the combination reaction between sulphur dioxide gas and liquid water to produce sulfurous acid.

A solution of 105.0 mL of 0.300 M NaOH is mixed with a solution of 150.0 mL of 0.060 M AlCl3. (a) Write the balanced chemical equation for the reaction that occurs.

Assume that you have an aqueous solution of an unknown salt. Treatment of the solution with dilute NaOH, Na2SO4, and KCl produces no precipitate. Which of the following cations might the solution contain? (a) Ag+ (b) Cs+ (c) Ba2+ (d) NH4 +

Assume that you have an aqueous solution of an unknown salt. Treatment of the solution with dilute BaCl2, AgNO3, and Cu(NO3)2 produces no precipitate. Which of the following anions might the solution contain? (a) Cl- (b) NO3 (c) OH- (d) SO4- 2-

How could you use a precipitation reaction to separate each of the following pairs of cations? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (a)

How could you use a precipitation reaction to separate each of the following pairs of cations? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (b)

How could you use a precipitation reaction to separate each of the following pairs of anions? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (a)

Uranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear weapons. UF6 can be produced in a two-step reaction. Solid uranium (IV) oxide, UO2, is first made to react with hydrofluoric acid (HF) solution to form solid UF4 with water as a by-product. UF4 further reacts with fluorine gas to form UF6. (b) Which step is an acid-base reaction?

The following three solutions are mixed: 100.0 mL of 0.100 M Na2SO4, 50.0 mL of 0.300 M ZnCl2, and 100.0 mL of 0.200 M Ba(CN)2. (a) What ionic compounds will precipitate out of solution?

A 25.0-mL sample of 0.050 M barium nitrate solution was mixed with 25.0 mL of 0.050 M sodium sulfate solution labeled with radioactive sulfur-35. The activity of the initial sodium sulfate solution was 1.22 * 106 Bq>mL. After the resultant precipitate was removed by filtration, the remaining filtrate was found to have an activity of 250 Bq/mL. (a) Write a balanced chemical equation for the reaction that occurred.

A 250.0 g sample of a white solid is known to be a mixture of KNO3, BaCl2, and NaCl. When 100.0 g of this mixture is dis-solved in water and allowed to react with excess H2SO4, 67.3 g of a white precipitate is collected. When the remaining 150.0 g of the mixture is dissolved in water and allowed to react with excess AgNO3, 197.6 g of a second precipitate is collected. (a) What are the formulas of the two precipitates?

Write balanced ionic equations for the following reactions. (b) Aqueous sodium hydroxide is neutralized by aqueous acetic acid.

Write balanced ionic equations for the following reactions. (a) Aqueous perchloric acid is neutralized by aqueous calcium hydroxide.

Write balanced ionic equations for the following reactions. (b) Aqueous barium hydroxide is neutralized by aqueous nitric acid.

Write balanced ionic equations for the following reactions. (a) Aqueous hydrobromic acid is neutralized by aqueous calcium hydroxide.

Acetylene 1C2H22 and nitrogen 1N22 both contain a triple bond, but they differ greatly in their chemical properties. (c) Write balanced chemical equations for the complete oxidation of N2 to form N2O51g2 and of acetylene to form CO21g2 and H2O1g2. Write a balanced chemical equation for the complete oxidation of acetylene to form CO2( g) and H2O(g).

Trifluoroacetic acid has the chemical formula CF3CO2H. It is a colorless liquid that has a density of 1.489 g/mL. (b) Trifluoroacetic acid can react with NaOH in aqueous solution to produce the trifluoroacetate ion, CF3COO2. Write the balanced chemical equation for this reaction.

A hydrochloric acid solution will neutralize a sodium hydroxide solution. Look at the molecular views showing one beaker of HCl and four beakers of NaOH. Which NaOH beaker will just neutralize the HCl beaker? Begin by writing a balanced chemical equation for the neutralization reaction.

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' d. aqueous ammonium chloride and aqueous calcium hydroxide

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' a. HCl(aq) + Hg2(NO3)2(aq)¡

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' b. Cr(NO3)3(aq) + LiOH(aq)¡

Baking soda (sodium bicarbonate, NaHCO3) reacts with acids in foods to form carbonic acid 1H2CO32, which in turn decomposes to water and carbon dioxide gas. In a cake batter, the CO21g2 forms bubbles and causes the cake to rise. (a) A rule of thumb in baking is that 1/2 teaspoon of baking soda is neutralized by one cup of sour milk. The acid component in sour milk is lactic acid, CH3CH1OH2COOH. Write the chemical equation for this neutralization reaction.

A solution contains one or more of the following ions: Hg2 2 + , Ba2 + , and Fe2 + . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Which ions were present in the original solution?

A solution contains one or more of the following ions: Hg2 2 + , Ba2 + , and Fe2 + . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Write net ionic equations for the formation of each of the precipitates observed.

A compound with the formula XOCl2 reacts with water, yielding HCl and another acid H2XO3, which has two acidic hydrogens that react with NaOH. When 0.350 g of XOCl2 was added to 50.0 mL of water and the resultant solution was titrated, 96.1 mL of 0.1225 M NaOH was required to react with all the acid. (a) Write a balanced equation for the reaction of XOCl2 with H2O.

(a) Write a balanced equation for the reaction of potassium metal with water.

The mixing of which pair of reactants will result in a precipitation reaction?

What salt is produced in each of the following neutralization reactions?

Which of the following is a precipitation reaction?

Bacl2(aq)+agno3(aq)→

Chromium(iii) nitrate and sodium phosphate

Which of the following is a precipitation reaction