Chapter 4 5 162 What The Molar Concentration Chloride Ions

Chapter 04 – Reactions in Aqueous Solutions

162. What is the molar concentration of chloride ions in a solution prepared by mixing 100.

mL of 2.0 M KCl with 50. mL of a 1.5 M CaCl2 solution?

163. What volume of concentrated nitric acid (15.0 M) is required to make 100. mL of a 3.0

M nitric acid solution?

Chapter 04 – Reactions in Aqueous Solutions

164. During a titration the following data were collected. A 10. mL portion of an unknown

monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to

neutralize the sample. What is the molarity of the acid solution?

165. During a titration the following data were collected. A 10. mL portion of an unknown

monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to

neutralize the sample. How many moles of acid are present in 2.0 liters of this unknown

solution?

Chapter 04 – Reactions in Aqueous Solutions

166. If 145 grams of potassium nitrate were added to water to make 1,500 mL of solution.

What would the molarity of the resulting solution be?

167. During a titration the following data were collected. A 50.0 mL portion of an HCl

solution was titrated with 0.500 M NaOH; 200. mL of the base was required to neutralize the

sample. How many grams of HCl are present in 500. mL of this acid solution?

Chapter 04 – Reactions in Aqueous Solutions

168. Which substance is acting as a Brønsted acid in the following reaction?

HSO4– + NH4+ → H2SO4 + NH3

169.

Select True or False: H2O is acting as a Brønsted acid in the following reaction.

NH3 + H2O → NH4+ + OH–

Chapter 04 – Reactions in Aqueous Solutions

170. Shown here is the balanced molecular equation that would occur between CaCl2(aq) and

Na2CO3(aq). Which of the following is the balanced net ionic equation?

Molecular equation: CaCl2(aq) + Na2CO3(aq) → CaCO3(s) + 2NaCl(aq)

171.

True or False: The two reactions shown here represent balanced molecular and net ionic reactions for the acid-base

neutralization reaction between H3PO4(aq) and Ba(OH)2(aq).

Molecular equation: 2H3PO4(aq) + 3Ba(OH)2(aq) → Ba3(PO4)2(s) + 6H2O(l)

Net ionic equation: 2H3PO4(aq) + 3Ba2+(aq) + 6OH–(aq) → Ba3(PO4)2(s) + 6H2O(l)

Chapter 04 – Reactions in Aqueous Solutions

172. Select True or False: The following two equations show both the correct balanced

molecular and net ionic equations for the reaction that would occur between Al(s) and

Co(NO3)2(aq).

Molecular equation: 2Al(s) + 3Co(NO3)2(aq) → 2Al(NO3)3(aq) + 3Co(s)

Net ionic equation: 2Al(s) + Co2+(aq) → 2Al3+(aq) + Co(s)

173. Shown here is the balanced molecular equation for the reaction that would occur between

CuCl2(aq) and Pb(s). Which of the following, if any, shows the correctly balanced net ionic

equation?

Molecular equation: CuCl2(aq) + Pb(s) → Cu(s) + PbCl2(s)

Chapter 04 – Reactions in Aqueous Solutions

174. A piece of copper metal was added to an aqueous solution of silver nitrate, and within a

few minutes it was observed that a grey crystalline solid formed on surface of the copper. The

solution turned a blue color characteristic of copper(II) ions. Select the correct balanced

chemical equation for this reaction.

175. A piece of copper metal was added to an aqueous solution of silver nitrate, and within a

few minutes it was observed that a grey crystalline solid formed on surface of the copper. The

solution turned a blue color characteristic of copper(II) ions. Select the correct net ionic

equation for this reaction.

Chapter 04 – Reactions in Aqueous Solutions

176. A piece of lead metal was added to an aqueous solution of copper(II) nitrate, and within

a few minutes it was observed that the lead turned black and crumbled. The characteristic blue

solution of copper (II) ions had faded. (NOTE: Lead forms a 2+ ion when it reacts.) Select the

balanced chemical equation for this reaction.

177. Select True or False: The following net ionic equation correctly shows the result of this

experiment: A piece of lead metal was added to an aqueous solution of copper(II) nitrate, and

within a few minutes it was observed that the lead turned black and crumbled. The

characteristic blue solution of copper(II) ions had faded. (NOTE: Lead forms a 2+ ion when it

reacts.)

Chapter 04 – Reactions in Aqueous Solutions

178. A piece of zinc metal was added to an aqueous solution of lead(II) nitrate. After some

time it was observed that the zinc metal appeared to fall apart and a solid had accumulated at

the bottom of the reaction vessel.

Select the balanced chemical equation for this reaction.

179. Select True or False: The following net ionic equation correctly shows the result when a

piece of zinc metal is added to an aqueous solution of lead(II) nitrate. After some time it was

observed that the zinc metal appeared to fall apart and a solid had accumulated at the bottom

of the reaction vessel.

Zn(s) + Pb2+(aq) →Zn2+(aq) + Pb(s)

Chapter 04 – Reactions in Aqueous Solutions

180. The following experiments were carried out and observations recorded.

Expt. #1: copper metal was added to an aqueous solution of silver nitrate

Observation: The copper become coated with a substance.

Expt. #2: lead metal was added to an aqueous solution of copper(II) nitrate

Observation: The lead turned black and crumbled.

Expt. #3: zinc metal was added to an aqueous solution of lead(II) nitrate

Observation: The zinc appeared to fall apart.

Which, if any, of the following properly ranks the metals from most active to least active.

Chapter 04 – Reactions in Aqueous Solutions

181. Which, if any of the following correctly shows the balanced molecular equation for the

reaction that occurs when aqueous solutions of potassium iodide and lead(II) nitrate are

combined.

Chapter 04 – Reactions in Aqueous Solutions

182. If 73.5 mL of 0.200 M KI(aq) was required to precipitate all of the lead(II) ion from an

aqueous solution of lead(II) nitrate, how many moles of Pb2+ were originally in the solution?

183. Select True or False: Sugar dissolves in water, therefore it is a strong electrolyte.

184. Select True or False: Silver chloride (AgCl) has an extremely low solubility in water;

therefore, it is a weak electrolyte.

Chapter 04 – Reactions in Aqueous Solutions

185. Select True or False: Most compounds containing chlorides, bromides, and iodides are

186.

Select True or False: The following reaction is an acid-base neutralization reaction.

H2SO4(aq) + CaBr2(aq) → CaSO4(s) + 2HBr(g)

187.

Select True or False: The oxidation number of N in NO is +7.

Chapter 04 – Reactions in Aqueous Solutions

188.

Select True or False: Hydrogen is oxidized in the following chemical reaction.

H2 + Cl2 → 2HCl

189.

Select True or False: The following equation is an example of a net ionic equation.

Na+(aq) + Br–(aq) + Ag+(aq) + NO3–(aq) → AgBr(s) + Na+(aq) + NO3–(aq)

190. Select True or False: The oxidation number of iodine increases by 6 in the following

reaction.

Chapter 04 – Reactions in Aqueous Solutions

192. Select True or False: The following reaction is a redox reaction.

CaC2(s) + H2O(l) → HCCH(g) + CaO(s)