Chapter 4 Chem

You mix 50.0 mL of 0.165 M AgNO3 with 25.0 mL of 0.302 M KCl. What is the maximum mass of AgCl that can be formed?

1.08 g

. The pH of 1.0 × 10-3 M HNO3 is ____ .

3.0

Which one of the following compounds is a weak electrolyte when dissolved in water? a) CH3CO2H b) NaCH3CO2 c) KNO3 d) Na2SO4 e) sugar

CH3CO2H

Give the name of an acidic oxide and write a balanced chemical equation for the reaction of the oxide with water.

Carbon dioxide. CO2(aq) + H2O(l) → H2CO3(aq). (Other acidic oxides include nitrogen dioxide, sulfur dioxide, and sulfur trioxide.)

Which one of the following compounds is a nonelectrolyte when dissolved in water? a) NaBr b) Cu(NO3)2 c) NH3 d) KOH e) CaCl2

NH3

The pH of a sodium hydroxide solution gradually decreases if the solution is left in contact with air. In fact, the process can be hastened if a person exhales over a sodium hydroxide solution. Write a balanced chemical equation that describes the process by which the sodium hydroxide concentration decreases.

NaOH(aq) + CO2(aq) → Na+ (aq) + HCO3 - (aq)

acid is produced in a larger quantity than any other chemical in the United States. This chemical is used in the production of fertilizers, pigments, alcohol, paper and detergents.

Sulfuric

Which of the following chemical equations represent oxidation-reduction reactions? 1) Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s) 2) SrO(s) + H2O(l) → Sr(OH)2(aq) 3) AgNO3(aq) + NaI(aq) → AgI(s) + NaNO3(aq) a) 1 b) 2 c) 1 and 2 d) 1 and 3 e) 2 and 3

a) 1

The pH of 6.0 M KOH is 14.78. What is the hydrogen ion concentration of this solution? a) 1.7 × 10-15 M b) 2.2 × 10-14 M c) 6.0 × 10-14 M d) 1.0 × 10-6 M e) 1.3 × 10-1 M

a) 1.7 × 10-15 M

A 25.00 mL sample of NaOH is titrated with 15.23 mL of 0.2250 M HCl. What is the concentration of the NaOH solution? a) 2.198 × 10-3 M b) 0.02872 M c) 0.1371 M d) 0.3693 M e) 0.5223 M

c) 0.1371 M

. What is the pH of 0.53 M HNO3? a) -1.07 b) 0.22 c) 0.276 d) 1.07 e) 5.32

c) 0.276

How many liters of 0.1107 M NaOH contain 10.00 g of NaOH? a) 0.7290 L b) 1.107 L c) 2.258 L d) 3.198 L e) 4.428 L

c) 2.258 L

If 1.928 g KNO3 is dissolved in enough water to make 250.0 mL of solution, what is the molarity of potassium nitrate? a) 6.912 × 10-4 M b) 4.767 × 10-3 M c) 7.627 × 10-2 M d) 1.297 × 10-1 M e) 7.712 M

c) 7.627 × 10-2 M

A white solid is either KBr or KNO3. If an aqueous solution is prepared, which reagent will allow you to distinguish between the two compounds? a) HCl b) H2 c) AgNO3 d) CaO e) FeCl3

c) AgNO3

What is the net ionic equation for the reaction of limestone with a strong acid? a) Ca(s) + 2 H+ (aq) → Ca2+(aq) + H2(g) b) CaO(s) + 2 H+(aq) → Ca2+(aq) + H2O(l) c) CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + H2CO3(aq) d) CaCO3(s) + 2 H+ (aq) → Ca2+(aq) + H2CO3(s) e) CaCO3(s) + 2 H+ (aq) → Ca2+(aq) + CO2(g) + H2O(l)

c) CaCO3(s) + 2 HCl(aq) → CaCl2(aq) + H2CO3(aq)

Write a balanced equation for the reaction of baking soda, NaHCO3, with hydrochloric acid. a) HCl(aq) + NaHCO3(aq) → H2CO3(s) + NaCl(aq) b) 4 HCl(aq) + NaHCO3(aq) → CCl4(aq) + 2H2O(l) + NaOH(aq) c) HCl(aq) + NaHCO3(aq) → NaCl(aq) + H2O(l) + CO2(g) d) HCl(aq) + NaHCO3(aq) → NaOH(aq) + HCl(aq) + CO2(g) e) 4 HCl(aq) + NaHCO3(aq) → CH4(aq) + 2 Cl2(g) + O2(g) + NaOH(aq)

c) HCl(aq) + NaHCO3(aq) → NaCl(aq) + H2O(l) + CO2(g)

What is the oxidation number of each atom in potassium sulfate? a) K = +1, S = 0, O = -2 b) K = -1, S = +5, O = -2 c) K = +1, S = +6, O = -2 d) K = +1, S = +6, O = -1 e) K = -1, S = -2, O = +4

c) K = +1, S = +6, O = -2

What are the spectator ions in the reaction between nitric acid and sodium hydroxide? a) Na+ , OH- , H+ , and NO3 - b) H+ and OHc) Na+ and NO3 - d) H+ and NO3 - e) Na+ and OH

c) Na+ and NO3 -

Metal oxides react with water to produce ________. a) hydrogen gas b) acids c) bases d) precipitates e) reduced metals

c) bases

What is the oxidation number of nitrogen in N2O3? a) 0 b) +1 c) +2 d) +3 e) +4

d) +3

Which one of the following solutions will have the highest electrical conductivity? a) 0.010 M KCl b) 0.010 M CaI2 c) 0.010 M MgSO4 d) 0.010 M Al(NO3)3 e) 0.010 M Na2SO4

d) 0.010 M Al(NO3)3

Which one of the following solutions will have the highest electrical conductivity? a) 0.10 M AlCl3 b) 0.15 M SrBr2 c) 0.20 M NaBr d) 0.25 M Mg(NO3)2 e) 0.30 M KClO4

d) 0.25 M Mg(NO3)2

What is the mass, in grams, of solute in 0.175 L of 3.17 × 10-2 M KCl? a) 0.00555 g b) 0.181 g c) 0.255 g d) 0.414 g e) 13.5 g

d) 0.414 g

What is the net ionic equation for the reaction of sodium hydroxide with iron(III) nitrate? a) 3 Na+ (aq) + Fe3+(aq) → Na3Fe(s) b) NaOH(aq) + FeNO3(aq) → FeOH(s) + NaNO3(aq) c) Fe3+(aq) + 3 NO3 - (aq) → Fe(NO3)3(s) d) Fe3+(aq) + 3 OH- (aq) → Fe(OH)3(s) e) Na+ (aq) + NO3 - (aq) → NaNO3(s)

d) Fe3+(aq) + 3 OH- (aq) → Fe(OH)3(s)

What is the net ionic equation for the reaction of potassium hydroxide and hydrochloric acid? a) H+ (aq) + KOH(aq) → H2O(l) + K+ (aq) b) K+ (aq) + Cl- (aq) → KCl(aq) c) HCl(aq) + KOH(aq) → H2O(l) d) H+ (aq) + OH- (aq) → H2O(l) e) KOH(aq) + H2O(l) → H+ (aq) + K(OH)2(s)

d) H+ (aq) + OH- (aq) → H2O(l)

Which of the following compounds are strong acids: HClO4, H3PO4, H2SO4, CH3CO2H, and HSO4 - ? a) H2SO4 and CH3CO2H b) H2SO4 and HSO4 - c) HClO4, H3PO4, and H2SO4 d) HClO4 and H2SO4 e) all of the above

d) HClO4 and H2SO4

Classify the reaction below. FeCl3(aq) + 3 NaOH(aq) → Fe(OH)3(s) + 3 NaCl(aq) a) gas forming b) oxidation-reduction c) acid-base d) precipitation e) decomposition

d) precipitation

. What is the oxidation number of phosphorus in CaHPO4? a) -3 b) -1 c) +1 d) +3 e) +5

e) +5

. What is the oxidation number of manganese in KMnO4? a) -2 b) 0 c) +3 d) +5 e) +7

e) +7

Potassium hydrogen phthalate (KHP) is a weak acid that is used to standardize sodium hydroxide according to the net ionic equation below. HC8H4O4 - (aq) + OH- (aq) → H2O(l) + C8H4O4 2- (aq) If 1.4802 g KHP (molar mass = 204.2 g/mol) is titrated with 28.34 mL of NaOH, what is the concentration of NaOH? a) 0.03536 M b) 0.1385 M c) 0.2004 M d) 0.2176 M e) 0.2713 M

e) 0.2713 M

. If 4.39 g AlCl3 is dissolved in enough water to make exactly 100.0 mL of solution, what is the molar concentration of chloride ion? a) 0.0234 M b) 0.0934 M c) 0.110 M d) 0.132 M e) 0.988 M

e) 0.988 M

If 0.1500 g of impure soda ash (Na2CO3) is titrated with 21.99 mL of 0.1043 M HCl, what is the percent purity of the soda ash? Na2CO3(aq) + 2 HCl(aq) → 2 NaCl(aq) + H2O(l) + CO2(g) a) 12.15% b) 16.21% c) 48.62% d) 73.94% e) 81.03%

e) 81.03%

What is the net ionic equation for the reaction below? AgNO3(aq) + KBr(aq) → AgBr(s) + KNO3(aq) a) K+ (aq) + NO3 - (aq) → KNO3(s) b) AgNO3(aq) + KBr(aq) → AgBr(s) c) K+ (aq) + NO3 - (aq) → KNO3(aq) d) AgNO3(aq) + KBr(aq) → AgBr(s) + KNO3(aq) e) Ag+ (aq) + Br- (aq) → AgBr(s)

e) Ag+ (aq) + Br- (aq) → AgBr(s)

Which compound in the reaction below undergoes reduction? SO2(g) + H2O(l) → H2SO3(aq) a) SO2 b) H2O c) H2SO3 d) both SO2 and H2O e) No compound is reduced.

e) No compound is reduced.

Which of the following compounds are likely to be insoluble in water: Na2CO3, AgNO3, ZnS, KOH, Cu(OH)2, and NH4Cl? a) ZnS and NH4Cl b) KOH and Cu(OH)2 c) AgNO3, Cu(OH)2, and NH4Cl d) Na2CO3, ZnS, and KOH e) ZnS and Cu(OH)2

e) ZnS and Cu(OH)2

All of the following statements about acids and bases are true EXCEPT a) bases turn litmus paper blue. b) reactions between strong acids and bases are called neutralization reactions. c) acids tend to taste sour. d) bases increase the concentration of hydroxide ion in water. e) acids are produced by the reduction of water.

e) acids are produced by the reduction of water.

Compounds whose aqueous solutions conduct electricity are called ________ .

electrolytes

A ________ agent loses electrons in an oxidation-reduction reaction.

reducing

The net ionic equation for the reaction of silver nitrate and sodium chloride is as follows. Ag+ (aq) + Cl- (aq) → AgCl(s) Sodium and nitrate ions are referred to as ________ ions because they are not involved in the reaction.

spectator

If 5.00 mL of 1.66 × 10-1 M HCl is diluted to exactly 250.0 L with water, what is the concentration of the resulting solution? a) 3.32 × 10-3 M b) 1.33 × 10-2 M c) 1.45 × 10-2 M d) 4.07 × 10-2 M e) 8.30 M

a) 3.32 × 10-3 M

Which statement about the reaction below is correct? K2SO4 + Ba(NO3)2 → BaSO4 + 2 KNO3 a) BaSO4 will precipitate. b) KNO3 will precipitate. c) Both BaSO4 and KNO3 will precipitate. d) Neither BaSO4 nor KNO3 will precipitate. e) No reaction will occur because K2SO4 is insoluble.

a) BaSO4 will precipitate.

Which compound in the reaction below undergoes oxidation? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) a) CH4 b) O2 c) CO2 d) H2O e) CH4 and CO2

a) CH4

A major use of calcium oxide (lime) is in pollution control at coal burning power plants. Which reaction below occurs in the smokestack of a power plant? a) CaO(s) + SO3(g) → CaSO4(s) b) CaO(s) + SO3(g) → Ca(s) + SO2(g) + O2(g) c) CaO(s) + SO2(g) → CaS(s) + O2(g) d) 2 CaO(s) + C(s) → Ca2C(s) + O2(g) e) CaO(s) + C(s) → CaCO(s)

a) CaO(s) + SO3(g) → CaSO4(s)

Which compound is the reducing agent in the reaction below? I - (aq) + ClO- (aq) → IO- (aq) + Cl- (aq) a) I- b) ClO- c) H2O d) IO- e) Cl

a) I

What is the oxidation of each atom in sodium hypochlorite, NaClO? a) Na = +1, Cl = +1, O = -2 b) Na = -1, Cl = +3, O = -2 c) Na = +1, Cl = +1, O = +2 d) Na = -1, Cl = -1, O = +2 e) Na = +1, Cl = -1, O = 0

a) Na = +1, Cl = +1, O = -2

A precipitate will form when an aqueous solution of Ba(NO3)2 is added to an aqueous solution of ________. a) Na2SO4 b) AgNO3 c) KI d) Ca(ClO4)2 e) HCl

a) Na2SO4

A hydrochloric acid solution has a pH of 3.50. How many grams of HCl are present in 1.0 L of this solution? a) 3.2 × 10-4 g b) 0.012 g c) 0.096 g d) 3.5 g e) 87 g

b) 0.012 g

All of the following are oxidation-reduction reactions EXCEPT a) H2(g) + Cl2(g) → 2 HCl(g) b) C6H12O6(s) → 6 C(s) + 6 H2O(l) c) Ca(s) + 2 HBr(aq) → CaBr2(aq) + H2(g) d) 2 NaBr(aq) + F2(g) → 2 NaF(aq) + Br2(g) e) 2 H2O(l) → 2 H2(g) + O2(g)

b) C6H12O6(s) → 6 C(s) + 6 H2O(l)

Which of the following directions correctly describe the preparation of 0.500 L of 0.150 M NaOH from a 6.00 M stock solution? a) Dilute 0.200 L of 6.00 M NaOH to a volume of 0.500 L. b) Dilute 12.5 mL of 6.00 M NaOH to a volume of 0.500 L. c) Combine 0.200 L of 6.00 M NaOH with 0.500 L of water. d) Dilute 475 mL of 6.00 M NaOH to a volume of 0.500 L. e) Combine 12.5 mL of 6.00 M NaOH with 0.500 L of water

b) Dilute 12.5 mL of 6.00 M NaOH to a volume of 0.500 L.

Which of the following compounds is a weak acid? a) HCl b) HF c) HBr d) HNO3 e) HClO4

b) HF

Which of the following elements is a reducing agent? a) O2 b) K c) N2 d) F2 e) Ne

b) K

Which of the following compounds is a weak base? a) LiOH b) NH3 c) CH3CO2H d) Ba(OH)2 e) KCl

b) NH3

A precipitate will form when an aqueous solution of iron(III) chloride is added to ________. a) Ca(NO3)2 b) NaOH c) HCl d) NaCH3CO2 e) KClO4

b) NaOH

Sulfuric acid is the product of the reaction of ________ and H2O. a) SO2 b) SO3 c) SO3 2- d) SO4 - e) SO4 2-

b) SO3

Which of the following compounds are likely to be soluble in water: Ni(OH)2, ZnCl2, CuS, Fe2(CO3)3, AgCl, and Pb(NO3)2? a) ZnCl2 b) ZnCl2 and Pb(NO3)2 c) CuS and AgCl d) Fe2(CO3)3 and Ni(OH)2 e) none of the compounds are soluble

b) ZnCl2 and Pb(NO3)2