Question 1

What is the concentration of Hg22+ in a saturated solution of Hg2Cl2 if Ksp = 1 × 10−18?

Accepted Answer

A)  1 × 10−9 M 
B)  2 × 10−9 M 
C)  3 × 10−7 M 
D)  6 × 10−7 M 
E)  1 × 10−6 M 
A)  1 × 10−9 M 
B)  2 × 10−9 M 
C)  3 × 10−7 M 
D)  6 × 10−7 M 
E)  1 × 10−6 M

Question 2

What is the water solubility of PbI2 (Ksp = 8.4 × 10−9)in 0.15 M KI?

Accepted Answer

A)  3.7 × 10−7 M 
B)  5.6 × 10−7 M 
C)  1.9 × 10−6 M 
D)  1.1 × 10−4 M 
E)  6.1 × 10−4 M 
A)  3.7 × 10−7 M 
B)  5.6 × 10−7 M 
C)  1.9 × 10−6 M 
D)  1.1 × 10−4 M 
E)  6.1 × 10−4 M

Question 3

What is the net ionic equation for the reaction of iron(III)hydroxide with a strong acid?

Accepted Answer

A)  3OH−(aq)+ 3H+(aq)→ 3H2O(l) 
B)  Fe3+(aq)+ 3OH−(aq)+ 3H+(aq)→ Fe3+(aq)+ 3H2O(l) 
C)  Fe(OH)3(s)+ 3H+(aq)→ Fe3+(aq)+ 3H2O(l) 
D)  Fe3+(aq)+ 3H+(aq)→ Fe3+(aq)+ 3H2O(l) 
E)  Fe(OH)3(s)+ 3H+(aq)→ FeH3(s)+ 3OH−(aq) 
A)  3OH−(aq)+ 3H+(aq)→ 3H2O(l) 
B)  Fe3+(aq)+ 3OH−(aq)+ 3H+(aq)→ Fe3+(aq)+ 3H2O(l) 
C)  Fe(OH)3(s)+ 3H+(aq)→ Fe3+(aq)+ 3H2O(l) 
D)  Fe3+(aq)+ 3H+(aq)→ Fe3+(aq)+ 3H2O(l) 
E)  Fe(OH)3(s)+ 3H+(aq)→ FeH3(s)+ 3OH−(aq)

Question 4

At pH 10.0,only 0.019 g of MgCl2 will dissolve per 1 L of solution.What is the Ksp of magnesium chloride,MgCl2?

Accepted Answer

A)  2 × 10−13 
B)  2 × 10−12 
C)  2 × 10−10 
D)  2 × 10−8 
E)  2 × 10−6 
A)  2 × 10−13 
B)  2 × 10−12 
C)  2 × 10−10 
D)  2 × 10−8 
E)  2 × 10−6

Question 5

What is the chemical equation that describes the dissolution of nickel(II)hydroxide in water?

Accepted Answer

A)  Ni(OH)2(s)  ? Ni2+(aq)+ 2OH?(aq) 
B)  Ni2+(aq)+ 3OH?(aq)  ? Ni(OH)2(s) 
C)  Ni2OH(s)+ H+(aq)  ? 2Ni+(aq)+ H2O(l) 
D)  Ni(OH)2(s)+ 2H+(aq)  ? Ni2+(aq)+ 2H2O(l) 
E)  Ni(OH)2(aq)+ H2O(l)  ? Ni(OH)3(s)+ H+(aq) 
A)  Ni(OH)2(s)  ? Ni2+(aq)+ 2OH?(aq) 
B)  Ni2+(aq)+ 3OH?(aq)  ? Ni(OH)2(s) 
C)  Ni2OH(s)+ H+(aq)  ? 2Ni+(aq)+ H2O(l) 
D)  Ni(OH)2(s)+ 2H+(aq)  ? Ni2+(aq)+ 2H2O(l) 
E)  Ni(OH)2(aq)+ H2O(l)  ? Ni(OH)3(s)+ H+(aq)

Question 6

Given the following reactions, AgBr(s)  ? Ag+(aq)+ Br-(aq)
Ksp = 5.4 × 10-13
Ag+(aq)+ 2 CN-(aq)  ? Ag(CN)2-(aq)
Kf = 1.2 × 1021
Determine the equilibrium constant for the reaction below.
AgBr(s)+ 2 CN-(aq)  ? Ag(CN)2-(aq)+ Br-(aq)

Accepted Answer

A)  4.5 × 10-34 
B)  1.5 × 10-9 
C)  6.5 × 108 
D)  1.2 × 1021 
E)  2.2 × 1033 
A)  4.5 × 10-34 
B)  1.5 × 10-9 
C)  6.5 × 108 
D)  1.2 × 1021 
E)  2.2 × 1033

Question 7

What is the molar solubility of Fe(OH)3(s)in a solution that is buffered at pH 2.50 at 25°C? The Ksp of Fe(OH)3 is 6.3 × 10-38 at 25°C.

Accepted Answer

A)  6.9 × 10-28 M 
B)  2.0 × 10-26 M 
C)  1.3 × 10-13 M 
D)  2.0 × 10-3 M 
E)  5.0 × 102 M 
A)  6.9 × 10-28 M 
B)  2.0 × 10-26 M 
C)  1.3 × 10-13 M 
D)  2.0 × 10-3 M 
E)  5.0 × 102 M

Question 8

The addition of an anion to dissolve one precipitate from a mixture of precipitates is known as _____ .

Accepted Answer

A)  solubility product 
B)  common ion effect 
C)  complex formation 
D)  solution formation 
E)  selective precipitation 
A)  solubility product 
B)  common ion effect 
C)  complex formation 
D)  solution formation 
E)  selective precipitation

Question 9

The Ksp of barium chromate is 1.2 × 10−10.What is the concentration of Ba2+ in equilibrium with BaCrO4(s)if [CrO42−] = 4.3 × 10−3 M?

Accepted Answer

A)  5.1 × 10−13 M 
B)  2.8 × 10−8 M 
C)  1.1 × 10−5 M 
D)  1.7 × 10−4 M 
E)  2.5 × 10−3 M 
A)  5.1 × 10−13 M 
B)  2.8 × 10−8 M 
C)  1.1 × 10−5 M 
D)  1.7 × 10−4 M 
E)  2.5 × 10−3 M

Question 10

The Ksp of Ca(OH)2 is 5.5 × 10-5 at 25°C.What is the concentration of OH-(aq)in a saturated solution of Ca(OH)2(aq)?

Accepted Answer

A)  1.9 × 10-3 M 
B)  7.4 × 10-3 M 
C)  2.4 × 10-2 M 
D)  4.0 × 10-2 M 
E)  4.8 × 10-2 M 
A)  1.9 × 10-3 M 
B)  7.4 × 10-3 M 
C)  2.4 × 10-2 M 
D)  4.0 × 10-2 M 
E)  4.8 × 10-2 M

Question 11

What is the equilibrium constant expression for the dissolution of solid calcium fluoride in water?

Accepted Answer

A)  Ksp = [Ca2+][F?] 
B)  Ksp = [Ca2+]2[F?] 
C)  Ksp = [Ca2+][F?]2 
D)  $K_{\mathrm{sp}}=\frac{\left[\mathrm{Ca}^{2+}\right]\left[\mathrm{F}^{-}\right]^{2}}{\left[\mathrm{CaF}_{2}\right]}$ 
E)  $K_{\mathrm{sp}}=\frac{\left[\mathrm{Ca}^{2+}\right]\left[\mathrm{F}^{-}\right]}{[\mathrm{CaF}]}$ 
A)  Ksp = [Ca2+][F?] 
B)  Ksp = [Ca2+]2[F?] 
C)  Ksp = [Ca2+][F?]2 
D)  $K_{\mathrm{sp}}=\frac{\left[\mathrm{Ca}^{2+}\right]\left[\mathrm{F}^{-}\right]^{2}}{\left[\mathrm{CaF}_{2}\right]}$ 
E)  $K_{\mathrm{sp}}=\frac{\left[\mathrm{Ca}^{2+}\right]\left[\mathrm{F}^{-}\right]}{[\mathrm{CaF}]}$

Question 12

Determine the equilibrium constant,K,for the following reaction, Mg(OH)2(s)+ 2H+(aq)→ Mg2+(aq)+ 2H2O(l)
Given the Ksp of Mg(OH)2 is 6 × 10−12 and Kw is 1.0 × 10−14.

Accepted Answer

A)  6 × 10−26 
B)  6 × 10−12 
C)  1 × 10−14 
D)  6 × 1016 
E)  2 × 10−3 
A)  6 × 10−26 
B)  6 × 10−12 
C)  1 × 10−14 
D)  6 × 1016 
E)  2 × 10−3

Question 13

Ksp stands for

Accepted Answer

A)  saturated precipitate.. 
B)  soluble precipitate. 
C)  soluble particle. 
D)  saturated precipitate. 
E)  solubility product. 
A)  saturated precipitate.. 
B)  soluble precipitate. 
C)  soluble particle. 
D)  saturated precipitate. 
E)  solubility product.

Question 14

A soluble ionic species,SX,is dissolved in water.An excess of slightly soluble solid,MX,is added to the solution.Which of the boxes below represents MX in equilibrium with M+ (squares)and X− (circles)in the presence of SX?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 15

Consider the equilibrium of PbCl2(s)in water. PbCl2(s)  ? Pb2+(aq)+ 2Cl?(aq), What is the effect of adding NaCl(aq)to the equilibrium solution?

Accepted Answer

A)  The sodium ion reduces the Pb2+ to Pb(s). 
B)  PbCl2 solubility increases due to the common-ion effect. 
C)  PbNa2(s)precipitates. 
D)  The NaCl(aq)has no effect on the system. 
E)  PbCl2(s)precipitates until equilibrium is reestablished. 
A)  The sodium ion reduces the Pb2+ to Pb(s). 
B)  PbCl2 solubility increases due to the common-ion effect. 
C)  PbNa2(s)precipitates. 
D)  The NaCl(aq)has no effect on the system. 
E)  PbCl2(s)precipitates until equilibrium is reestablished.

Question 16

What is the chemical equation that describes the dissolution of silver oxalate,Ag2(C2O4),in water?

Accepted Answer

A)  Ag2(C2O4)(s)  ? Ag22+(aq)+ C2O42?(aq) 
B)  Ag2(C2O4)(s)  ? 2Ag+(aq)+ C2O42?(aq) 
C)  Ag2(C2O4)(s)  ? Ag2+(aq)+ C2O4?(aq) 
D)  2Ag+(aq)+ C2O42?(aq)  ? Ag2(C2O4)(s) 
E)  Ag2+(aq)+ C2O4?(aq)  ? Ag2(C2O4)(s) 
A)  Ag2(C2O4)(s)  ? Ag22+(aq)+ C2O42?(aq) 
B)  Ag2(C2O4)(s)  ? 2Ag+(aq)+ C2O42?(aq) 
C)  Ag2(C2O4)(s)  ? Ag2+(aq)+ C2O4?(aq) 
D)  2Ag+(aq)+ C2O42?(aq)  ? Ag2(C2O4)(s) 
E)  Ag2+(aq)+ C2O4?(aq)  ? Ag2(C2O4)(s)

Question 17

What volume of water is needed to completely dissolve 100 g of AgBr (Ksp = 5 × 10−13,187.8 g/mol)?

Accepted Answer

A)  1 × 10−2 L 
B)  7 × 105 L 
C)  1 × 108 L 
D)  3 × 1010 L 
E)  1 × 1012 L 
A)  1 × 10−2 L 
B)  7 × 105 L 
C)  1 × 108 L 
D)  3 × 1010 L 
E)  1 × 1012 L

Question 18

Consider the equilibrium of lead sulfide,PbS,in water. PbS(s)  ? Pb2+(aq)+ S2?(aq), What is the effect of adding PbS(s)to the solution?

Accepted Answer

A)  The PbS(s)has no effect on the system. 
B)  More Pb2+ and S2? will form. 
C)  More Pb2+ will form,but the concentration of S2? will remain constant. 
D)  More S2? will form,but the concentration of Pb2+ will remain constant. 
E)  The concentrations of Pb2+ and S2? will decrease. 
A)  The PbS(s)has no effect on the system. 
B)  More Pb2+ and S2? will form. 
C)  More Pb2+ will form,but the concentration of S2? will remain constant. 
D)  More S2? will form,but the concentration of Pb2+ will remain constant. 
E)  The concentrations of Pb2+ and S2? will decrease.

Question 19

A solution containing an unknown metal ion is analyzed by qualitative analysis.Addition of chloride has no effect on the solution.Addition of H2S at pH 0.5 results in no precipitate.Addition of H2S at pH 9.0 results in no precipitate.What group(s)of cations may be present?

Accepted Answer

A)  Group I 
B)  Group II 
C)  Group III 
D)  Group IV 
E)  None of the groups 
A)  Group I 
B)  Group II 
C)  Group III 
D)  Group IV 
E)  None of the groups

Question 20

What is the water solubility of BaCO3 (Ksp = 2.6 × 10−9)in a solution containing 0.20 M CO32-(aq)?

Accepted Answer

A)  5.2 × 10−10 M 
B)  1.3 × 10−8 M 
C)  5.1 × 10−5 M 
D)  2.5 × 10−4 M 
E)  1.0 × 10−5 M 
A)  5.2 × 10−10 M 
B)  1.3 × 10−8 M 
C)  5.1 × 10−5 M 
D)  2.5 × 10−4 M 
E)  1.0 × 10−5 M

Exam 15: Complex Ion and Precipitation Equilibria

What is the concentration of Hg22+ in a saturated solution of Hg2Cl2 if Ksp = 1 × 10−18?

What is the water solubility of PbI2 (Ksp = 8.4 × 10−9)in 0.15 M KI?

What is the net ionic equation for the reaction of iron(III)hydroxide with a strong acid?

At pH 10.0,only 0.019 g of MgCl2 will dissolve per 1 L of solution.What is the Ksp of magnesium chloride,MgCl2?

What is the chemical equation that describes the dissolution of nickel(II)hydroxide in water?

Given the following reactions, AgBr(s) ? Ag+(aq)+ Br-(aq) Ksp = 5.4 × 10-13 Ag+(aq)+ 2 CN-(aq) ? Ag(CN)2-(aq) Kf = 1.2 × 1021 Determine the equilibrium constant for the reaction below. AgBr(s)+ 2 CN-(aq) ? Ag(CN)2-(aq)+ Br-(aq)

What is the molar solubility of Fe(OH)3(s)in a solution that is buffered at pH 2.50 at 25°C? The Ksp of Fe(OH)3 is 6.3 × 10-38 at 25°C.

The addition of an anion to dissolve one precipitate from a mixture of precipitates is known as _____ .

The Ksp of barium chromate is 1.2 × 10−10.What is the concentration of Ba2+ in equilibrium with BaCrO4(s)if [CrO42−] = 4.3 × 10−3 M?

The Ksp of Ca(OH)2 is 5.5 × 10-5 at 25°C.What is the concentration of OH-(aq)in a saturated solution of Ca(OH)2(aq)?

What is the equilibrium constant expression for the dissolution of solid calcium fluoride in water?

Determine the equilibrium constant,K,for the following reaction, Mg(OH)2(s)+ 2H+(aq)→ Mg2+(aq)+ 2H2O(l) Given the Ksp of Mg(OH)2 is 6 × 10−12 and Kw is 1.0 × 10−14.

Ksp stands for

A soluble ionic species,SX,is dissolved in water.An excess of slightly soluble solid,MX,is added to the solution.Which of the boxes below represents MX in equilibrium with M+ (squares)and X− (circles)in the presence of SX?

Consider the equilibrium of PbCl2(s)in water. PbCl2(s) ? Pb2+(aq)+ 2Cl?(aq), What is the effect of adding NaCl(aq)to the equilibrium solution?

What is the chemical equation that describes the dissolution of silver oxalate,Ag2(C2O4),in water?

What volume of water is needed to completely dissolve 100 g of AgBr (Ksp = 5 × 10−13,187.8 g/mol)?

Consider the equilibrium of lead sulfide,PbS,in water. PbS(s) ? Pb2+(aq)+ S2?(aq), What is the effect of adding PbS(s)to the solution?

A solution containing an unknown metal ion is analyzed by qualitative analysis.Addition of chloride has no effect on the solution.Addition of H2S at pH 0.5 results in no precipitate.Addition of H2S at pH 9.0 results in no precipitate.What group(s)of cations may be present?

What is the water solubility of BaCO3 (Ksp = 2.6 × 10−9)in a solution containing 0.20 M CO32-(aq)?

Matter and Measurements

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Mass Relations in Chemistry;stoichiometry

Reactions in Aqueous Solution

Gases

Electronic Structure and the Periodic Table

Covalent Bonding

Thermochemistry

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Gaseous Chemical Equilibrium

Acids and Bases

Equilibria in Acid-Base Solutions

Spontaneity of Reaction

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What is the concentration of Hg₂²⁺ in a saturated solution of Hg₂Cl₂ if K_sp = 1 × 10−¹⁸?

What is the water solubility of PbI₂ (K_sp = 8.4 × 10−⁹)in 0.15 M KI?

At pH 10.0,only 0.019 g of MgCl₂ will dissolve per 1 L of solution.What is the K_sp of magnesium chloride,MgCl₂?

Given the following reactions, AgBr(s) ? Ag⁺(aq)+ Br^-(aq) K_sp = 5.4 × 10^-13 Ag⁺(aq)+ 2 CN^-(aq) ? Ag(CN)₂^-(aq) K_f = 1.2 × 10²¹ Determine the equilibrium constant for the reaction below. AgBr(s)+ 2 CN^-(aq) ? Ag(CN)₂^-(aq)+ Br^-(aq)

What is the molar solubility of Fe(OH)₃(s)in a solution that is buffered at pH 2.50 at 25°C? The K_sp of Fe(OH)₃ is 6.3 × 10^-38 at 25°C.

The K_sp of barium chromate is 1.2 × 10−¹⁰.What is the concentration of Ba²⁺ in equilibrium with BaCrO₄(s)if [CrO₄²⁻] = 4.3 × 10−³ M?

The K_sp of Ca(OH)₂ is 5.5 × 10^-5 at 25°C.What is the concentration of OH^-(aq)in a saturated solution of Ca(OH)₂(aq)?

Determine the equilibrium constant,K,for the following reaction, Mg(OH)₂(s)+ 2H⁺(aq)→ Mg²⁺(aq)+ 2H₂O(l) Given the K_sp of Mg(OH)₂ is 6 × 10−¹² and K_w is 1.0 × 10−¹⁴.

K_sp stands for

A soluble ionic species,SX,is dissolved in water.An excess of slightly soluble solid,MX,is added to the solution.Which of the boxes below represents MX in equilibrium with M⁺ (squares)and X− (circles)in the presence of SX?

Consider the equilibrium of PbCl₂(s)in water. PbCl₂(s) ? Pb²⁺(aq)+ 2Cl?(aq), What is the effect of adding NaCl(aq)to the equilibrium solution?

What is the chemical equation that describes the dissolution of silver oxalate,Ag₂(C₂O₄),in water?

What volume of water is needed to completely dissolve 100 g of AgBr (K_sp = 5 × 10−¹³,187.8 g/mol)?

Consider the equilibrium of lead sulfide,PbS,in water. PbS(s) ? Pb²⁺(aq)+ S²^?(aq), What is the effect of adding PbS(s)to the solution?

A solution containing an unknown metal ion is analyzed by qualitative analysis.Addition of chloride has no effect on the solution.Addition of H₂S at pH 0.5 results in no precipitate.Addition of H₂S at pH 9.0 results in no precipitate.What group(s)of cations may be present?

What is the water solubility of BaCO₃ (K_sp = 2.6 × 10−⁹)in a solution containing 0.20 M CO₃^2-(aq)?