Deck 15: Complex Ion and Precipitation Equilibria

Question 1

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

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)

Answer 1

Ni(OH)₂(s) ? Ni²⁺(aq)+ 2OH?(aq)

Question 2

Consider the equilibrium of Ca(OH)₂(s)in water. Ca(OH)₂(s) ? Ca²⁺(aq)+ 2OH?(aq), What is the effect of raising the pH of the solution?

A) Ca²⁺(aq)is reduced to Ca(s).
B) The concentration of hydronium ion increases.
C) The concentration of Ca²⁺ increases as Ca(OH)₂ dissolves.
D) Ca(OH)₂(s)precipitates until equilibrium is reestablished.
E) Hydroxide ion is reduced to H₂(g).

Answer 2

Ca(OH)₂(s)precipitates until equilibrium is reestablished.

Question 3

For AgCl,K_sp = 1.8 × 10−¹⁰.What will occur if 250 mL of 1.5 × 10−³ M NaCl is mixed with 250 mL of 2.0 × 10−⁷ M AgNO₃?

A) Q > K_sp.A precipitate will form.
B) K_sp > Q.A precipitate will form.
C) Q = K_sp.No precipitate will form.
D) Q > K_sp.No precipitate will form.
E) K_sp > Q.No precipitate will form.

Answer 3

K_sp > Q.No precipitate will form.

Question 4

The K_sp of aluminum hydroxide,Al(OH)₃,is 2 × 10−³¹.What pH is required to limit the Al³⁺ concentration to less than or equal to 1 × 10−¹⁰ M?

A) 3.6
B) 6.4
C) 7.1
D) 7.8
E) 11.5

Question 5

Which of the following equations is the solubility product of Cu(II)hydroxide,Cu(OH)₂?

A)
$K_{\mathrm{sp}}=\frac{\left[\mathrm{Cu}(\mathrm{OH})_{2}\right]}{\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}}$
B)
$K_{\mathrm{sp}}=\frac{\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}}{\left[\mathrm{Cu}(\mathrm{OH})_{2}\right]}$
C)
$K_{\mathrm{sp}}=\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]$
D)
$K_{s p}=\left[\mathrm{Cu}^{2+}\right]^{2}\left[\mathrm{OH}^{-}\right]$
E)
$K_{\mathrm{sp}}=\left[\mathrm{Cu}^{2+}\right]\left[\mathrm{OH}^{-}\right]^{2}$

Question 6

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25°C.What mass of BaSO₄ (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25°C?

A) 2.6 × 10−⁸ g
B) 4.5 × 10−⁸ g
C) 1.0 × 10−⁵ g
D) 1.6 × 10−⁴ g
E) 2.4 × 10−³ g

Question 7

Which of the following equations represents the formation constant of Ti(NH₃)₆³⁺?

A) Ti³⁺(aq)+ (NH₃)₆(aq) ? Ti(NH₃)₆³⁺(aq)
B) Ti(NH₃)₆³⁺(aq) ? Ti³⁺(aq)+ 6NH₃(aq)
C) Ti³⁺(aq)+ NH₃(aq) ? Ti(NH₃)³⁺(aq)
D) 6Ti³⁺(aq)+ 6NH₃(aq) ? Ti(NH₃)₆³⁺(aq)
E) Ti³⁺(aq)+ 6NH₃(aq) ? Ti(NH₃)₆³⁺(aq)

Question 8

Consider the equilibrium of magnesium fluoride,MgF₂(s),in water. MgF₂(s) ? Mg²⁺(aq)+ 2F?(aq), What is the effect of adding perchloric acid (i.e.decreasing the pH of solution)?

A) The acid will have no effect on the magnesium fluoride equilibrium.
B) The F? will be protonated,resulting in more MgF₂(s)dissolving.
C) More MgF₂(s)will be formed,thus reducing Mg²⁺ and F? concentrations in solution.
D) Magnesium perchlorate,Mg(ClO₄)₂(s),will precipitate.
E) Magnesium hydride,MgH₂(s),will precipitate.

Question 9

The K_sp of calcium phosphate is 1 × 10−³³.What is the concentration of Ca²⁺ in equilibrium with Ca₃(PO₄)₂(s)if [PO₄³⁻] = 1 × 10−⁵ M?

A) 1 × 10−²⁸ M
B) 1 × 10−²³ M
C) 1 × 10−¹¹ M
D) 5 × 10−¹⁰ M
E) 2 × 10−⁸ M

Question 10

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?

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 11

What is the equilibrium constant expression for the dissolution of solid lead oxalate,PbC₂O₄,in water?

A) $K_{s p}=\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\right]$
B) K_sp = [Pb]² [C₂O₄]²
C) $K_{\mathrm{sp}}=\frac{\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\right]}{\left[\mathrm{PbC}_{2} \mathrm{O}_{4}\right]}$
D) $K_{\mathrm{sp}}=\frac{\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{C}^{4+}\right]^{2}\left[\mathrm{O}^{2-}\right]^{4}}{\left[\mathrm{PbC}_{2} \mathrm{O}_{4}\right]}$
E) $K_{\mathrm{sp}}=\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{C}_{2}\right]\left[\mathrm{O}_{4}^{2-}\right]$

Question 12

What is the chemical equation that describes the dissolution of calcium iodate in water?

A) CaI₂(s) ? Ca²⁺(aq)+ 2I?(aq)
B) Ca²⁺(aq)+ IO₃?(aq) ? CaIO₃(s)
C) Ca(IO₃)₂(s) ? Ca(s)+ I₂(aq)+ 3O₂(g)
D) Ca(IO₃)₂(s) ? Ca²⁺(aq)+ 2IO₃?(aq)
E) Ca(IO₃)₂(s) ? CaI₂(aq)+ 3O₂(g)

Question 13

Consider the equilibrium of lead sulfide,PbS,in water. PbS(s) ? Pb²⁺(aq)+ S^2?(aq), What is the effect of adding PbS(s)to the solution?

A) The PbS(s)has no effect on the system.
B) More Pb²⁺ and S^2? will form.
C) More Pb²⁺ will form,but the concentration of S^2? will remain constant.
D) More S^2? will form,but the concentration of Pb²⁺ will remain constant.
E) The concentrations of Pb²⁺ and S^2? will decrease.

Question 14

The formation constant for Ag(CN)₂−(aq)is 2 × 10²⁰.At what cyanide ion concentration is [Ag⁺] = [ Ag(CN)₂−]?

A) 3 × 10−⁴¹ M
B) 5 × 10−²¹ M
C) 7 × 10−¹¹ M
D) 6 × 10−⁶ M
E) 1 × 10¹⁰ M

Question 15

The K_sp of Fe(OH)₃(s)is 3 × 10−³⁹.What concentration of Fe³⁺ can exist in solution at pH 3.0?

A) 3 × 10−⁴ M
B) 3 × 10−⁶ M
C) 3 × 10−²¹ M
D) 3 × 10−²⁴ M
E) 3 × 10−³⁰ M

Question 16

K_sp stands for

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

Question 17

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

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

Question 18

The K_sp of calcium iodate is 7.1 × 10−⁷.What is the concentration of Ca²⁺ in equilibrium with Ca(IO₃)₂(s)if [IO₃−] = 3.3 × 10−² M?

A) 3.3 × 10−⁷ M
B) 2.2 × 10−⁵ M
C) 8.1 × 10−⁵ M
D) 6.5 × 10−⁴ M
E) 7.1 × 10−³ M

Question 19

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?

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 20

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

A) K_sp = [Ca²⁺][F?]
B) K_sp = [Ca²⁺]²[F?]
C) K_sp = [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 21

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

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

Question 22

What is the water solubility of PbI₂ (K_sp = 8.4 × 10−⁹,MM = 461 g/mol)in moles per liter?

A) 8.4 × 10−⁹ M
B) 1.9 × 10−⁷ M
C) 9.1 × 10−⁵ M
D) 1.3 × 10−³ M
E) 2.0 × 10−³ M

Question 23

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

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 24

The solubility of BaCrO₄(s)in water is 3.7 milligrams in 1.0 L at 25°C.What is the value of K_sp for BaCrO₄?

A) 2.1 × 10^-10
B) 8.6 × 10^-10
C) 1.4 × 10^-5
D) 1.5 × 10^-5
E) 2.9 × 10^-5

Question 25

For PbCl₂,K_sp = 1.7 × 10−⁵.What will occur if 250 mL of 0.12 M Pb(NO₃)₂ is mixed with 250 mL of 0.070 M NaCl?

A) Q > K_sp.A precipitate will form.
B) K_sp > Q.A precipitate will form.
C) Q = K_sp.No precipitate will form.
D) Q > K_sp.No precipitate will form.
E) K_sp > Q.No precipitate will form.

Question 26

What volume of water is needed to completely dissolve 1.0 g of Ag₂CrO₄ (K_sp = 8.0 × 10−¹²,MM = 331.8 g/mol)?

A) 0.94 L
B) 1.1 L
C) 1.7 L
D) 24 L
E) 2.6 × 10⁵ L

Question 27

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

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

Question 28

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?

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

Question 29

What is the water solubility of Hg₂Br₂ (K_sp = 6 × 10−²³)in moles per liter?

A) 8 × 10−¹² M
B) 1 × 10−⁸ M
C) 2 × 10−⁸ M
D) 4 × 10−⁸ M
E) 3 × 10−⁶ M

Question 30

What is the water solubility of AgCl (K_sp = 1.8 × 10−¹⁰)in 0.25 M NaCl?

A) 4.5 × 10−¹¹ M
B) 7.2 × 10−¹⁰ M
C) 1.8 × 10−⁹ M
D) 1.7 × 10−⁷ M
E) 1.3 × 10−⁵ M

Question 31

The K_sp of BaSO₄ is 1.1 × 10^-10 at 25°C.What mass of BaSO₄ (molar mass = 233.4 g/mol)will dissolve in 1.0 L of water at 25°C?

A) 2.6 × 10−⁸ g
B) 4.5 × 10−⁸ g
C) 1.0 × 10−⁵ g
D) 1.6 × 10−⁴ g
E) 2.4 × 10−³ g

Question 32

What is the water solubility of AgI (K_sp = 1 × 10−¹⁶,MM = 234.8 g/mol)in moles per liter?

A) 1 × 10−³² M
B) 1 × 10−¹⁶ M
C) 1 × 10−⁸ M
D) 2 × 10−⁶ M
E) 4 × 10−1¹ M

Question 33

For Ca(OH)₂,K_sp = 4.0 × 10−⁶.What will occur if 1.0 L of 0.100 M Ca(NO₃)₂ is prepared in a solution that is buffered at pH 12.50?

A) Q > K_sp.A precipitate will form.
B) K_sp > Q.A precipitate will form.
C) Q = K_sp.No precipitate will form.
D) Q > K_sp.No precipitate will form.
E) K_sp > Q.No precipitate will form.

Question 34

What is the concentration of Ag⁺ in a saturated solution of Ag₂CrO₄ if K_sp = 1 × 10−¹²?

A) 1 × 10−¹² M
B) 5 × 10−⁵ M
C) 6 × 10−⁵ M
D) 1 × 10−⁴ M
E) 2 × 10−⁴ M

Question 35

A saturated solution of lead(II)sulfate can be prepared by diluting 0.0101 g of PbSO₄ to 250 mL.What is the K_sp of lead(II)sulfate?

A) 8.3 × 10−¹²
B) 1.6 × 10−⁹
C) 1.8 × 10−⁸
D) 4.5 × 10−⁸
E) 8.4 × 10−⁷

Question 36

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

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 37

What is the water solubility of BaF₂(s)in 0.033 M KF(aq)at 25°C? The K_sp of BaF₂ is 1.8 × 10^-7 at 25°C.

A) 2.7 × 10^-6 M
B) 5.5 × 10^-6 M
C) 4.1 × 10^-5 M
D) 1.1 × 10^-4 M
E) 1.7 × 10^-4 M

Question 38

For Mg(OH)₂,K_sp = 6 × 10−¹².What will occur if 1.0 L of 0.010 M Mg(NO₃)₂ is prepared at pH 10.00?

A) Q > K_sp.A precipitate will form.
B) K_sp > Q.A precipitate will form.
C) Q = K_sp.No precipitate will form.
D) Q > K_sp.No precipitate will form.
E) K_sp > Q.No precipitate will form.

Question 39

What is the water solubility of AgCl (K_sp = 1.8 × 10−¹⁰,MM = 143.4 g/mol)in grams per liter?

A) 1.3 × 10−¹² g/L
B) 2.6 × 10−⁸ g/L
C) 9.4 × 10−⁸ g/L
D) 9.6 × 10−⁴ g/L
E) 1.9 × 10−³ g/L

Question 40

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)?

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 41

Determine the equilibrium constant,K,for the following reaction, Ca(OH)₂(s)+ 2H⁺(aq)→ Ca²⁺(aq)+ 2H₂O(l)
Given the K_sp of Ca(OH)₂ is 4.0 × 10−⁶ and K_w is 1.0 × 10−^-14.

A) 4.0 × 10²⁰
B) 4.0 × 10⁶
C) 1.0 × 10¹⁴
D) 2.5 × 10⁹
E) 4.0 × 1022

Question 42

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

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 43

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.

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 44

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.

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

Question 45

What is the net ionic equation for the reaction of Ca₃(PO₄)₂ with a strong acid?

A) Ca₃(PO₄)₂(s)+ 6H⁺(aq)→ 3CaH₃(s)+ 2PO₄³⁻(aq)
B) Ca₃(PO₄)₂(s)+ 6H⁺(aq)→ 3Ca²⁺(aq)+ 2H₃PO₄(aq)
C) 2PO₄³⁻(aq)+ 2H⁺(aq)→ H₂PO₄−(aq)
D) 3Ca²⁺(aq)+ 2PO₄³⁻(aq)+ 6H⁺(aq)→ 2H₃PO₄(aq)+ 3Ca²⁺(aq)
E) Ca₃(PO₄)₂(s)+ 16H⁺(aq)→ Ca₃P₂(s)+ 8H₂O(l)

Question 46

In the qualitative analysis scheme,Mg²⁺ is a group IV cation.What anion is used to precipitate Mg²⁺?

A) OH−
B) Cl−
C) PO₄³⁻
D) S²⁻
E) CO₃²⁻

Question 47

Which of the boxes below represents solid MX₂ in equilibrium with M²⁺ (squares)and X− (circles)?

A)
B)
C)
D)
E)

Question 48

An aqueous solution contains 0.010 M Br^- and 0.010 M I^-.If Ag⁺ is added until AgBr(s)just begins to precipitate,what are the concentrations of Ag⁺ and I^-? (K_sp of AgBr = 5.4 × 10^-13,K_sp of AgI = 8.5 × 10^-17)

A) [Ag⁺] = 5.4 × 10^-11 M,[I^-] = 1.0 × 10^-2 M
B) [Ag⁺] = 8.5 × 10^-15 M,[I^-] = 1.0 × 10^-2 M
C) [Ag⁺] = 5.4 × 10^-11 M,[I^-] = 1.6 × 10^-6 M
D) [Ag⁺] = 8.5 × 10^-15 M,[I^-] = 6.4 × 10¹ M
E) [Ag⁺] = 8.5 × 10^-15 M,[I^-] = 1.6 × 10^-6 M

Question 49

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

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

Question 50

Consider the reaction Cu(OH)₂(s)+ 4NH₃(aq) ? Cu(NH₃)₄²⁺(aq)+ 2OH?(aq)
K = 4 × 10?⁷
If the K_f for Cu(NH₃)₄²⁺ is 1 × 10¹²,what is the value of K_sp for Cu(OH)₂?

A) 4 × 10?¹⁹
B) 2 × 10?¹³
C) 5 × 10?¹²
D) 4 × 10?⁷
E) 4 × 10⁵

Question 51

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?

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

Question 52

Which of the following metals will precipitate as chloride salts: Ag⁺,Pb²⁺,Ca²⁺,K⁺,and Cu²⁺?

A) Ag⁺
B) Pb²⁺,Ca²⁺,and Cu²⁺
C) Ag⁺,K⁺,and Cu²⁺
D) Ag⁺ and Pb²⁺
E) Ca²⁺ and Cu²⁺

Question 53

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)

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

Question 54

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 a precipitate.What group of cations is present?

A) Group I
B) Group II
C) Group III
D) Group IV
E) Group V

Question 55

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?

A)
B)
C)
D)
E)

Question 56

A solution contains 0.10 M Ca²⁺ and 0.10 M Mg²⁺.The pH of the solution is raised without changing the volume of the solution.What percentage of Mg²⁺ remains in solution when Ca(OH)₂(s)first begins to precipitate? (K_sp of Ca(OH)₂ = 4.0 × 10−⁶ and K_sp of Mg(OH)₂ = 7.1 × 10−¹²)

A) 1.8 × 10−⁴ %
B) 4.0 × 10−⁴ %
C) 6.3 × 10−³ %
D) 7.2 × 10−³ %
E) 1.4 × 10−² %

Question 57

What is the net ionic equation for the reaction of ZnS with a strong acid?

A) ZnS(s)+ 2H⁺(aq)→ Zn²⁺(aq)+ H₂S(aq)
B) Zn²⁺(aq)+ 2H⁺(aq)→ ZnH₂(aq)
C) S²⁻(aq)+ 2H⁺(aq)→ H₂S(aq)
D) S²⁻(aq)+ 2H⁺(aq)→ H₂S(s)
E) No reaction will occur.

Question 58

What is the net ionic equation for the reaction of KCl with a strong base?

A) KCl(s)+ OH−(aq)→ KOH(aq)+ Cl−(aq)
B) KCl(aq)+ OH−(aq)→ KOH(aq)+ Cl−(aq)
C) K⁺(aq)+ OH−(aq)→ KOH(s)
D) Cl−(aq)+ OH−(aq)→ HOCl(aq)
E) No reaction will occur.

Question 59

What is the net ionic equation for the reaction of an aqueous solution of AgNO₃ and NH₃?

A) AgNO₃(s)+ NH₃(aq)→ AgNH₃(s)+ NO₃−(aq)
B) Ag⁺(aq)+ NH₃(aq)→ AgNH₃(s)
C) Ag⁺(aq)+ 2NH₃(aq)→ Ag(NH₃)₂⁺(aq)
D) AgNO₃(s)+ 2NH₃(aq)→ Ag(NH₃)₂⁺(aq)+ NO₃−(aq)
E) No reaction will occur.