Question 1

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

Accepted Answer

The correct chemical equation for the dissolution of nickel(II) hydroxide in water is Ni(OH)2(s) ⇌ Ni^2+(aq) + 2OH^-(aq), which matches choice A.

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?

Accepted Answer

Raising the pH of the solution increases the concentration of OH− ions, which shifts the equilibrium to the left, causing more Ca(OH)₂ to precipitate 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 × 10−⁷M AgNO₃?

Accepted Answer

E

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?

Accepted Answer

The equilibrium equation for the dissolution of aluminum hydroxide is: Al(OH)3 (s) ⇌ Al3+ (aq) + 3 OH- (aq) The solubility constant, K_sp, for this reaction is 2 × 10−³¹, which means that at equilibrium, the product of the concentrations of Al3+ and OH- ions is equal to 2 × 10−³¹. Let's assume that the initial concentration of Al3+ is zero, so the initial concentration of OH- is also zero. As aluminum hydroxide dissolves, the concentration of OH- ions increases, and Al3+ ions are produced in the process. At equilibrium, the concentration of Al3+ ions will be equal to the concentration of OH- ions produced. Let x be the concentration of OH- ions produced at equilibrium. Then the concentration of Al3+ ions will also be x, and we can write: Ksp = [Al3+][OH-]3 2 × 10−³¹ = x * x3 x4 = 2 × 10−³¹ x = (2 × 10−³¹)1/4 x = 6.31 × 10−³ The pH of a solution is defined as the negative logarithm of the concentration of H+ ions. In this case, we want to limit the concentration of Al3+ ions to less than or equal to 1 × 10−¹⁰ M, which means that the concentration of OH- ions should be at least 1 × 10−¹⁰ M. The concentration of H+ ions required to produce this concentration of OH- ions can be calculated from the following equation: Kw = [H+][OH-] 1.0 × 10−⁴¹ = x * 1.0 × 10−¹⁰ x = 1.0 × 10−⁴³ The pH required to limit the concentration of Al3+ ions to less than or equal to 1 × 10−¹⁰ M is: pH = -log[H+] pH = -log(1.0 × 10−⁴³) pH = 3.6 Therefore, the correct answer is choice (C).

Question 5

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

Accepted Answer

The solubility product ($K_{\mathrm{sp}}$) for a salt is the product of the concentrations of its ions, each raised to the power of its coefficient in the balanced dissolution equation. For Cu(OH)$_2$, the dissolution equation is $Cu(OH)_2(s) \rightarrow Cu^{2+}(aq) + 2OH^{-}(aq)$, so $K_{\mathrm{sp}} = [Cu^{2+}][OH^{-}]^2$.

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?

Accepted Answer

The answer of The K_sp of BaSO₄ is 1.1 ×...

Question 7

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

Accepted Answer

The formation constant equation for a complex ion typically shows the metal ion and the ligands combining to form the complex ion. Choice E correctly shows titanium ion and 6 ammonia molecules combining to form the complex ion, which matches the stoichiometry for the formation of such a complex.

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)?

Accepted Answer

Perchloric acid is a strong acid that will dissociate completely in water, increasing the concentration of H+ ions. The H+ ions will protonate the F- ions, forming HF. This will shift the equilibrium to the right, favoring the dissolution of more MgF2(s) in water, resulting in more Mg2+ and F- ions in solution. Therefore, the correct choice is B, more MgF2(s) will dissolve due to protonation of F-.

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?

Accepted Answer

The equilibrium constant for the dissolution of calcium phosphate is:

Ca3(PO4)2(s) ⇌ 3Ca2+(aq) + 2PO43-(aq)

KS1U1B1spS1U1B0 = [Ca2+]3[PO43-]2

KS1U1B1spS1U1B0 = 1 × 10−S1U1P133S1S1P0

We are given the concentration of [PO43-] and want to find [Ca2+] in equilibrium.

Let x be the concentration of Ca2+ in equilibrium.

Then according to the equilibrium constant expression:

KS1U1B1spS1U1B0 = x3(1 × 10−S1U1P133S1S1P0)2

x3 = KS1U1B1spS1U1B0 / (1 × 10−S1U1P133S1S1P0)2

x = (KS1U1B1spS1U1B0)1/3 / (1 × 10−S1U1P133S1S1P0)2/3

x = (1 × 10−S1U1P133S1S1P0)−S1U1P13S1U1B0/3

Now we can substitute the given values:

[Ca2+] = (1 × 10−S1U1P133S1S1P0)−S1U1P13S1U1B0/3 = 2 × 10−S1U1P18S1S1P0 M

Therefore, the answer is E: 2 × 10-S1U1P18S1S1P0 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?

Accepted Answer

Adding NaCl increases the concentration of Cl⁻ ions due to the common-ion effect, causing PbCl₂ to precipitate until equilibrium is reestablished.

Question 11

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

Accepted Answer

The equilibrium constant expression for the dissolution of a solid in water, known as the solubility product constant ($K_{sp}$), includes only the concentrations of the ions in solution. For lead oxalate, $PbC_2O_4$, which dissociates into $Pb^{2+}$ and $C_2O_4^{2-}$ ions in water, the correct expression is $K_{sp}=[Pb^{2+}][C_2O_4^{2-}]$.

Question 12

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

Accepted Answer

The correct chemical equation for the dissolution of calcium iodate in water should contain the products Ca2+ and IO3-. Choice D is the only one that includes these products in the aqueous state, along with the solid calcium iodate. The other choices either include incorrect products or reactants, or have products in the wrong state.

Question 13

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

Adding more PbS(s) will not have any effect on the system as the equilibrium is already established with the given concentration of Pb²⁺ and S²⁻. Therefore, the addition of PbS(s) will not shift the equilibrium in any direction.

Question 14

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

Accepted Answer

The formation constant Kf = [Ag(CN)2−]/([Ag+][CN−]^2). Given Kf = 2 × 10^20 and [Ag+] = [Ag(CN)2−], we have 2 × 10^20 = 1/([CN−]^2). Solving for [CN−], we get [CN−] = 7 × 10−11 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?

Accepted Answer

The dissociation reaction of Fe(OH)₃(s) is: Fe(OH)₃(s) ⇌ Fe³⁺(aq) + OH−(aq) The equilibrium constant for this reaction is the solubility product constant, K_sp, which is given as 3 × 10−³⁹. At pH 3.0, the hydroxide ion concentration is 10−¹¹ M. We can assume that the concentration of Fe³⁺ in solution is much less than the hydroxide ion concentration, so we can neglect the contribution of the Fe³⁺ to the overall pH. Therefore, using the equilibrium expression for the dissociation reaction, we get: K_sp = [Fe³⁺][OH−] 3 × 10−³⁹ = [Fe³⁺][10−¹¹] Solving for [Fe³⁺], we get: [Fe³⁺] = (3 × 10−³⁹) / (10−¹¹) [Fe³⁺] = 3 × 10−²⁸ M Therefore, the concentration of Fe³⁺ that can exist in solution at pH 3.0 is 3 × 10−²⁸ M, which corresponds to choice B.

Question 16

K_sp stands for

Accepted Answer

K_sp is a notation that stands for the solubility product, a constant for a given substance at a specific temperature that represents the product of the concentrations of the ions of a soluble salt in equilibrium with its solid form.

Question 17

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

Accepted Answer

The dissolution of silver oxalate in water involves the dissociation into two silver ions (Ag⁺) and one oxalate ion (C₂O₄²⁻).

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?

Accepted Answer

The given equilibrium reaction is: Ca(IO3)2 (s) ⇌ Ca2+ + 2 IO3- The equilibrium constant expression for the reaction is: K = [Ca2+][IO3-]^2 The value of the equilibrium constant, K_sp, is given as 7.1 × 10−⁷. To calculate the concentration of Ca2+ in equilibrium with Ca(IO3)2 (s), we need to first calculate the concentration of IO3- ions in the solution. Given: [IO3-] = 3.3 × 10−² M Let the concentration of Ca2+ ions in equilibrium be x M. Using the equilibrium constant expression, we can write: K = [Ca2+][IO3-]^2 7.1 × 10−⁷ = x(3.3 × 10−²)^2 x = 6.5 × 10−⁴ M Therefore, the concentration of Ca2+ in equilibrium with Ca(IO3)2 (s) is 6.5 × 10−⁴ M. The answer is choice D) 6.5 × 10−⁴ 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?

Accepted Answer

The solubility product expression for barium chromate is Ksp = [Ba²⁺][CrO₄²⁻]. Given Ksp = 1.2 × 10⁻¹⁰ and [CrO₄²⁻] = 4.3 × 10⁻³ M, solve for [Ba²⁺]: [Ba²⁺] = Ksp / [CrO₄²⁻] = (1.2 × 10⁻¹⁰) / (4.3 × 10⁻³) = 2.8 × 10⁻⁸ M.

Question 20

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

Accepted Answer

The correct expression for the dissolution of calcium fluoride, $CaF_2$, in water is given by the solubility product constant $K_{\mathrm{sp}}$, which is the product of the molar concentrations of the ions each raised to the power of its coefficient in the balanced equation. For $CaF_2$, the dissolution equation is $CaF_2(s) \rightarrow Ca^{2+}(aq) + 2F^{-}(aq)$, so $K_{\mathrm{sp}} = [Ca^{2+}][F^{-}]^2$. Solid calcium fluoride is not included in the expression because its concentration is considered constant and is incorporated into the equilibrium constant.

Quiz 15: Complex Ion and Precipitation Equilibria

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

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?

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 × 10−⁷M AgNO₃?

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?

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

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?

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

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) ?

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?

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

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

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?

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

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

K_sp stands for

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

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?

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?

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

Quiz 15: Complex Ion and Precipitation Equilibria

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

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?

For AgCl,Ksp = 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 × 10−7M AgNO3?

The Ksp 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?

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

The Ksp 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?

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

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) ?

The Ksp 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?

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

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

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?

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

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

Ksp stands for

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

The Ksp 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?

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?

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

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?

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 × 10−⁷M AgNO₃?

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?

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

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?

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

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) ?

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?

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

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?

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

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

K_sp stands for

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

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?

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?