Question 1

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO₃)₂.Which statement is correct? [K_sp(Ca(OH)₂)= 6.5 × 10^-6]

Accepted Answer

First, we need to write out the balanced chemical equation for the reaction between KOH and Ca(NO3)2:

Ca(NO3)2 + 2KOH → Ca(OH)2 + 2KNO3

From the equation, we can see that for every mole of KOH added, one mole of Ca(OH)2 will be formed.

The initial concentration of Ca(NO3)2 is 0.0010 M, which is much lower than the solubility of Ca(OH)2 (6.5 × 10-6 M). This means that Ca(NO3)2 is unsaturated and there is no precipitate present.

When 0.015 mol of KOH is added, it will react with 0.015 mol of Ca(NO3)2 to form 0.015 mol of Ca(OH)2. This will increase the concentration of Ca(OH)2 in the solution to 0.015 M, which is still below the solubility of Ca(OH)2. Therefore, there will be no precipitate and the solution will remain unsaturated.

Option B is the correct choice.

Question 2

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L.What is K_sp for this compound?

Accepted Answer

The solubility product constant expression for magnesium carbonate, MgCO3(s), in aqueous solution is: MgCO3(s) ↔ Mg2+(aq) + CO32-(aq) The equilibrium expression for this dissolution reaction is: K_sp = [Mg2+][CO32-] Let x be the molar solubility of magnesium carbonate, then: [Mg2+] = x mol/L [CO32-] = x mol/L Substituting the values of [Mg2+] and [CO32-] into the Ksp expression gives: K_sp = x * x = x^2 Substituting the given value of the molar solubility (1.8 × 10^-4 mol/L) gives: K_sp = (1.8 × 10^-4)2 K_sp = 3.24 × 10^-8 Therefore, the correct answer is D) 3.2 × 10^-8.

Question 3

mL of 0.150 M KI? [K_sp(PbI₂)=1.4 × 10^-8]

Accepted Answer

The solubility product expression for PbI2 is Ksp = [Pb2+][I-]^2. Given Ksp = 1.4 × 10^-8, and assuming [I-] = 0.150 M, solve for [Pb2+]. [Pb2+] = Ksp / [I-]^2 = 1.4 × 10^-8 / (0.150)^2 = 6.2 × 10^-7 M.

Question 4

The solubility of lead(II)chloride is 0.45 g/100 mL of solution.What is the K_sp of PbCl₂?

Accepted Answer

The solubility product (Ksp) of PbCl2 can be calculated using its solubility and the dissociation equation PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq). Given the solubility is 0.45 g/100 mL, first convert this to moles/L (molarity, M) using the molar mass of PbCl2 (207.2 + 35.45*2 = 278.1 g/mol). Solubility in moles/L = 0.45 g / 278.1 g/mol / 0.1 L = 1.62 × 10^-2 M. For each mole of PbCl2 that dissolves, 1 mole of Pb2+ and 2 moles of Cl- are produced. Therefore, [Pb2+] = 1.62 × 10^-2 M and [Cl-] = 2 * 1.62 × 10^-2 M = 3.24 × 10^-2 M. Ksp = [Pb2+][Cl-]^2 = (1.62 × 10^-2)(3.24 × 10^-2)^2 = 1.7 × 10^-5.

Question 5

Calculate the solubility of silver oxalate,Ag₂C₂ O₄,in pure water. [K_sp(Ag₂C₂O₄)= 1.0 × 10^-11]

Accepted Answer

Ksp = [Ag+]^2[C2O42-] = 1.0 × 10^-11Let the solubility of Ag2C2O4 be x M. Then, [Ag+] = 2x M and [C2O42-] = x M.Substituting these values into the Ksp expression, we get:(2x)^2(x) = 1.0 × 10^-114x^3 = 1.0 × 10^-11x^3 = 2.5 × 10^-12x = 1.4 × 10^-4 M

Question 6

Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10^-3 M MgCl₂ are added to 500.0 mL of 1.2 × 10^-3 M NaF? [K_sp (MgF₂)= 6.9 × 10^-9]

Accepted Answer

To determine if a precipitate of magnesium fluoride will form, we need to calculate the ion product of magnesium fluoride, Q, and compare it to the solubility product constant, Ksp.

The balanced chemical equation for the reaction is:

Mg2+(aq) + 2F-(aq) → MgF2(s)

The initial concentrations of Mg2+ and F- ions are:

[Mg2+] = 1.1 × 10^-3 M
[F-] = 1.2 × 10^-3 M

Using the stoichiometry of the balanced equation, we can see that the concentration of Mg2+ ions is in excess:

[Mg2+]excess = [Mg2+] - 0 = 1.1 × 10^-3 M

Therefore, the maximum amount of MgF2 that could possibly form is limited by the concentration of F- ions remaining. Assume that x is the molar solubility of MgF2 in water. Then:

[Mg2+] = x M
[F-] = 1.2 × 10^-3 M - 2x M

The ion product Q is:

Q = [Mg2+][F-]^2 = x(1.2 × 10^-3 - 2x)^2

Substituting the values given, we get:

Q = (1.1 × 10^-3)(1.2 × 10^-3)^2 = 1.584 × 10^-9

Comparing Q to the solubility product constant Ksp:

Ksp = 6.9 × 10^-9

We see that Q < Ksp. This means that MgF2 will not precipitate out of solution since there is still room for more MgF2 to dissolve. Therefore, the answer is B.

Question 7

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution.What is the K_sp for Mg₃(P O₄)₂?

Accepted Answer

The answer of The solubility of magnesium phosphate is 2.27...

Question 8

Will a precipitate (ppt)form when 300.0 mL of 5.0 × 10^-5M AgNO₃ are added to 200.0 mL of 2.5 × 10^-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Accepted Answer

When 5.0 × 10^-5 M AgNO3 is added to 2.5 × 10^-7 M NaBr, there is a possibility of Ag+ reacting with Br- to form AgBr, which has a low solubility and forms a precipitate. Therefore, a precipitate of AgBr will form in this case.

Question 9

Calculate the solubility of zinc hydroxide,Zn(OH)₂,in 1.00 M NaOH.K_sp = 3.0 × 10^-16 for Zn(OH)₂,K_f = 3.0 × 10¹⁵ for Zn(OH)₄^2-

Accepted Answer

The answer of Calculate the solubility of zinc hydroxide,Zn(OH)₂,in 1.00...

Question 10

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III)fluoride.[K_sp(CrF₃)= 6.6 × 10^-11]

Accepted Answer

To initiate precipitation, the ion product [Cr³⁺][F⁻]³ must equal the Ksp. Given [F⁻] = 0.095 M, solve for [Cr³⁺]: [Cr³⁺] = Ksp / [F⁻]³ = 6.6 × 10⁻¹¹ / (0.095)³ = 7.7 × 10⁻⁸ M.

Question 11

Which compound has the lowest solubility in pure water?

Accepted Answer

FePO4 has the lowest solubility product constant (Ksp) value, which indicates low solubility in water.

Question 12

Consider the dissolution of MnS in water.[K_sp(MnS)=3.0 × 10^-14] MnS(s)+ H₂O(l) Mn²⁺(aq)+ HS^-(aq)+ OH^-(aq) How is the solubility of manganese(II)sulfide affected by the addition of aqueous potassium hydroxide to the system?

Accepted Answer

When aqueous potassium hydroxide is added to the system, the hydroxide ions will react with the hydrogen sulfide ions produced from the reaction between water and the dissolved hydrogen sulfide gas. H2S + OH- --> HS- + H2O. This reaction will shift the equilibrium of the original dissolution reaction to the left, decreasing the amount of dissolved MnS and therefore decreasing its solubility.

Question 13

Write the ion product expression for calcium phosphate,Ca₃(P O₄)₂.

Accepted Answer

The answer of Write the ion product expression for calcium...

Question 14

Will a precipitate (ppt)form when 20.0 mL of 1.1 × 10^-3 M Ba(NO₃)₂ are added to 80.0 mL of 8.4 ×10^-4M Na₂CO₃?

Accepted Answer

BaCO₃ is insoluble in water and will precipitate when Ba²⁺ ions from Ba(NO₃)₂ react with CO₃²⁻ ions from Na₂CO₃.

Question 15

The molar solubility of tin(II)iodide is 1.28 × 10^-2 mol/L.What is K_sp for this compound?

Accepted Answer

The solubility product constant, $K_{sp}$, for tin(II) iodide, which dissociates into one tin(II) ion and two iodide ions in solution, can be calculated using the formula $K_{sp} = [Sn^{2+}][I^-]^2$. Given the molar solubility is $1.28 \times 10^{-2}$ mol/L, the concentration of $Sn^{2+}$ is $1.28 \times 10^{-2}$ mol/L, and the concentration of $I^-$ is $2 \times 1.28 \times 10^{-2} = 2.56 \times 10^{-2}$ mol/L. Thus, $K_{sp} = (1.28 \times 10^{-2})(2.56 \times 10^{-2})^2 = 8.39 \times 10^{-6}$.

Question 16

If 50.0 mL of 1.2 × 10^-3 M Pb(NO₃)₂ are added to 50.0 mL of 2.0 × 10^-4 M Na₂S,what takes place?

Accepted Answer

When the two solutions are mixed, Pb2+ ions will react with S2- ions from the Na2S solution to form a precipitate of PbS according to the following chemical equation:

Pb(NO3)2(aq) + Na2S(aq) → PbS(s) + 2NaNO3(aq)

Therefore, choice A is the correct answer. No other precipitates will form as the other ions do not have a suitable partner for precipitation.

Question 17

Which compound has the highest solubility in pure water?

Accepted Answer

The solubility of a compound in water is directly related to its solubility product constant (Ksp). The higher the Ksp value, the more soluble the compound is in water. Among the given options, PbCl2 has the highest Ksp value of 1.7 × 10^-5, indicating it has the highest solubility in pure water.

Question 18

The molar solubility of manganese(II)carbonate is 4.2 × 10^-6 M.What is K_sp for this compound?

Accepted Answer

The solubility product constant (Ksp) expression for the dissolution of manganese(II) carbonate is as follows:
MnCO3(s) ⇌ Mn2+(aq) + CO32-(aq)

The balanced chemical equation shows that 1 mole of solid MnCO3 produces 1 mole of Mn2+ and 1 mole of CO32- in solution. Therefore, at equilibrium, the concentration of Mn2+ and CO32- in solution is equal to the molar solubility of MnCO3:

[Mn2+] = [CO32-] = 4.2 × 10^-6 M

The Ksp expression is the product of the concentrations of the products raised to their stoichiometric coefficients, each raised to a power equal to its coefficient:
Ksp = [Mn2+][CO32-]

Substituting the equilibrium concentrations of Mn2+ and CO32- in terms of the molar solubility of MnCO3:
Ksp = (4.2 × 10^-6 M) × (4.2 × 10^-6 M) = 1.8 × 10^-11

Therefore, the answer is D, 1.8 × 10^-11.

Question 19

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[K_sp(MgF₂)= 6.9 × 10^-9] rev: 08_14_2014_QC_52437

Accepted Answer

The balanced chemical equation for the precipitation reaction is:

MgS1U1P12+S1S1P0 + 2NaF → MgFS1U1B12S1U1B0 + Na2S1U1B0

From the equation, we can see that one mole of MgS1U1P12+S1S1P0 reacts with two moles of NaF to form one mole of MgFS1U1B12S1U1B0.

Therefore, the number of moles of MgS1U1P12+S1S1P0 required to react with all the NaF present in the solution is:

(2 mol NaF / 1 mol MgS1U1P12+S1S1P0) x (0.10 mol NaF) = 0.20 mol MgS1U1P12+S1S1P0

The volume of the solution is not given, so we cannot calculate the exact concentration. However, we can calculate the minimum concentration of MgS1U1P12+S1S1P0 needed to provide 0.20 mol:

minimum concentration = (0.20 mol) / (1 L) = 0.20 M

Since this value is larger than all the given answer choices except E, the correct answer is E, 6.9 × 10S1U1P1-7S1S1P0 M.

Question 20

What is the ion product expression for magnesium fluoride,MgF₂?

Accepted Answer

The answer of What is the ion product expression for...

Quiz 17: Acid-Base Equilibria and Solubility Equilibria

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO₃) ₂.Which statement is correct? [K_sp(Ca(OH) ₂) = 6.5 × 10^-6]

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L.What is K_sp for this compound?

mL of 0.150 M KI? [K_sp(PbI₂) =1.4 × 10^-8]

The solubility of lead(II) chloride is 0.45 g/100 mL of solution.What is the K_sp of PbCl₂?

Calculate the solubility of silver oxalate,Ag₂C₂ O₄,in pure water. [K_sp(Ag₂C₂O₄) = 1.0 × 10^-11]

Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10^-3 M MgCl₂ are added to 500.0 mL of 1.2 × 10^-3 M NaF? [K_sp (MgF₂) = 6.9 × 10^-9]

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution.What is the K_sp for Mg₃(P O₄) ₂?

Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10^-5M AgNO₃ are added to 200.0 mL of 2.5 × 10^-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Calculate the solubility of zinc hydroxide,Zn(OH) ₂,in 1.00 M NaOH.K_sp = 3.0 × 10^-16 for Zn(OH) ₂,K_f = 3.0 × 10¹⁵ for Zn(OH) ₄^2-

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride.[K_sp(CrF₃) = 6.6 × 10^-11]

Which compound has the lowest solubility in pure water?

Consider the dissolution of MnS in water.[K_sp(MnS) =3.0 × 10^-14] MnS(s) + H₂O(l) Mn²⁺(aq) + HS^-(aq) + OH^-(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Write the ion product expression for calcium phosphate,Ca₃(P O₄) ₂.

Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10^-3 M Ba(NO₃) ₂ are added to 80.0 mL of 8.4 ×10^-4M Na₂CO₃?

The molar solubility of tin(II) iodide is 1.28 × 10^-2 mol/L.What is K_sp for this compound?

If 50.0 mL of 1.2 × 10^-3 M Pb(NO₃) ₂ are added to 50.0 mL of 2.0 × 10^-4 M Na₂S,what takes place?

Which compound has the highest solubility in pure water?

The molar solubility of manganese(II) carbonate is 4.2 × 10^-6 M.What is K_sp for this compound?

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[K_sp(MgF₂) = 6.9 × 10^-9] rev: 08_14_2014_QC_52437

What is the ion product expression for magnesium fluoride,MgF₂?

Quiz 17: Acid-Base Equilibria and Solubility Equilibria

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO3) 2.Which statement is correct? [Ksp(Ca(OH) 2) = 6.5 × 10-6]

The molar solubility of magnesium carbonate is 1.8 × 10-4 mol/L.What is Ksp for this compound?

mL of 0.150 M KI? [Ksp(PbI2) =1.4 × 10-8]

The solubility of lead(II) chloride is 0.45 g/100 mL of solution.What is the Ksp of PbCl2?

Calculate the solubility of silver oxalate,Ag2C2 O4,in pure water. [Ksp(Ag2C2O4) = 1.0 × 10-11]

Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10-3 M MgCl2 are added to 500.0 mL of 1.2 × 10-3 M NaF? [Ksp (MgF2) = 6.9 × 10-9]

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution.What is the Ksp for Mg3(P O4) 2?

Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10-5M AgNO3 are added to 200.0 mL of 2.5 × 10-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Calculate the solubility of zinc hydroxide,Zn(OH) 2,in 1.00 M NaOH.Ksp = 3.0 × 10-16 for Zn(OH) 2,Kf = 3.0 × 1015 for Zn(OH) 42-

Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride.[Ksp(CrF3) = 6.6 × 10-11]

Which compound has the lowest solubility in pure water?

Consider the dissolution of MnS in water.[Ksp(MnS) =3.0 × 10-14] MnS(s) + H2O(l) Mn2+(aq) + HS-(aq) + OH-(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Write the ion product expression for calcium phosphate,Ca3(P O4) 2.

Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10-3 M Ba(NO3) 2 are added to 80.0 mL of 8.4 ×10-4M Na2CO3?

The molar solubility of tin(II) iodide is 1.28 × 10-2 mol/L.What is Ksp for this compound?

If 50.0 mL of 1.2 × 10-3 M Pb(NO3) 2 are added to 50.0 mL of 2.0 × 10-4 M Na2S,what takes place?

Which compound has the highest solubility in pure water?

The molar solubility of manganese(II) carbonate is 4.2 × 10-6 M.What is Ksp for this compound?

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[Ksp(MgF2) = 6.9 × 10-9] rev: 08_14_2014_QC_52437

What is the ion product expression for magnesium fluoride,MgF2?

Suppose 0.015 mol of KOH is added to 1.00 L of 0.0010 M Ca(NO₃) ₂.Which statement is correct? [K_sp(Ca(OH) ₂) = 6.5 × 10^-6]

The molar solubility of magnesium carbonate is 1.8 × 10^-4 mol/L.What is K_sp for this compound?

mL of 0.150 M KI? [K_sp(PbI₂) =1.4 × 10^-8]

The solubility of lead(II) chloride is 0.45 g/100 mL of solution.What is the K_sp of PbCl₂?

Calculate the solubility of silver oxalate,Ag₂C₂ O₄,in pure water. [K_sp(Ag₂C₂O₄) = 1.0 × 10^-11]

Does a precipitate of magnesium fluoride form if 300.0 mL of 1.1 × 10^-3 M MgCl₂ are added to 500.0 mL of 1.2 × 10^-3 M NaF? [K_sp (MgF₂) = 6.9 × 10^-9]

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution.What is the K_sp for Mg₃(P O₄) ₂?

Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10^-5M AgNO₃ are added to 200.0 mL of 2.5 × 10^-7M NaBr? Answer yes or no,and identify the precipitate if there is one.

Calculate the solubility of zinc hydroxide,Zn(OH) ₂,in 1.00 M NaOH.K_sp = 3.0 × 10^-16 for Zn(OH) ₂,K_f = 3.0 × 10¹⁵ for Zn(OH) ₄^2-

Calculate the minimum concentration of Cr³⁺ that must be added to 0.095 M NaF in order to initiate a precipitate of chromium(III) fluoride.[K_sp(CrF₃) = 6.6 × 10^-11]

Consider the dissolution of MnS in water.[K_sp(MnS) =3.0 × 10^-14] MnS(s) + H₂O(l) Mn²⁺(aq) + HS^-(aq) + OH^-(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Write the ion product expression for calcium phosphate,Ca₃(P O₄) ₂.

Will a precipitate (ppt) form when 20.0 mL of 1.1 × 10^-3 M Ba(NO₃) ₂ are added to 80.0 mL of 8.4 ×10^-4M Na₂CO₃?

The molar solubility of tin(II) iodide is 1.28 × 10^-2 mol/L.What is K_sp for this compound?

If 50.0 mL of 1.2 × 10^-3 M Pb(NO₃) ₂ are added to 50.0 mL of 2.0 × 10^-4 M Na₂S,what takes place?

The molar solubility of manganese(II) carbonate is 4.2 × 10^-6 M.What is K_sp for this compound?

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride.[K_sp(MgF₂) = 6.9 × 10^-9] rev: 08_14_2014_QC_52437

What is the ion product expression for magnesium fluoride,MgF₂?