Question 1

What is the concentration of Pb²⁺ ions in a solution prepared by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI? [K_sp(PbI₂) =1.4 × 10^-8]

Accepted Answer

The concentration of Pb²⁺ ions is determined by the solubility product (K_sp) of PbI₂. The initial concentration of I^- from KI is high, which suppresses the dissolution of PbI₂. Using the K_sp expression and the initial I^- concentration, the concentration of Pb²⁺ is calculated to be 6.2 × 10^-7 M.

Question 2

Which compound has the lowest solubility in pure water?

Accepted Answer

The answer of Which compound has the lowest solubility in...

Question 3

Write the ion product expression for calcium phosphate, Ca₃(PO₄)₂.

Accepted Answer

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

Question 4

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 5

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

Accepted Answer

The ion product expression for magnesium fluoride, MgF2, is [Mg2+][F-]2. The given formula, MgF₂, indicates that there is one Mg2+ ion and two F- ions present in the compound, which matches the ion product expression for MgF2. Option B has the correct code and symbol for MgF2.

Question 6

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

KOH reacts with Ca(NO3)2 to form Ca(OH)2 and KNO3. However, the amount of KOH added is not enough to fully react with all the Ca(NO3)2 present in the solution, so the solution remains unsaturated and no precipitate forms. The concentration of calcium ions is not significantly affected by the addition of the small amount of KOH. The presence of KOH does not raise the solubility of Ca(NO3)2.

Question 7

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

Accepted Answer

When solutions of Pb(NO3)2 and Na2S are mixed, a precipitate of PbS (lead sulfide) forms due to the insolubility of PbS in water. This is a result of a double displacement reaction where the cation of one reactant (Pb2+) combines with the anion of the other reactant (S2-) to form an insoluble compound, PbS.

Question 8

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

Accepted Answer

BaCO3 (Barium Carbonate) is known to be insoluble in water, leading to the formation of a precipitate when solutions of Ba(NO3)2 and Na2CO3 are mixed.

Question 9

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

Accepted Answer

The solubility product constant, Ksp, is given as 1.0 × 10-11. The balanced equation for the dissociation of silver oxalate is:

Ag2C2O4 (s) ⇌ 2Ag+ (aq) + C2O42- (aq)

Since the dissociation of silver oxalate produces two Ag+ ions for every one unit of Ag2C2O4 that dissolves, we can express the solubility of silver oxalate as x mol/L, which will result in 2x mol/L of Ag+ and x mol/L of C2O42- in solution.

Substituting these values into the expression for Ksp, we get:

Ksp = [Ag+]2[C2O42-]
1.0 × 10-11 = (2x)2(x)
1.0 × 10-11 = 4x3

Solving for x gives:

x = 1.4 × 10-4 mol/L

Therefore, the solubility of silver oxalate in pure water is 1.4 × 10-4 mol/L. The correct answer is choice A.

Question 10

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution. What is the K_sp for Mg₃(PO₄)₂?

Accepted Answer

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

Question 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?

Accepted Answer

The addition of aqueous potassium hydroxide will increase the concentration of hydroxide ions in solution. These hydroxide ions will react with the dissolved hydrogen sulfide ions, causing a shift in the equilibrium towards the reactant side (Le Chatelier's principle). This will decrease the concentration of hydrogen sulfide ions in solution, decreasing the solubility of manganese(II) sulfide.

Question 12

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 13

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

Accepted Answer

Manganese(II) carbonate dissociates in water as follows:

MnCO3(s) ⇌ Mn2+(aq) + CO32-(aq)

The equilibrium expression for this reaction is:

Ksp = [Mn2+][CO32-]

We are given the molar solubility of manganese(II) carbonate, which is the number of moles of the compound that dissolve per liter of solution. Let x be the molar solubility of MnCO3. Then:

MnCO3(s) ⇌ Mn2+(aq) + CO32-(aq)
I         x           x

At equilibrium, the concentration of Mn2+ and CO32- ions is equal to x M. Therefore, we can substitute these values into the equilibrium expression and get:

Ksp = x^2

Substituting the given value of molar solubility into this equation gives:

Ksp = (4.2 × 10^-6)^2 = 1.764 × 10^-11

Because our answer must be expressed in scientific notation, we choose the closest value, D) 1.8 × 10^-11.

Question 14

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

Accepted Answer

The equilibrium reaction for the dissolution of magnesium carbonate is:

MgCO3(s) ⇌ Mg2+(aq) + CO32-(aq)

The solubility product constant, Ksp, is the product of the concentrations of the ions raised to their stoichiometric coefficients in the equilibrium equation. The stoichiometry of this equation is 1:1:1, so:

Ksp = [Mg2+][CO32-]

We are given the molar solubility of magnesium carbonate, which is the concentration of the dissolved Mg2+ and CO32- ions when the solution is at equilibrium with the solid magnesium carbonate:

[Mg2+] = [CO32-] = 1.8 × 10-4 mol/L

Substituting these values into the expression for Ksp gives:

Ksp = (1.8 × 10-4 mol/L)2 = 3.24 × 10-8 = 3.2 × 10-8 (to two significant figures)

Therefore, the answer is D: 3.2 × 10-8. The solubility product constant (Ksp) is calculated as the product of the concentrations of the constituent ions, each raised to the power of its stoichiometric coefficient in the balanced chemical equation for the dissolution of the compound.

The balanced equation for the dissolution of magnesium carbonate (MgCO3) is:

MgCO3(s) ⇌ Mg2+(aq) + CO32-(aq)

So, the Ksp expression for magnesium carbonate is:

Ksp = [Mg2+][CO32-]

We are given the molar solubility of magnesium carbonate, which is the concentration of the dissolved Mg2+ and CO32- ions at equilibrium. Since magnesium carbonate dissolves into one Mg2+ ion and one CO32- ion, the concentrations of these ions are equal to each other, and we can represent them as x.

Therefore, we can write:

[Mg2+] = [CO32-] = x

The molar solubility of magnesium carbonate is given as 1.8 × 10^-4 mol/L, so we can substitute this value for x:

[Mg2+] = [CO32-] = 1.8 × 10^-4 mol/L

Now, we can calculate Ksp:

Ksp = [Mg2+][CO32-] = (1.8 × 10^-4 mol/L)(1.8 × 10^-4 mol/L) = 3.24 × 10^-8

Rounding to the correct number of significant figures, the answer is D) 3.2 × 10^-8.

Question 15

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

Accepted Answer

When AgNO3 and NaBr are mixed, AgBr will precipitate out according to the following chemical equation: AgNO3 + NaBr → AgBr + NaNO3. The solubility product constant (Ksp) of AgBr is 7.7 x 10^-13 which indicates that it has a low solubility in water and therefore will precipitate out when the concentrations of Ag+ and Br- ions exceed the Ksp value. Since the concentrations given in the question exceed the Ksp value, a precipitate of AgBr will form.

Question 16

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

The balanced chemical equation for the precipitation reaction is:

CrS1U1P13+S1S1P0 + 3 NaFS1U1P1MS1S1P0 -> CrFS1U1B13S1U1B0 + 3 NaS1U1P10

The stoichiometric ratio between CrS1U1P13+S1S1P0 and NaFS1U1P1MS1S1P0 is 1:3. Therefore, if x is the minimum concentration of CrS1U1P13+S1S1P0 required to initiate the precipitation reaction, the concentration of NaFS1U1P1MS1S1P0 consumed will be 3x.

The solubility product constant for chromium(III) fluoride is given as:

KS1U1B1spS1U1B0(CrFS1U1B13S1U1B0) = 6.6 × 10S1U1P1-11S1S1P0

At equilibrium, the product of the ion concentrations of Cr3+ and F- should be equal to the solubility product constant. Let y be the concentration of F- ions that precipitate as CrFS1U1B13S1U1B0. Then, the equilibrium concentration of Cr3+ ions will also be y.

From the balanced equation, we know that the initial concentration of F- ions is 0.095 M. Assuming complete precipitation, the equilibrium concentration of F- ions will be (0.095 - 3x + y) M.

Substituting the equilibrium concentrations into the solubility product expression, we get:

( y )( 0.095 - 3x + y )3 = 6.6 × 10S1U1P1-11S1S1P0

Expanding and simplifying the equation yields a quadratic equation in y:

3yS1S1P2 - (0.285 - 9x)y + (0.095 - 3x)3.95 × 10S1U1P1-11 = 0

Using the quadratic formula, we can solve for y as:

y = [ (0.285 - 9x) ± sqrt( (0.285 - 9x)S1S1P2 - 4(3)(0.095 - 3x)(3.95 × 10S1U1P1-11) ) ] / (2(3))

To determine the minimum value of x, we need to find the value of x that makes y the smallest positive value. This occurs when the radical expression inside the square root is zero. Solving this equation for x gives:

(0.285 - 9x)S1S1P2 - 4(3)(0.095 - 3x)(3.95 × 10S1U1P1-11) = 0

Solving for x gives x = 7.7 × 10S1U1P1-8 M. Therefore, the answer is (C).

Question 17

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]

Accepted Answer

The answer of Calculate the minimum concentration of Mg²⁺ that...

Question 18

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

Given the solubility product constant (Ksp) for Zn(OH)2 is 3.0 × 10^-16 and the formation constant (Kf) for Zn(OH)4^2- is 3.0 × 10^15, we can calculate the solubility of Zn(OH)2 in 1.00 M NaOH. The reaction for the dissolution of Zn(OH)2 in excess OH^- (from NaOH) to form Zn(OH)4^2- is:Zn(OH)2(s) + 2OH^-(aq) → Zn(OH)4^2-(aq)The overall equilibrium constant (K) for this reaction can be found by multiplying Ksp for Zn(OH)2 and Kf for Zn(OH)4^2-, which gives K = Ksp * Kf = (3.0 × 10^-16) * (3.0 × 10^15) = 9.0 × 10^-1.Since the concentration of OH^- is fixed at 1.00 M, we can set up the equilibrium expression for the reaction as:K = [Zn(OH)4^2-] / [OH^-]^2Plugging in the values, we get:9.0 × 10^-1 = [Zn(OH)4^2-] / (1.00)^2Solving for [Zn(OH)4^2-], we find it to be 0.9 M. However, this is not the final answer because the question asks for the solubility of Zn(OH)2, not the concentration of Zn(OH)4^2-. The solubility of Zn(OH)2 is equivalent to the concentration of Zn(OH)4^2- formed, which is 0.9 M, but this does not match any of the provided options, indicating a mistake in the calculation process.The correct approach involves recognizing that the solubility of Zn(OH)2 in a solution of NaOH involves both the solubility product (Ksp) and the formation of the complex ion (Zn(OH)4^2-), but the calculation must correctly account for the concentration of OH^- ions and the formation constant to find the solubility in these conditions. The error in the explanation above is in the misinterpretation of how the Ksp and Kf values are used to calculate the solubility of Zn(OH)2 in a basic solution. The correct calculation involves more detailed steps that consider the specific interaction between Zn(OH)2 and the OH^- ions from NaOH, leading to the formation of Zn(OH)4^2- and correctly applying the equilibrium principles to find the solubility. The initial explanation incorrectly concludes with a concentration that is not among the options, suggesting a misunderstanding of the equilibrium process in this context.

Question 19

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 20

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^MNaF? [K_sp(MgF₂) = 6.9 × 10^-9]

Accepted Answer

The answer of Does a precipitate of magnesium fluoride form...

Quiz 17: Acid-Base Equilibria and Solubility Equilibria

What is the concentration of Pb²⁺ ions in a solution prepared by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI? [K_sp(PbI₂) =1.4 × 10^-8]

Which compound has the lowest solubility in pure water?

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

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

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]

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

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

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

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution. What is the K_sp for Mg₃(PO₄) ₂?

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?

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?

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

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

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]

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]

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-.

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

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^MNaF? [K_sp(MgF₂) = 6.9 × 10^-9]

Quiz 17: Acid-Base Equilibria and Solubility Equilibria

What is the concentration of Pb2+ ions in a solution prepared by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI? [Ksp(PbI2) =1.4 × 10-8]

Which compound has the lowest solubility in pure water?

Write the ion product expression for calcium phosphate, Ca3(PO4) 2.

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

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? [Ksp(Ca(OH) 2) = 6.5 × 10-6]

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?

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?

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

The solubility of magnesium phosphate is 2.27 × 10-3 g/1.0 L of solution. What is the Ksp for Mg3(PO4) 2?

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?

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?

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

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 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]

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]

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-.

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

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]

What is the concentration of Pb²⁺ ions in a solution prepared by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI? [K_sp(PbI₂) =1.4 × 10^-8]

Write the ion product expression for calcium phosphate, Ca₃(PO₄) ₂.

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

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]

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

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

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

The solubility of magnesium phosphate is 2.27 × 10^-3 g/1.0 L of solution. What is the K_sp for Mg₃(PO₄) ₂?

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?

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

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

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

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]

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]

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-.

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

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^MNaF? [K_sp(MgF₂) = 6.9 × 10^-9]