Question 1

Write the solubility product constant expression for the following salt: Na₂CO₃.

Accepted Answer

The solubility product constant expression for the salt Na₂CO₃ is given by [Na⁺]₂[CO₃^2-]. Option D is the only choice that matches this expression without any additional terms or coefficients.

Question 2

Choose the compound that is most soluble in water.

Accepted Answer

Potassium sulfide (K2S) is the most soluble in water among the given options because it is an ionic compound with potassium, which is an alkali metal, and alkali metal compounds are generally highly soluble in water. The other compounds contain sulfides of metals that are typically insoluble in water.

Question 3

At a temperature for which the solubility product constant of calcium carbonate is 4.7 × 10^-9, what mass of the salt will dissolve in 100 mL of water?

Accepted Answer

The solubility product constant for calcium carbonate is given by:Ksp = [Ca2+][CO32-] = 4.7 × 10^-9Let x be the molar solubility of calcium carbonate in mol/L. Then, the concentration of calcium ions and carbonate ions in solution will also be x mol/L.Substituting these values into the Ksp expression, we get:4.7 × 10^-9 = x^2Solving for x, we get:x = 2.17 × 10^-5 mol/LThe mass of calcium carbonate that will dissolve in 100 mL of water is:mass = moles × molar massmass = (2.17 × 10^-5 mol/L) × (100.1 g/mol) × (100 mL/1 L)mass = 0.69 mgTherefore, the correct answer is A) 0.69 mg.

Question 4

Equal volumes of 0.020 M Ag⁺ solution and 2.0 M NH₃ solution are mixed. Kf for [Ag(NH₃)₂]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10^-22.

Accepted Answer

The answer of Equal volumes of 0.020 M Ag⁺ solution...

Question 5

The solubility product constant of PbI2 is 7.1 × 10^-9. How many moles of PbI2 will precipitate if 250 ml of a 0.200 M solution of NaI are added to 150 ml of 0.100 M solution of Pb(NO₃)₂? You may neglect hydrolysis.

Accepted Answer

The answer of The solubility product constant of PbI2 is...

Question 6

What is the concentration of Ca²⁺ in ppm (mg/L) in cave water saturated with calcite (calcium carbonate, Ksp = 4.7 × 10^-9)?

Accepted Answer

The answer of What is the concentration of Ca²⁺ in...

Question 7

What is the composition of the precipitate formed when H₂S gas is bubbled through 1.0 litre of a solution of 0.010 M Zn²⁺, 0.010 M Pb²⁺, and 0.010 M Mn²⁺, buffered at pH 2.0, until 0.10 mol of H2S has been added? [Ksp values are: ZnS: 1.6 × 10^-23; MnS: 7.0 × 10^-16; PbS: 7.0 × 10^-29. For H₂S, Ka1 = 1.0 × 10^-7; Ka₂ = 1.3 × 10^-13.

Accepted Answer

The correct answer is E.The concentration of H2S in the solution is:[H2S] = 0.10 mol / 1.0 L = 0.10 MThe concentration of HS- in the solution is:[HS-] = [H2S] * Ka1 / [H+] = 0.10 M * 1.0 × 10-7 / 10-2 = 1.0 × 10-6 MThe concentration of S2- in the solution is:[S2-] = [H2S] * Ka1 * Ka2 / [H+]2 = 0.10 M * 1.0 × 10-7 * 1.3 × 10-13 / 10-4 = 1.3 × 10-16 MThe concentration of Zn2+ in the solution is:[Zn2+] = 0.010 MThe concentration of Pb2+ in the solution is:[Pb2+] = 0.010 MThe concentration of Mn2+ in the solution is:[Mn2+] = 0.010 MThe Qsp for ZnS is:Qsp = [Zn2+][S2-] = 1.0 × 10-6 M * 1.3 × 10-16 M = 1.3 × 10-22The Qsp for MnS is:Qsp = [Mn2+][S2-] = 1.0 × 10-6 M * 1.3 × 10-16 M = 1.3 × 10-22The Qsp for PbS is:Qsp = [Pb2+][S2-] = 1.0 × 10-6 M * 1.3 × 10-16 M = 1.3 × 10-22Since Qsp > Ksp for all three metal sulfides, all three metal sulfides will precipitate out of solution.

Question 8

What molar concentration of silver ion could exist in a solution in which the concentration of CrO₄^2- is 1.0 × 10^-4 M? (Ksp of Ag₂CrO₄ = 1.1 × 10^-12)

Accepted Answer

The answer of What molar concentration of silver ion could...

Question 9

Write the solubility product constant expression for the following salt: Ag₂SO₄.

Accepted Answer

The solubility product constant expression for the salt Ag₂SO₄ is given by [Ag⁺]2[SO₄^2-]. This expression is obtained by multiplying the concentrations of the ions in the equilibrium expression, with the coefficient of each ion being the same as its stoichiometric coefficient in the balanced chemical equation for the dissolution of the salt. The correct choice is B, where the expression is squared, since there are two Ag⁺ ions for every unit of the salt that dissolves.

Question 10

Write the solubility product constant for KAl(SO₄)₂(s)?

Accepted Answer

The answer of Write the solubility product constant for KAl(SO₄)₂(s)? ...

Question 11

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag⁺(aq)? (Ksp for AgX(s) = 5.2 × 10^-17; Kf for Ag(CN)^2- = 5.6 × 10¹⁸)

Accepted Answer

The correct answer is A because the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag+(aq) is 3.1 × 10-3 M. This can be calculated using the following equation:Ksp = [Ag+][X-]Kf = [Ag(CN)2-]/[Ag+][CN-]2[Ag(CN)2-] = Kf[Ag+][CN-]2[CN-] = sqrt(Ksp/[Kf][Ag+][X-])[CN-] = sqrt(5.2 × 10-17/[5.6 × 1018][0.0184][0.149])[CN-] = 3.1 × 10-3 M

Question 12

Write the solubility product constant expression for the following salt: Ca₃(PO₄)₂.

Accepted Answer

The solubility product constant expression for Ca₃(PO₄)₂ is [Ca²⁺]³[PO₄^3-]².

Question 13

Equal volumes of a 0.020 M Zn²⁺ solution and a 2.0 M NH₃ solution are mixed. Kf for [Zn(NH₃)₄]²⁺ is 4.1 × 10⁸. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC₂O₄ precipitate? What is Q? Ksp ZnC₂O₄= 2.7 × 10^-8

Accepted Answer

The balanced equation for the dissolution of ZnS in water is:

ZnS(s) ⇌ Zn2+(aq) + S2-(aq)

The solubility product expression for ZnS is:

Ksp = [Zn2+][S2-]

When the ZnS solution is mixed with the NHSB solution, the following reaction occurs:

ZnS + 2NHSB ⇌ [Zn(NHSB)2] + H2S

The equilibrium constant expression for this reaction is:

K = [Zn(NHSB)2]/[ZnS][NHSB]2

We can relate K to Ksp using the formation constant Kf for [Zn(NHSB)S]:

Kf = [Zn(NHSB)S]/[Zn2+][NHSB]

Rearranging the expression for Kf and substituting it into the equilibrium constant expression K, we get:

K = [Zn(NHSB)S]/Kf

Substituting the given values, we get:

K = (0.020 M)(2.0 M)2/4.1 × 10^-18 M = 1.91 × 10^13

When enough sodium oxalate is added to make the solution 0.10 M in oxalate, it reacts with the Zn2+ ions to form the complex ion [Zn(C2O4)4]2-. The reaction is:

Zn2+ + 4C2O42- ⇌ [Zn(C2O4)4]2-

The equilibrium constant expression for this reaction is:

K = [Zn(C2O4)4]2-/([Zn2+][C2O42-]^4)

The value of K can be calculated from the given Ksp for ZnC2O4 and the solubility product expression:

K = Ksp/([Zn2+][C2O42-]^4)

Substituting the given values, we get:

K = 2.7 × 10^-18/([Zn2+][C2O42-]^4)

At equilibrium, Q = K. Therefore,

K = Q = [Zn(NHSB)S][Zn2+][NHSB]/([ZnS][NHSB]2)

Substituting the given values, we get:

1.91 × 10^13 = [Zn(NHSB)S][Zn2+]/([ZnS][NHSB])

Assuming that the volumes of the solutions are equal, the initial concentration of Zn2+ is [Zn2+] = 0.020 M. The concentration of NHSB is 2.0 M, and the concentration of oxalate after addition of the sodium oxalate is 0.10 M. Therefore,

[Zn(NHSB)S] = [Zn(NHSB)S]eq = Kf[Zn2+][NHSB]/([NHSB] + [C2O42-])

Substituting the given values, we get:

[Zn(NHSB)S]eq = (4.1 × 10^-18 M)(0.020 M)(2.0 M)/0.10 M = 8.2 × 10^-17 M

Substituting these values into the equation for K, we get:

1.91 × 10^13 = (8.2 × 10^-17 M)[Zn2+]/(0.020 M)

Solving for [Zn2+], we get:

[Zn2+] = 7.8 × 10^-6 M

Substituting this value into the solubility product expression for ZnC2O4 and solving for Q, we get:

Q = [Zn2+][C2O42-]^4 = (7.8 × 10^-6 M)(0.10 M)^4 = 2.9 × 10^-12

Since Q is greater than Ksp, ZnC2O4 will precipitate. Therefore, the answer is C.

Question 14

Write the solubility product constant expression for the following salt: Ca(OH)₂.

Accepted Answer

The solubility product expression for Ca(OH)₂ is Ksp = [Ca²⁺][OH⁻]², reflecting the dissociation into one Ca²⁺ ion and two OH⁻ ions.

Question 15

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10^-25 TlBr 3.4 × 10^-6 AgCl 1.8 × 10^-10 FeS 6 × 10^-19 CuI 1.1 × 10^-12

Accepted Answer

The compound with the lowest Ksp value is the least soluble. In this case, ZnS has the lowest Ksp value of 2 × 10^-25, indicating that it is the least soluble of the five compounds listed.

Question 16

When 200 mL of 0.10 M BaCl₂ is added to 100 mL of 0.30 M Na₂SO₄, the number of moles of BaSO₄ (solubility product = 1.1 × 10^-10) precipitated is ________.

Accepted Answer

The correct answer is A.The number of moles of BaSO4 precipitated can be calculated using the solubility product constant and the concentrations of the reactants. The solubility product constant for BaSO4 is 1.1 × 10^-10. The concentration of Ba2+ in the solution is 0.10 M and the concentration of SO42- in the solution is 0.30 M. The reaction between Ba2+ and SO42- is:Ba2+ + SO42- → BaSO4The number of moles of BaSO4 precipitated can be calculated using the following equation:Ksp = [Ba2+][SO42-]1.1 × 10^-10 = (0.10 M)(0.30 M)[BaSO4] = 3.7 × 10^-9 MThe number of moles of BaSO4 precipitated is:moles of BaSO4 = (3.7 × 10^-9 M)(0.200 L) = 0.020 mol

Question 17

Write the solubility product constant expression for the following salt: PbC₂O₄.

Accepted Answer

The solubility product constant expression for PbC₂O₄ is [Pb²⁺][C₂O₄^2-]. This is because the salt dissociates into one Pb²⁺ ion and one C₂O₄^2- ion.

Question 18

The relationship between the molar concentration of silver ion in a saturated solution of silver phosphate and the solubility product constant for silver phosphate is ________.

Accepted Answer

The answer of The relationship between the molar concentration of...

Question 19

The molar solubility of calcium phosphate in a saturated aqueous solution of the salt is given by ________.

Accepted Answer

The answer of The molar solubility of calcium phosphate in...

Question 20

Write the solubility product constant expression for the following salt: CoS.

Accepted Answer

The solubility product constant expression for CoS is Ksp=[Co2+][S2-]. CoS does not have any charges, so there is no need to differentiate between different oxidation states of cobalt or sulfur, as shown in choices A, B, D, and E. Choice C correctly shows the product of the concentrations of Co2+ and S2-, which is the solubility product constant of CoS.

Quiz 18: Solubility and Complex-Ion Equilibria

Write the solubility product constant expression for the following salt: Na₂CO₃.

Choose the compound that is most soluble in water.

At a temperature for which the solubility product constant of calcium carbonate is 4.7 × 10^-9, what mass of the salt will dissolve in 100 mL of water?

Equal volumes of 0.020 M Ag⁺ solution and 2.0 M NH₃ solution are mixed. Kf for [Ag(NH₃) ₂]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10^-22.

The solubility product constant of PbI2 is 7.1 × 10^-9. How many moles of PbI2 will precipitate if 250 ml of a 0.200 M solution of NaI are added to 150 ml of 0.100 M solution of Pb(NO₃) ₂? You may neglect hydrolysis.

What is the concentration of Ca²⁺ in ppm (mg/L) in cave water saturated with calcite (calcium carbonate, Ksp = 4.7 × 10^-9) ?

What molar concentration of silver ion could exist in a solution in which the concentration of CrO₄^2- is 1.0 × 10^-4 M? (Ksp of Ag₂CrO₄ = 1.1 × 10^-12)

Write the solubility product constant expression for the following salt: Ag₂SO₄.

Write the solubility product constant for KAl(SO₄) ₂(s) ?

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag⁺(aq) ? (Ksp for AgX(s) = 5.2 × 10^-17; Kf for Ag(CN) ^2- = 5.6 × 10¹⁸)

Write the solubility product constant expression for the following salt: Ca₃(PO₄) ₂.

Equal volumes of a 0.020 M Zn²⁺ solution and a 2.0 M NH₃ solution are mixed. Kf for [Zn(NH₃) ₄]²⁺ is 4.1 × 10⁸. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC₂O₄ precipitate? What is Q? Ksp ZnC₂O₄= 2.7 × 10^-8

Write the solubility product constant expression for the following salt: Ca(OH) ₂.

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10^-25 TlBr 3.4 × 10^-6 AgCl 1.8 × 10^-10 FeS 6 × 10^-19 CuI 1.1 × 10^-12

When 200 mL of 0.10 M BaCl₂ is added to 100 mL of 0.30 M Na₂SO₄, the number of moles of BaSO₄ (solubility product = 1.1 × 10^-10) precipitated is ________.

Write the solubility product constant expression for the following salt: PbC₂O₄.

The relationship between the molar concentration of silver ion in a saturated solution of silver phosphate and the solubility product constant for silver phosphate is ________.

The molar solubility of calcium phosphate in a saturated aqueous solution of the salt is given by ________.

Write the solubility product constant expression for the following salt: CoS.

Quiz 18: Solubility and Complex-Ion Equilibria

Write the solubility product constant expression for the following salt: Na2CO3.

Choose the compound that is most soluble in water.

At a temperature for which the solubility product constant of calcium carbonate is 4.7 × 10-9, what mass of the salt will dissolve in 100 mL of water?

Equal volumes of 0.020 M Ag+ solution and 2.0 M NH3 solution are mixed. Kf for [Ag(NH3) 2]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10-22.

The solubility product constant of PbI2 is 7.1 × 10-9. How many moles of PbI2 will precipitate if 250 ml of a 0.200 M solution of NaI are added to 150 ml of 0.100 M solution of Pb(NO3) 2? You may neglect hydrolysis.

What is the concentration of Ca2+ in ppm (mg/L) in cave water saturated with calcite (calcium carbonate, Ksp = 4.7 × 10-9) ?

What molar concentration of silver ion could exist in a solution in which the concentration of CrO42- is 1.0 × 10-4 M? (Ksp of Ag2CrO4 = 1.1 × 10-12)

Write the solubility product constant expression for the following salt: Ag2SO4.

Write the solubility product constant for KAl(SO4) 2(s) ?

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag+(aq) ? (Ksp for AgX(s) = 5.2 × 10-17; Kf for Ag(CN) 2- = 5.6 × 1018)

Write the solubility product constant expression for the following salt: Ca3(PO4) 2.

Equal volumes of a 0.020 M Zn2+ solution and a 2.0 M NH3 solution are mixed. Kf for [Zn(NH3) 4]2+ is 4.1 × 108. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC2O4 precipitate? What is Q? Ksp ZnC2O4 = 2.7 × 10-8

Write the solubility product constant expression for the following salt: Ca(OH) 2.

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10-25 TlBr 3.4 × 10-6 AgCl 1.8 × 10-10 FeS 6 × 10-19 CuI 1.1 × 10-12

When 200 mL of 0.10 M BaCl2 is added to 100 mL of 0.30 M Na2SO4, the number of moles of BaSO4 (solubility product = 1.1 × 10-10) precipitated is ________.

Write the solubility product constant expression for the following salt: PbC2O4.

The relationship between the molar concentration of silver ion in a saturated solution of silver phosphate and the solubility product constant for silver phosphate is ________.

The molar solubility of calcium phosphate in a saturated aqueous solution of the salt is given by ________.

Write the solubility product constant expression for the following salt: CoS.

Write the solubility product constant expression for the following salt: Na₂CO₃.

At a temperature for which the solubility product constant of calcium carbonate is 4.7 × 10^-9, what mass of the salt will dissolve in 100 mL of water?

Equal volumes of 0.020 M Ag⁺ solution and 2.0 M NH₃ solution are mixed. Kf for [Ag(NH₃) ₂]+ is 1.6 × 107. If trisodium arsenate is added so that the arsenate ion concentration is 0.10 M, will silver arsenate precipitate? What is Q? Ksp for silver arsenate is 1.0 × 10^-22.

The solubility product constant of PbI2 is 7.1 × 10^-9. How many moles of PbI2 will precipitate if 250 ml of a 0.200 M solution of NaI are added to 150 ml of 0.100 M solution of Pb(NO₃) ₂? You may neglect hydrolysis.

What is the concentration of Ca²⁺ in ppm (mg/L) in cave water saturated with calcite (calcium carbonate, Ksp = 4.7 × 10^-9) ?

What molar concentration of silver ion could exist in a solution in which the concentration of CrO₄^2- is 1.0 × 10^-4 M? (Ksp of Ag₂CrO₄ = 1.1 × 10^-12)

Write the solubility product constant expression for the following salt: Ag₂SO₄.

Write the solubility product constant for KAl(SO₄) ₂(s) ?

What is the minimum concentration of CN- that will prevent the precipitation of AgX(s) from a solution that is 0.149 M in X-(aq) and 0.0184 M in Ag⁺(aq) ? (Ksp for AgX(s) = 5.2 × 10^-17; Kf for Ag(CN) ^2- = 5.6 × 10¹⁸)

Write the solubility product constant expression for the following salt: Ca₃(PO₄) ₂.

Equal volumes of a 0.020 M Zn²⁺ solution and a 2.0 M NH₃ solution are mixed. Kf for [Zn(NH₃) ₄]²⁺ is 4.1 × 10⁸. If enough sodium oxalate is added to make the solution 0.10 M in oxalate, will ZnC₂O₄ precipitate? What is Q? Ksp ZnC₂O₄= 2.7 × 10^-8

Write the solubility product constant expression for the following salt: Ca(OH) ₂.

The following table lists five compounds and their Ksp value. Which is least soluble? ZnS 2 × 10^-25 TlBr 3.4 × 10^-6 AgCl 1.8 × 10^-10 FeS 6 × 10^-19 CuI 1.1 × 10^-12

When 200 mL of 0.10 M BaCl₂ is added to 100 mL of 0.30 M Na₂SO₄, the number of moles of BaSO₄ (solubility product = 1.1 × 10^-10) precipitated is ________.

Write the solubility product constant expression for the following salt: PbC₂O₄.