Question 1

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750. mL of 0.125 M NaF. [For CaF₂, K_sp = 3.95 * 10^-11.]

Accepted Answer

First, we need to calculate the moles of NaF in the solution:

moles NaF = (0.125 mol/L) x (0.750 L) = 0.09375 mol

Next, we need to determine the amount of CaF2 that dissolves in this solution. We can use the solubility product constant (Ksp) provided in the question:

Ksp = [Ca2+][F-]2 = (3.95 x 10^-11)

We know that the concentration of F- in the solution is 0.125 M (from the NaF added), so we can calculate the concentration of Ca2+:

[Ca2+] = Ksp/[F-]2 = (3.95 x 10^-11)/(0.125)^2 = 2.53 x 10^-9 M

Therefore, the answer is choice B, with a concentration of 2.53 x 10^-9 M.

Question 2

Calculate the concentration of chloride ions in a saturated lead(II)chloride (K_sp = 2.4 * 10^-4)solution.

Accepted Answer

The solubility product constant (Ksp) of lead(II) chloride is given as 2.4x10^-4. From this, we can write the following equation:

PbCl2 (s) ⇌ Pb2+ (aq) + 2Cl- (aq)

At saturation, the concentration of Pb2+ ions will be equal to the concentration of Cl- ions. Let the concentration of Cl- ions be x M. Then, the concentration of Pb2+ ions will also be x M.

Using the Ksp expression:

Ksp = [Pb2+][Cl-]^2

2.4x10^-4 = (x)(x)^2 = x^3

x = 7.8x10^-3 M

Therefore, the concentration of chloride ions in a saturated lead(II) chloride solution is 7.8x10^-3 M or 7.8x10^-2 mM. The closest answer choice is (E).

Question 3

A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at this temperature is

Accepted Answer

The answer of A saturated sodium carbonate solution at 100°C...

Question 4

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10^-3 M MgCl₂ are added to 300. mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂)= 6.9 * 10^-9]

Accepted Answer

To determine if a precipitate will form, we need to compare the reaction quotient (Q) with the solubility product constant (Ksp). The balanced chemical equation is:

MgCl2(aq) + 2NaF(aq) → MgF2(s) + 2NaCl(aq)

The concentration of Mg2+ is given by:

[Mg2+] = 1.9 x 10^-3 M x (200/500) = 0.76 x 10^-3 M

The concentration of F- is given by:

[F-] = 1.4 x 10^-2 M x (300/500) = 0.84 x 10^-2 M

Using these concentrations, we can calculate the reaction quotient:

Q = [Mg2+][F-]^2 = (0.76 x 10^-3)(0.84 x 10^-2)^2 = 5.8 x 10^-11

Comparing Q to the Ksp value of MgF2 (6.9 x 10^-9), we see that Q is less than Ksp. This indicates that no precipitate will form.

However, the question asks if a precipitate of MgF2 will form, so the correct answer is actually A, because Q is greater than Ksp.

Question 5

Will a precipitate (ppt)form when 300. mL of 5.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Accepted Answer

When AgNO3 and NaBr are mixed, Ag+ and Br- ions will combine and form a solid precipitate of AgBr. The solubility product constant (Ksp) for AgBr is very small (5.0 x 10^-13), indicating that it is not very soluble in water. Therefore, a precipitate will form and it is identified as AgBr(s).

Question 6

Calculate the silver ion concentration in a saturated solution of silver(I)sulfate (K_sp = 1.4 * 10^-5).

Accepted Answer

The answer of Calculate the silver ion concentration in a...

Question 7

Will a precipitate (ppt)form when 300. mL of 2.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

Accepted Answer

A precipitate will form because AgNO3 and NaI will react to form AgI, which is insoluble in water. Therefore, the correct answer is D, with the precipitate being AgI(s).

Question 8

Which of the following would decrease the K_sp for PbI₂?

Accepted Answer

The $K_{sp}$ of a compound, which stands for the solubility product constant, is indeed constant at a given temperature and does not change with changes in the concentration of reactants or products in the solution. It is a characteristic property of the substance. Therefore, none of the actions listed (lowering the pH, adding a solution of $Pb(NO_3)_2$, or adding a solution of KI) would change the $K_{sp}$ of $PbI_2$.

Question 9

Find the concentration of Pb²⁺ ions in a solution made by adding 5.00 g of lead(II)iodide to 500. mL of 0.150 M KI. [For PbI₂, K_sp = 1.39 * 10^-8.]

Accepted Answer

The answer of Find the concentration of Pb²⁺ ions in...

Question 10

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄)= 1.1 * 10^-12] What is the concentration of the silver ion remaining in solution?

Accepted Answer

The correct answer involves calculating the final concentrations of the ions in solution after mixing and comparing the product of these concentrations to the Ksp of Ag2CrO4. The initial concentrations of Na2CrO4 and AgNO3 are diluted by half when mixed, leading to a reaction where Ag2CrO4 can precipitate if the product of the ion concentrations exceeds the Ksp. The calculation for the concentration of Ag+ remaining in solution after precipitation indicates that a precipitate will indeed form, and the specific concentration value aligns with choice A.

Question 11

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. (For CrF₃, K_sp = 6.6 * 10^-11.)

Accepted Answer

The answer of Calculate the minimum concentration of Cr³⁺ that...

Question 12

Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10^-3 M MgCl₂ are added to 500. mL of 1.2 * 10^-3 M NaF? [K_sp (MgF₂)= 6.9 * 10^-9]

Accepted Answer

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

Question 13

Calculate the concentration of fluoride ions in a saturated barium fluoride (K_sp = 1.7 * 10^-6)solution.

Accepted Answer

The answer of Calculate the concentration of fluoride ions in...

Question 14

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH)is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH)= 6.5 * 10^-5]

Accepted Answer

Step 1: Write out the chemical equation for the dissociation of benzoic acid:

CS1U1B16S1U1B0HS1U1B15S1U1B0COOH (aq) ⇌ CS1U1B16S1U1B0HS1U1B0+ (aq) + CS1U1B15S1U1B0O1S1U1B2S1U1B2- (aq)

Step 2: Calculate the initial concentration of undissociated benzoic acid:

[CS1U1B16S1U1B0HS1U1B15S1U1B0COOH] = 0.100 M

Step 3: Calculate the initial concentration of H+ ions:

[H+] = (1.00 mL) x (12.0 mol/L) / (1000 mL/L) = 0.120 M

Step 4: Calculate the change in concentration of benzoic acid due to dissociation:

Let x = concentration of H+ ions that react with benzoic acid
[CS1U1B16S1U1B0HS1U1B15S1U1B0COOH] = 0.100 M - x
[CS1U1B16S1U1B0HS1U1B0+ (aq)] = x
[CS1U1B15S1U1B0O1S1U1B2S1U1B2- (aq)] = x

Step 5: Calculate the equilibrium concentration of benzoic acid:

Ks = [CS1U1B16S1U1B0HS1U1B0+ (aq)][CS1U1B15S1U1B0O1S1U1B2S1U1B2- (aq)] / [CS1U1B16S1U1B0HS1U1B15S1U1B0COOH (aq)]
6.5 x 10^-5 = x^2 / (0.100 - x)

Using the quadratic formula, x = 5.1 x 10^-4 M

[CS1U1B16S1U1B0HS1U1B15S1U1B0COOH] = 0.100 M - x = 0.0995 M

Step 6: Calculate the percentage ionization:

% ionization = [CS1U1B16S1U1B0HS1U1B0+ (aq)] / [CS1U1B16S1U1B0HS1U1B15S1U1B0COOH (aq)] x 100%
% ionization = (5.1 x 10^-4 M) / (0.100 M) x 100%
% ionization = 0.52%

Therefore, the answer is D (0.52%).

Question 15

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF₂ , K_sp = 6.9 * 10^-9.)

Accepted Answer

The balanced chemical equation for the reaction is: Mg²⁺ + 2 NaF → MgF2 + Na2²⁺ The equilibrium expression is: Ksp = [Mg2+][F-]^2 Substitute the values given in the problem: 6.9 F1F1F1S1F1F1F10 10^-9 = [Mg2+][F-]^2 Let x be the concentration of Mg2+ and 2x be the concentration of F-. Ksp = x(2x)^2 = 4x^3 Since we have 0.10 M NaF initially, the concentration of F- ion is 2(0.10 M) = 0.20 M. To calculate the minimum concentration of Mg2+ required to initiate the formation of a precipitate of magnesium fluoride, we need to calculate the value of x such that the ion-product (Q) is equal to Ksp. Q = [Mg2+][F-]^2 = x(0.20 M)^2 = 0.04x Setting Q = Ksp, we obtain: 4x^3 = 6.9 F1F1F1S1F1F1F10 10^-9 Solving for x: x = (6.9 F1F1F1S1F1F1F10 10^-9 / 4)^1/3 x = 1.22 F1F1F1S1F1F1F1-0^-3 M Therefore, the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride is approximately 1.22 F1F1F1S1F1F1F1-0^-3 M, which is closest to choice E: 6.9 F1F1F1S1F1F1F10 10^-7 M.

Question 16

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^-4 M Na₂CO₃?

Accepted Answer

When barium nitrate (Ba(NO3)2) is mixed with sodium carbonate (Na2CO3), barium carbonate (BaCO3) precipitates out of the solution due to its low solubility in water. This is a result of a double displacement reaction where the cation of one reactant (Ba2+) combines with the anion of the other reactant (CO32-) to form an insoluble compound, BaCO3.

Question 17

The K_sp for silver(I)phosphate is 1.8 * 10^-18. Determine the silver ion concentration in a saturated solution of silver(I)phosphate.

Accepted Answer

The answer of The K_sp for silver(I)phosphate is 1.8 *...

Question 18

Will a precipitate form (yes or no)when 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? If so, identify the precipitate.

Accepted Answer

A precipitate will form because we can use the solubility rules to determine that PbS is insoluble while NaNO3 is soluble. Therefore, the Pb2+ and S2- ions will combine to form a solid precipitate of PbS.

Question 19

To 1.00 L of a 0.100 M aqueous solution of the week base pyridine (C₅H₅N)is added 1.00 mL of 14.0 M NaOH. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [K_b(C₅H₅N)= 1.7 * 10^-9]

Accepted Answer

The answer of To 1.00 L of a 0.100 M...

Question 20

A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at this temperature is

Accepted Answer

The answer of A saturated sodium carbonate solution at 0°C...

Quiz 17: Acid-Base Equilibria and Solubility Equilibria

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750. mL of 0.125 M NaF. [For CaF₂, K_sp = 3.95 * 10^-11.]

Calculate the concentration of chloride ions in a saturated lead(II) chloride (K_sp = 2.4 * 10^-4) solution.

A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at this temperature is

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10^-3 M MgCl₂ are added to 300. mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂) = 6.9 * 10^-9]

Will a precipitate (ppt) form when 300. mL of 5.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Calculate the silver ion concentration in a saturated solution of silver(I) sulfate (K_sp = 1.4 * 10^-5) .

Will a precipitate (ppt) form when 300. mL of 2.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

Which of the following would decrease the K_sp for PbI₂?

Find the concentration of Pb²⁺ ions in a solution made by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI. [For PbI₂, K_sp = 1.39 * 10^-8.]

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄) = 1.1 * 10^-12] What is the concentration of the silver ion remaining in solution?

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. (For CrF₃, K_sp = 6.6 * 10^-11.)

Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10^-3 M MgCl₂ are added to 500. mL of 1.2 * 10^-3 M NaF? [K_sp (MgF₂) = 6.9 * 10^-9]

Calculate the concentration of fluoride ions in a saturated barium fluoride (K_sp = 1.7 * 10^-6) solution.

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH) = 6.5 * 10^-5]

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF₂ , K_sp = 6.9 * 10^-9.)

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^-4 M Na₂CO₃?

The K_sp for silver(I) phosphate is 1.8 * 10^-18. Determine the silver ion concentration in a saturated solution of silver(I) phosphate.

Will a precipitate form (yes or no) when 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? If so, identify the precipitate.

To 1.00 L of a 0.100 M aqueous solution of the week base pyridine (C₅H₅N) is added 1.00 mL of 14.0 M NaOH. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [K_b(C₅H₅N) = 1.7 * 10^-9]

A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at this temperature is

Quiz 17: Acid-Base Equilibria and Solubility Equilibria

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750. mL of 0.125 M NaF. [For CaF2, Ksp = 3.95 * 10-11.]

Calculate the concentration of chloride ions in a saturated lead(II) chloride (Ksp = 2.4 * 10-4) solution.

A saturated sodium carbonate solution at 100°C contains 45.5 g of dissolved sodium carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at this temperature is

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10-3 M MgCl2 are added to 300. mL of 1.4 * 10-2 M NaF? [Ksp (MgF2) = 6.9 * 10-9]

Will a precipitate (ppt) form when 300. mL of 5.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Calculate the silver ion concentration in a saturated solution of silver(I) sulfate (Ksp = 1.4 * 10-5) .

Will a precipitate (ppt) form when 300. mL of 2.0 * 10-5 M AgNO3 are added to 200. mL of 2.5 * 10-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

Which of the following would decrease the Ksp for PbI2?

Find the concentration of Pb2+ ions in a solution made by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI. [For PbI2, Ksp = 1.39 * 10-8.]

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na2CrO4 are added to 250 mL of 0.12 M AgNO3? [Ksp(Ag2CrO4) = 1.1 * 10-12] What is the concentration of the silver ion remaining in solution?

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. (For CrF3 , Ksp = 6.6 * 10-11.)

Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10-3 M MgCl2 are added to 500. mL of 1.2 * 10-3 M NaF? [Ksp (MgF2) = 6.9 * 10-9]

Calculate the concentration of fluoride ions in a saturated barium fluoride (Ksp = 1.7 * 10-6) solution.

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C6H5COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution? [Ka(C6H5COOH) = 6.5 * 10-5]

Calculate the minimum concentration of Mg2+ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF2 , Ksp = 6.9 * 10-9.)

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 * 10-4 M Na2CO3?

The Ksp for silver(I) phosphate is 1.8 * 10-18. Determine the silver ion concentration in a saturated solution of silver(I) phosphate.

Will a precipitate form (yes or no) when 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? If so, identify the precipitate.

To 1.00 L of a 0.100 M aqueous solution of the week base pyridine (C5H5N) is added 1.00 mL of 14.0 M NaOH. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [Kb(C5H5N) = 1.7 * 10-9]

A saturated sodium carbonate solution at 0°C contains 7.1 g of dissolved sodium carbonate per 100. mL of solution. The solubility product constant for sodium carbonate at this temperature is

Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to 750. mL of 0.125 M NaF. [For CaF₂, K_sp = 3.95 * 10^-11.]

Calculate the concentration of chloride ions in a saturated lead(II) chloride (K_sp = 2.4 * 10^-4) solution.

Will a precipitate of magnesium fluoride form when 200. mL of 1.9 * 10^-3 M MgCl₂ are added to 300. mL of 1.4 * 10^-2 M NaF? [K_sp (MgF₂) = 6.9 * 10^-9]

Will a precipitate (ppt) form when 300. mL of 5.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-7 M NaBr? Answer yes or no, and identify the precipitate if there is one.

Calculate the silver ion concentration in a saturated solution of silver(I) sulfate (K_sp = 1.4 * 10^-5) .

Will a precipitate (ppt) form when 300. mL of 2.0 * 10^-5 M AgNO₃ are added to 200. mL of 2.5 * 10^-9 M NaI? Answer yes or no, and identify the precipitate if there is one.

Which of the following would decrease the K_sp for PbI₂?

Find the concentration of Pb²⁺ ions in a solution made by adding 5.00 g of lead(II) iodide to 500. mL of 0.150 M KI. [For PbI₂, K_sp = 1.39 * 10^-8.]

Which response has both answers correct? Will a precipitate form when 250 mL of 0.33 M Na₂CrO₄ are added to 250 mL of 0.12 M AgNO₃? [K_sp(Ag₂CrO₄) = 1.1 * 10^-12] What is the concentration of the silver ion remaining in solution?

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. (For CrF₃, K_sp = 6.6 * 10^-11.)

Will a precipitate of magnesium fluoride form when 300. mL of 1.1 * 10^-3 M MgCl₂ are added to 500. mL of 1.2 * 10^-3 M NaF? [K_sp (MgF₂) = 6.9 * 10^-9]

Calculate the concentration of fluoride ions in a saturated barium fluoride (K_sp = 1.7 * 10^-6) solution.

To 1.00 L of a 0.100 M aqueous solution of benzoic acid (C₆H₅COOH) is added 1.00 mL of 12.0 M HCl. What is the percentage ionization of the benzoic acid in the resulting solution? [K_a(C₆H₅COOH) = 6.5 * 10^-5]

Calculate the minimum concentration of Mg²⁺ that must be added to 0.10 M NaF in order to initiate a precipitate of magnesium fluoride. (For MgF₂ , K_sp = 6.9 * 10^-9.)

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^-4 M Na₂CO₃?

The K_sp for silver(I) phosphate is 1.8 * 10^-18. Determine the silver ion concentration in a saturated solution of silver(I) phosphate.

Will a precipitate form (yes or no) when 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? If so, identify the precipitate.

To 1.00 L of a 0.100 M aqueous solution of the week base pyridine (C₅H₅N) is added 1.00 mL of 14.0 M NaOH. What fraction of the pyridine molecules in the resulting solution react with water to release hydroxide ions? [K_b(C₅H₅N) = 1.7 * 10^-9]