Question 1

Solid potassium chromate (K₂CrO₄) is slowly added to a solution containing 0. 50 mol L^-1 AgNO₃ and 0. 50 mol L^-1 Ba(NO₃)₂. What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and respectively.

Accepted Answer

The answer of Solid potassium chromate (K₂CrO₄) is slowly added...

Question 2

What is the molar solubility of AgCl in 0. 40 mol L^-1 NH₃? K_sp for AgCl is and K_f for Ag(NH₃)₂⁺ is

Accepted Answer

The answer of What is the molar solubility of AgCl...

Question 3

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0. 50 mol L^-1 HCl for complete neutralization? K_a = 3.0 × 10^-8 for HOCl.

Accepted Answer

The answer of What is the pH at the equivalence...

Question 4

Match the following.
-pH = 7

Accepted Answer

pH = 7 indicates neutral conditions, which is the equivalence point of a strong acid-strong base titration.

Question 5

A solution of NaF is added dropwise to a solution that is 0.0188 mol L^-1 in . When the concentration of exceeds ________ mol L^-1, will precipitate. Neglect volume changes. For ,

Accepted Answer

The answer of A solution of NaF is added dropwise...

Question 6

Calculate the solubility (in g L^-1) of silver carbonate in water at 25 °C if the K_sp for is 8.4 × .

Accepted Answer

The answer of Calculate the solubility (in g L^-1) of...

Question 7

A 25.0 mL sample of 0.150 mol L^-1 butanoic acid is titrated with a 0.150 mol L^-1 NaOH solution. What is the pH after 13.3 mL of base is added? The of butanoic acid is 1.5 × 10^-5.

Accepted Answer

The answer of A 25.0 mL sample of 0.150 mol...

Question 8

What is the molar solubility of AgCl in 0. 10 mol L^-1 NaCN if the colourless complex ion Ag(CN)₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN)₂^- is 1.0 × 10²¹.

Accepted Answer

The correct answer is A because the molar solubility of AgCl in 0.10 mol L-1 NaCN is 0.050 mol L-1. This is because the formation of the colourless complex ion Ag(CN)2- decreases the concentration of free Ag+ ions in solution, which in turn decreases the solubility of AgCl.

Question 9

What is the pH of the resulting solution if 25.00 mL of 0.10 mol L^-1 acetic acid is added to 10.00 mL of 0.10 mol L^-1 NaOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH

Accepted Answer

First, we need to calculate the amount of moles of acetic acid and NaOH added:
moles of acetic acid = 0.1 mol/L x (25.00 mL/1000 mL) = 0.0025 mol
moles of NaOH = 0.1 mol/L x (10.00 mL/1000 mL) = 0.0010 mol

Since acetic acid and NaOH react in a 1:1 ratio, all the moles of NaOH will be used up by the acetic acid. This means that the remaining moles of acetic acid will be in solution and will determine the pH of the solution.

The initial moles of acetic acid in solution would be:
moles of acetic acid = 0.1 mol/L x (35.00 mL/1000 mL) = 0.0035 mol

Since acetic acid is a weak acid, we need to use the dissociation constant (Ka) to calculate the pH of the solution. The equation for the dissociation of acetic acid is as follows:
CH3COOH + H2O ⇌ CH3COO- + H3O+

The Ka for acetic acid is 1.8 x 10^-5. We can set up an ICE table to help us calculate the pH:

I: 0.0035 mol/L (initial concentration of acid)
C: -x mol/L (concentration change)
E: (0.0035-x) mol/L (equilibrium concentration of acid)

Ka = [CH3COO-][H3O+] / [CH3COOH]
1.8 x 10^-5 = x^2 / (0.0035 - x)

Solving the quadratic equation, we get x = 6.30 x 10^-4
pH = -log[H3O+] = -log(6.30 x 10^-4) = 3.20

However, we need to remember that we calculated the pH for the remaining acetic acid only, not for the entire solution. The NaOH that was added has contributed additional OH- ions to the solution. So we need to calculate the concentration of OH- ions before we can calculate the final pH.

The amount of NaOH added is 0.1 mol/L x (10.00 mL/1000 mL) = 0.0010 mol. Since NaOH is a strong base, it completely dissociates in solution. This means that the concentration of OH- ions in solution is equal to the amount of NaOH added, divided by the total volume of the solution:

[OH-] = 0.0010 mol / (25.00 mL + 10.00 mL) / 1000 mL/mL = 0.033 mol/L

To calculate the final pH, we can use the following equation:
pH = 14 - pOH = 14 - (-log[OH-]) = 14 - (-log0.033) = 14 + 1.48 = 15.48

Therefore, the pH of the resulting solution is 15.48, which corresponds to answer choice D.

Question 10

What is the pH of the resulting solution if 45 mL of 0.432 mol L^-1 methylamine, CH₃NH₂, is added to 15 mL of 0.234 mol L^-1 HCl? Assume that the volumes of the solutions are additive. K_a = 2.70 × 10^-11for CH₃NH₃⁺.

Accepted Answer

The answer of What is the pH of the resulting...

Question 11

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

Accepted Answer

In general, the solubility of a salt will increase as the size and charge of the cation increase. Therefore, the larger cations Ca2+ and K+ in options C and D, respectively, will make the corresponding salts more soluble than the smaller Na+ and H+ cations in options A and B. Additionally, the anions in all options are the same (Br-), so the only factor affecting solubility is the cation. Therefore, the solution containing CaBr2 should result in the least soluble PbBr2 due to the larger size and charge of the Ca2+ cation.

Question 12

What is the molar solubility of Mg(OH)₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH)₂ is

Accepted Answer

The first step is to write the balanced equation for the dissolution of Mg(OH)2 in water: Mg(OH)2(s) <=> Mg2+(aq) + 2OH-(aq) The equilibrium constant expression for this reaction is: Ksp = [Mg2+][OH-]^2 Since the solution is basic, we can assume that all the OH- comes from the dissociation of water: OH-(aq) + H2O(l) <=> H3O+(aq) + OH-(aq) Kw = [H3O+][OH-] = 1.0 x 10^-14 pH = 12.50 implies [H3O+] = 10^-12.50 = 3.16 x 10^-13 M Thus: [OH-] = Kw/[H3O+] = 3.16 x 10^-14 M Substituting these values into the expression for Ksp and solving for [Mg2+]: Ksp = [Mg2+][OH-]^2 1.1 x 10^-11 = [Mg2+](3.16 x 10^-14)^2 [Mg2+] = 5.6 x 10^-10 M The molar solubility of Mg(OH)2 in this solution is equal to the concentration of Mg2+: mol solubility = 5.6 x 10^-10 M Therefore, the best choice is B.

Question 13

Calculate the K_sp for silver carbonate if the solubility of Ag₂CO₃ in pure water is 3.5 × 10^-2g L^-1.

Accepted Answer

The solubility product constant (Ksp) expression for silver carbonate (Ag2CO3) is:
Ag2CO3(s) ⇌ 2Ag+(aq) + CO32-(aq)
Ksp = [Ag+]^2[CO32-]
We can use the relationship between Ksp values to find the Ksp for Ag2CO3:
Ksp(Ag2CO3) = Ksp(Ag2CO3) / Ksp(Ag2S) × Ksp(Ag2CO3/Ag2S)
Ksp(Ag2S) is the solubility product constant for Ag2S (silver sulfide), which is given as 3.5 × 10^-12.
Ksp(Ag2CO3/Ag2S) is the ion product quotient for the dissolution of Ag2CO3 and Ag2S, which we can assume is equal to the solubility product constant for Ag2S since it is more insoluble than Ag2CO3.
Ksp(Ag2CO3/Ag2S) = Ksp(Ag2S) = 3.5 × 10^-12
Substituting the given value for Ksp(Ag2S) and the known concentrations of Ag+ and CO32- in Ag2CO3 (which are equal because of the 1:1 stoichiometry) into the Ksp expression, we get:
3.5 × 10^-12 = (2x)^2(x)
x = solubility of Ag2CO3 = 5.9 × 10^-9 M
Therefore, the Ksp for Ag2CO3 is:
Ksp(Ag2CO3) = (5.9 × 10^-9)^2(5.9 × 10^-9) = 2.1 × 10^-17
This matches option B, so the answer is B.

Question 14

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 acetic acid with 10.00 mL of 0.10 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = for CH₃COOH.

Accepted Answer

This is a neutralization reaction, in which the acetic acid and potassium hydroxide react to form water and potassium acetate. The balanced chemical equation is:

CH3COOH + KOH → H2O + CH3COOK

The moles of acid and base are equal, since they have equal concentration and volume. So, the limiting reactant is the one with fewer moles, which is the acid. Therefore, all the acid is consumed by the base, and the excess amount of base determines the pH of the solution.

The amount of base is:

n(KOH) = C(KOH) x V(KOH)
n(KOH) = 0.10 mol/L x 0.01000 L
n(KOH) = 0.00100 mol

The amount of H+ and OH- produced by the reaction are equal and are given by:

n(H+) = n(OH-) = n(KOH) = 0.00100 mol

The volume of the final solution is:

V(final) = V(acid) + V(base) = 0.01000 L + 0.01000 L = 0.02000 L

So, the concentration of H+ and OH- can be calculated as:

C(H+) = n(H+) / V(final) = 0.00100 mol / 0.02000 L = 0.0500 mol/L
pH = -log[H+] = -log(0.0500) = 1.301

pOH = -log[OH-] = -log(0.0500) = 1.301
pH + pOH = 14.00
pH = 14.00 - pOH = 14.00 - 1.301 = 12.699
pH = 8.699 ≈ 8.72

Therefore, the pH of the solution is 8.72, which is closest to choice C.

Question 15

Formic acid (HCOOH, K_a = 1.8 × 10^-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 mol L^-1 NaOH to reach the equivalence point?

Accepted Answer

The answer of Formic acid (HCOOH, K_a = 1.8 ×...

Question 16

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 acetic acid (CH₃COOH) with 50.00 mL of 0. 100 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for

Accepted Answer

The answer of What is the pH of a solution...

Question 17

What is the molar solubility of silver iodide ( AgI) in water? The solubility-product constant for AgI is 8.5 × 10^-17 at 25 °C.

Accepted Answer

The answer of What is the molar solubility of silver...

Question 18

Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L^-1 HCl to reach the equivalence point?

Accepted Answer

The answer of Sodium hypochlorite, NaOCl, is the active ingredient...

Question 19

Calculate the molar solubility of thallium chloride (TlCl) in 0. 50 mol L^-1 NaCl at 25 °C. K_sp for TlCl is

Accepted Answer

The answer of Calculate the molar solubility of thallium chloride...

Question 20

What is the molar solubility of calcium hydroxide ( Ca(OH)₂) in water? The solubility-product constant for CaOH₂ is 4.5 × 10^-6 at

Accepted Answer

The answer of What is the molar solubility of calcium...

Quiz 16: Aqueous Ionic Equilibrium

Solid potassium chromate (K₂CrO₄) is slowly added to a solution containing 0. 50 mol L^-1 AgNO₃ and 0. 50 mol L^-1 Ba(NO₃) ₂. What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and respectively.

What is the molar solubility of AgCl in 0. 40 mol L^-1 NH₃? K_sp for AgCl is and K_f for Ag(NH₃) ₂⁺ is

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0. 50 mol L^-1 HCl for complete neutralization? K_a = 3.0 × 10^-8 for HOCl.

Match the following. -pH = 7

A solution of NaF is added dropwise to a solution that is 0.0188 mol L^-1 in . When the concentration of exceeds ________ mol L^-1, will precipitate. Neglect volume changes. For ,

Calculate the solubility (in g L^-1) of silver carbonate in water at 25 °C if the K_sp for is 8.4 × .

A 25.0 mL sample of 0.150 mol L^-1 butanoic acid is titrated with a 0.150 mol L^-1 NaOH solution. What is the pH after 13.3 mL of base is added? The of butanoic acid is 1.5 × 10^-5.

What is the molar solubility of AgCl in 0. 10 mol L^-1 NaCN if the colourless complex ion Ag(CN) ₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN) ₂^- is 1.0 × 10²¹.

What is the pH of the resulting solution if 25.00 mL of 0.10 mol L^-1 acetic acid is added to 10.00 mL of 0.10 mol L^-1 NaOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH

What is the pH of the resulting solution if 45 mL of 0.432 mol L^-1 methylamine, CH₃NH₂, is added to 15 mL of 0.234 mol L^-1 HCl? Assume that the volumes of the solutions are additive. K_a = 2.70 × 10^-11for CH₃NH₃⁺.

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

What is the molar solubility of Mg(OH) ₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH) ₂ is

Calculate the K_sp for silver carbonate if the solubility of Ag₂CO₃ in pure water is 3.5 × 10^-2g L^-1.

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 acetic acid with 10.00 mL of 0.10 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = for CH₃COOH.

Formic acid (HCOOH, K_a = 1.8 × 10^-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 mol L^-1 NaOH to reach the equivalence point?

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 acetic acid (CH₃COOH) with 50.00 mL of 0. 100 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for

What is the molar solubility of silver iodide ( AgI) in water? The solubility-product constant for AgI is 8.5 × 10^-17 at 25 °C.

Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L^-1 HCl to reach the equivalence point?

Calculate the molar solubility of thallium chloride (TlCl) in 0. 50 mol L^-1 NaCl at 25 °C. K_sp for TlCl is

What is the molar solubility of calcium hydroxide ( Ca(OH) ₂) in water? The solubility-product constant for CaOH₂ is 4.5 × 10^-6 at

Quiz 16: Aqueous Ionic Equilibrium

Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0. 50 mol L-1 AgNO3 and 0. 50 mol L-1 Ba(NO3) 2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and respectively.

What is the molar solubility of AgCl in 0. 40 mol L-1 NH3? Ksp for AgCl is and Kf for Ag(NH3) 2+ is

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0. 50 mol L-1 HCl for complete neutralization? Ka = 3.0 × 10-8 for HOCl.

Match the following. -pH = 7

A solution of NaF is added dropwise to a solution that is 0.0188 mol L-1 in . When the concentration of exceeds ________ mol L-1, will precipitate. Neglect volume changes. For ,

Calculate the solubility (in g L-1) of silver carbonate in water at 25 °C if the Ksp for is 8.4 × .

A 25.0 mL sample of 0.150 mol L-1 butanoic acid is titrated with a 0.150 mol L-1 NaOH solution. What is the pH after 13.3 mL of base is added? The of butanoic acid is 1.5 × 10-5.

What is the molar solubility of AgCl in 0. 10 mol L-1 NaCN if the colourless complex ion Ag(CN) 2- forms? Ksp for AgCl is 1.8 × 10-10 and Kf for Ag(CN) 2- is 1.0 × 1021.

What is the pH of the resulting solution if 25.00 mL of 0.10 mol L-1 acetic acid is added to 10.00 mL of 0.10 mol L-1 NaOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for CH3COOH

What is the pH of the resulting solution if 45 mL of 0.432 mol L-1 methylamine, CH3NH2, is added to 15 mL of 0.234 mol L-1 HCl? Assume that the volumes of the solutions are additive. Ka = 2.70 × 10-11 for CH3NH3+.

In which of the following solutions would solid PbBr2 be expected to be the least soluble at 25 °C?

What is the molar solubility of Mg(OH) 2 in a basic solution with a pH of 12.50? Ksp for Mg(OH) 2 is

Calculate the Ksp for silver carbonate if the solubility of Ag2CO3 in pure water is 3.5 × 10-2 g L-1.

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L-1 acetic acid with 10.00 mL of 0.10 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = for CH3COOH.

Formic acid (HCOOH, Ka = 1.8 × 10-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 mol L-1 NaOH to reach the equivalence point?

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L-1 acetic acid (CH3COOH) with 50.00 mL of 0. 100 mol L-1 KOH? Assume that the volumes of the solutions are additive. Ka = 1.8 × 10-5 for

What is the molar solubility of silver iodide ( AgI ) in water? The solubility-product constant for AgI is 8.5 × 10-17 at 25 °C.

Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L-1 HCl to reach the equivalence point?

Calculate the molar solubility of thallium chloride (TlCl) in 0. 50 mol L-1 NaCl at 25 °C. Ksp for TlCl is

What is the molar solubility of calcium hydroxide ( Ca(OH) 2) in water? The solubility-product constant for CaOH2 is 4.5 × 10-6 at

Solid potassium chromate (K₂CrO₄) is slowly added to a solution containing 0. 50 mol L^-1 AgNO₃ and 0. 50 mol L^-1 Ba(NO₃) ₂. What is the Ag⁺ concentration when BaCrO₄ just starts to precipitate? The K_sp for Ag₂CrO₄ and BaCrO₄ are 1.1 × 10^-12 and respectively.

What is the molar solubility of AgCl in 0. 40 mol L^-1 NH₃? K_sp for AgCl is and K_f for Ag(NH₃) ₂⁺ is

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0. 50 mol L^-1 HCl for complete neutralization? K_a = 3.0 × 10^-8 for HOCl.

A solution of NaF is added dropwise to a solution that is 0.0188 mol L^-1 in . When the concentration of exceeds ________ mol L^-1, will precipitate. Neglect volume changes. For ,

Calculate the solubility (in g L^-1) of silver carbonate in water at 25 °C if the K_sp for is 8.4 × .

A 25.0 mL sample of 0.150 mol L^-1 butanoic acid is titrated with a 0.150 mol L^-1 NaOH solution. What is the pH after 13.3 mL of base is added? The of butanoic acid is 1.5 × 10^-5.

What is the molar solubility of AgCl in 0. 10 mol L^-1 NaCN if the colourless complex ion Ag(CN) ₂^- forms? K_sp for AgCl is 1.8 × 10^-10 and K_f for Ag(CN) ₂^- is 1.0 × 10²¹.

What is the pH of the resulting solution if 25.00 mL of 0.10 mol L^-1 acetic acid is added to 10.00 mL of 0.10 mol L^-1 NaOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for CH₃COOH

What is the pH of the resulting solution if 45 mL of 0.432 mol L^-1 methylamine, CH₃NH₂, is added to 15 mL of 0.234 mol L^-1 HCl? Assume that the volumes of the solutions are additive. K_a = 2.70 × 10^-11for CH₃NH₃⁺.

In which of the following solutions would solid PbBr₂ be expected to be the least soluble at 25 °C?

What is the molar solubility of Mg(OH) ₂ in a basic solution with a pH of 12.50? K_spfor Mg(OH) ₂ is

Calculate the K_sp for silver carbonate if the solubility of Ag₂CO₃ in pure water is 3.5 × 10^-2g L^-1.

What is the pH of a solution made by mixing 10.00 mL of 0.10 mol L^-1 acetic acid with 10.00 mL of 0.10 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = for CH₃COOH.

Formic acid (HCOOH, K_a = 1.8 × 10^-4) is the principal component in the venom of stinging ants. What is the molarity of a formic acid solution if 25.00 mL of the formic acid solution requires 29.80 mL of 0.0567 mol L^-1 NaOH to reach the equivalence point?

What is the pH of a solution made by mixing 30.00 mL of 0.10 mol L^-1 acetic acid (CH₃COOH) with 50.00 mL of 0. 100 mol L^-1 KOH? Assume that the volumes of the solutions are additive. K_a = 1.8 × 10^-5for

What is the molar solubility of silver iodide ( AgI) in water? The solubility-product constant for AgI is 8.5 × 10^-17 at 25 °C.

Sodium hypochlorite, NaOCl, is the active ingredient in household bleach. What is the concentration of hypochlorite ion if 20.00 mL of bleach requires 32.00 mL of 0.500 mol L^-1 HCl to reach the equivalence point?

Calculate the molar solubility of thallium chloride (TlCl) in 0. 50 mol L^-1 NaCl at 25 °C. K_sp for TlCl is

What is the molar solubility of calcium hydroxide ( Ca(OH) ₂) in water? The solubility-product constant for CaOH₂ is 4.5 × 10^-6 at