Question 1

Determine the molar solubility of BaF₂in pure water.K_sp for BaF₂ = 2.45 × 10^-5.

Accepted Answer

The molar solubility of BaF₂ in pure water can be calculated using the K_sp expression:K_sp = [Ba²⁺][F^-]²Assuming that the molar solubility of BaF₂ is x, then:[Ba²⁺] = x[F^-] = 2xSubstituting these values into the K_sp expression, we get:2.45 × 10^-5 = x(2x)²2.45 × 10^-5 = 4x³x³ = 6.13 × 10^-6x = 1.83 × 10^-2 MTherefore, the molar solubility of BaF₂ in pure water is 1.83 × 10^-2 M.

Question 2

Determine the molar solubility of AgI in pure water.K_sp (AgI)= 8.51 × 10^-17.

Accepted Answer

The molar solubility of AgI in pure water can be calculated using the formula for the solubility product constant (Ksp). For AgI, which dissociates into Ag+ and I- ions, Ksp = [Ag+][I-]. Let the molar solubility be S, then Ksp = S^2. Solving for S gives S = sqrt(Ksp) = sqrt(8.51 × 10^-17) = 9.22 × 10^-9 M.

Question 3

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

Accepted Answer

The solubility product (Ksp) for CuI, which dissociates into Cu^2+ and I^-, can be calculated using the formula Ksp = [Cu^2+][I^-]. Given the molar solubility is 2.26 × 10^-6 M, both [Cu^2+] and [I^-] are 2.26 × 10^-6 M. Therefore, Ksp = (2.26 × 10^-6)^2 = 5.11 × 10^-12 M.

Question 4

Determine the solubility of the ions that is calculated from the Ksp for Na₃PO₄.

Accepted Answer

The solubility of ions from the Ksp can be calculated using the formula Ksp = [Na+]^1[S^-]^1 for NaS. Given Ksp = 27x10^-14, the solubility of Na+ and S- ions in water would be the square root of Ksp, which is sqrt(27x10^-14) = 5.2x10^-7. However, the closest match to this process, considering the format of the options, is 27x10^-14, which corresponds to the original Ksp value given. The options seem to represent Ksp values directly, rather than the calculated solubility from those Ksp values, leading to the selection of option D as the correct choice by interpreting the question's intent and the provided options.

Question 5

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Accepted Answer

The correct answer is A because the pH of the solution after the addition of 150.0 mL of HNO3 is 1.70. This is because the NH3 reacts with the HNO3 to form NH4+ and NO3-, and the H+ ions from the HNO3 lower the pH of the solution.

Question 6

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water.Calculate the K_sp for ZnS.

Accepted Answer

The solubility product constant, Ksp, is defined by the following equation:

ZnS(s) ↔ Zn2+(aq) + S2-(aq)

Ksp = [Zn2+][S2-]

At equilibrium, the concentration of each ion will be equal to the molar solubility, s:

Ksp = s^2

Substituting the given molar solubility (1.6 × 10^-12 M) into the Ksp expression yields:

Ksp = (1.6 × 10^-12)^2

Ksp = 2.56 × 10^-24 M^2

Therefore, the correct answer is (D) 2.6 × 10^-24 M.

Question 7

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Accepted Answer

After adding 200.0 mL of 0.10 M HNO3 to 100.0 mL of 0.10 M NH3, there is an excess of HNO3. The total volume is 300.0 mL, and the concentration of excess HNO3 is 0.0333 M. The pH is determined by the concentration of H+ ions from the excess HNO3, resulting in a pH of 1.48.

Question 8

Determine the molar solubility of MgCO₃in pure water.K_sp (MgCO₃)= 6.82 × 10^-6.

Accepted Answer

The answer of Determine the molar solubility of MgCO₃in...

Question 9

When a diprotic acid is titrated with a strong base,and the K_a1 and K_a2 are significantly different,then the pH vs.volume plot of the titration will have

Accepted Answer

Since the two dissociation constants are significantly different, the diprotic acid will have two distinct equivalence points. At the first equivalence point, only the first proton will be neutralized, resulting in a pH greater than 7. At the second equivalence point, both protons will be neutralized, resulting in a pH of exactly 7. Therefore, the pH vs. volume plot of the titration will have two distinct equivalence points below pH 7.

Question 10

Determine the molar solubility of PbSO₄ in pure water.K_sp (PbSO₄)= 1.82 × 10^-8.

Accepted Answer

The answer of Determine the molar solubility of PbSO₄ in...

Question 11

When titrating a weak base with a monoprotic acid at 25°C,the

Accepted Answer

When titrating a weak base with a monoprotic acid, the equivalence point occurs when all of the base has been neutralized by the acid. However, since the weak base is only partially ionized, there will be some unreacted base molecules present in the solution (even at the equivalence point). These unreacted base molecules will hydrolyze water to produce hydroxide ions, which will increase the pH of the solution above 7. Therefore, the pH at the equivalence point of a weak base-strong acid titration will be greater than 7. Choice E is the correct answer.

Question 12

Determine the molar solubility of Fe(OH)₂in pure water.K_sp for Fe(OH)₂= 4.87 × 10^-17.

Accepted Answer

The equilibrium equation is:

Fe(OH)2(s) ⇌ Fe2+(aq) + 2OH-(aq)

Ksp = [Fe2+][OH-]2

Molar solubility of Fe(OH)2(s) = x

[Fe2+] = x

[OH-] = 2x

Ksp = 4.87 × 10-17 = x (2x)2

x = molar solubility of Fe(OH)2(s) = 2.30 × 10-6 M.

Therefore, the best choice is E.

Question 13

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 100.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Accepted Answer

The answer of A 100.0 mL sample of 0.10 M...

Question 14

Determine the solubility of the ions that is calculated from the Ksp for Mg₂CO₃.

Accepted Answer

The answer of Determine the solubility of the ions that...

Question 15

100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Accepted Answer

The pH of the solution before the addition of any HNO₃ is determined by the concentration of NH₃ and its Kb. Using the formula for pOH: pOH = 1/2(pKb - log[base]), and converting to pH: pH = 14 - pOH, the pH is approximately 11.13.

Question 16

When titrating a weak base with HCl at 25°C,the

Accepted Answer

EAt the equivalence point of titrating a weak base with a strong acid like HCl, the solution will be acidic because the salt formed hydrolyzes to produce an acidic solution, making the pH less than 7. The moles of acid and base required to reach the equivalence point depend on their stoichiometry in the balanced equation, not on their strengths. However, for a 1:1 stoichiometric reaction, equal moles of acid and base are required. The statement about requiring more moles of acid than base is incorrect without specifying the stoichiometry of the reaction; however, in the context of typical titrations where they react in a 1:1 ratio, the amount of acid and base needed to reach the equivalence point would be the same, making both A and E correct in the context of the question's implications.

Question 17

Determine the molar solubility for Al(OH)₃ in pure water.K_sp for Al(OH)₃ = 1.3 × 10^-33.

Accepted Answer

We can use the given value of Ksp to calculate the molar solubility of Al(OH)3:

Ksp = [Al3+][OH-]^3

Let x be the molar solubility of Al(OH)3 in water. Then we can write:

Ksp = (x)(3x)^3 = 27x^4
1.3 × 10^-33 = 27x^4
x = (1.3 × 10^-33 / 27)^(1/4) = 2.6 × 10^-9 M

Therefore, the correct answer is choice D.

Question 18

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 50.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Accepted Answer

The answer of A 100.0 mL sample of 0.10 M...

Question 19

Determine the molar solubility for Pb₃(PO₄)₂ in pure water.Ksp for Pb₃(PO₄)₂ is 1.0 × 10^-54.

Accepted Answer

The answer of Determine the molar solubility for Pb₃(PO₄)₂ in...

Question 20

Determine the molar solubility for Zn(OH)₂ in pure water.Ksp for Zn(OH)₂ is 3.00 × 10^-17.

Accepted Answer

The solubility product expression for Zn(OH)₂ is Ksp = [Zn²⁺][OH⁻]². Let the molar solubility be s, then [Zn²⁺] = s and [OH⁻] = 2s. Ksp = s(2s)² = 4s³. Solving 4s³ = 3.00 × 10⁻¹⁷ gives s ≈ 1.96 × 10⁻⁶ M.

Quiz 17: Aqueous Ionic Equilibrium

Determine the molar solubility of BaF₂in pure water.K_sp for BaF₂ = 2.45 × 10^-5.

Determine the molar solubility of AgI in pure water.K_sp (AgI) = 8.51 × 10^-17.

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

Determine the solubility of the ions that is calculated from the Ksp for Na₃PO₄.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water.Calculate the K_sp for ZnS.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Determine the molar solubility of MgCO₃in pure water.K_sp (MgCO₃) = 6.82 × 10^-6.

When a diprotic acid is titrated with a strong base,and the K_a1 and K_a2 are significantly different,then the pH vs.volume plot of the titration will have

Determine the molar solubility of PbSO₄ in pure water.K_sp (PbSO₄) = 1.82 × 10^-8.

When titrating a weak base with a monoprotic acid at 25°C,the

Determine the molar solubility of Fe(OH) ₂in pure water.K_sp for Fe(OH) ₂= 4.87 × 10^-17.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 100.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Determine the solubility of the ions that is calculated from the Ksp for Mg₂CO₃.

100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

When titrating a weak base with HCl at 25°C,the

Determine the molar solubility for Al(OH) ₃ in pure water.K_sp for Al(OH) ₃ = 1.3 × 10^-33.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 50.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Determine the molar solubility for Pb₃(PO₄) ₂ in pure water.Ksp for Pb₃(PO₄) ₂ is 1.0 × 10^-54.

Determine the molar solubility for Zn(OH) ₂ in pure water.Ksp for Zn(OH) ₂ is 3.00 × 10^-17.

Quiz 17: Aqueous Ionic Equilibrium

Determine the molar solubility of BaF2 in pure water.Ksp for BaF2 = 2.45 × 10-5.

Determine the molar solubility of AgI in pure water.Ksp (AgI) = 8.51 × 10-17.

The molar solubility of CuI is 2.26 × 10-6 M in pure water.Calculate the Ksp for CuI.

Determine the solubility of the ions that is calculated from the Ksp for Na3PO4.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 150.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

The molar solubility of ZnS is 1.6 × 10-12 M in pure water.Calculate the Ksp for ZnS.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 200.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Determine the molar solubility of MgCO3 in pure water.Ksp (MgCO3) = 6.82 × 10-6.

When a diprotic acid is titrated with a strong base,and the Ka1 and Ka2 are significantly different,then the pH vs.volume plot of the titration will have

Determine the molar solubility of PbSO4 in pure water.Ksp (PbSO4) = 1.82 × 10-8.

When titrating a weak base with a monoprotic acid at 25°C,the

Determine the molar solubility of Fe(OH) 2 in pure water.Ksp for Fe(OH) 2= 4.87 × 10-17.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 100.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Determine the solubility of the ions that is calculated from the Ksp for Mg2CO3.

100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution before the addition of any HNO3.The Kb of NH3 is 1.8 × 10-5.

When titrating a weak base with HCl at 25°C,the

Determine the molar solubility for Al(OH) 3 in pure water.Ksp for Al(OH) 3 = 1.3 × 10-33.

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3.Determine the pH of the solution after the addition of 50.0 mL of HNO3.The Kb of NH3 is 1.8 × 10-5.

Determine the molar solubility for Pb3(PO4) 2 in pure water.Ksp for Pb3(PO4) 2 is 1.0 × 10-54.

Determine the molar solubility for Zn(OH) 2 in pure water.Ksp for Zn(OH) 2 is 3.00 × 10-17.

Determine the molar solubility of BaF₂in pure water.K_sp for BaF₂ = 2.45 × 10^-5.

Determine the molar solubility of AgI in pure water.K_sp (AgI) = 8.51 × 10^-17.

The molar solubility of CuI is 2.26 × 10^-6 M in pure water.Calculate the K_sp for CuI.

Determine the solubility of the ions that is calculated from the Ksp for Na₃PO₄.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 150.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

The molar solubility of ZnS is 1.6 × 10^-12 M in pure water.Calculate the K_sp for ZnS.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 200.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Determine the molar solubility of MgCO₃in pure water.K_sp (MgCO₃) = 6.82 × 10^-6.

When a diprotic acid is titrated with a strong base,and the K_a1 and K_a2 are significantly different,then the pH vs.volume plot of the titration will have

Determine the molar solubility of PbSO₄ in pure water.K_sp (PbSO₄) = 1.82 × 10^-8.

Determine the molar solubility of Fe(OH) ₂in pure water.K_sp for Fe(OH) ₂= 4.87 × 10^-17.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 100.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Determine the solubility of the ions that is calculated from the Ksp for Mg₂CO₃.

100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution before the addition of any HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Determine the molar solubility for Al(OH) ₃ in pure water.K_sp for Al(OH) ₃ = 1.3 × 10^-33.

A 100.0 mL sample of 0.10 M NH₃ is titrated with 0.10 M HNO₃.Determine the pH of the solution after the addition of 50.0 mL of HNO₃.The K_b of NH₃ is 1.8 × 10^-5.

Determine the molar solubility for Pb₃(PO₄) ₂ in pure water.Ksp for Pb₃(PO₄) ₂ is 1.0 × 10^-54.

Determine the molar solubility for Zn(OH) ₂ in pure water.Ksp for Zn(OH) ₂ is 3.00 × 10^-17.