Question 1

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO₃)₂. What is the equilibrium concentration of cobalt ions? K_f = 5.0 *10⁹ for Co(OH)₄²¯

Accepted Answer

First, let's write out the balanced chemical equation for the reaction between Co(NOS1U1B13S1U1B0)S1U1B12S1U1B0 and NaOH:

Co(NOS1U1B13S1U1B0)S1U1B12S1U1B0 + 2 NaOH → Co(OH)S1U1B14S1U1B0S1U1P12S1S1P0¯ + Na(NOS1U1B13S1U1B0)S1U1B12S1U1B0

We can use the equilibrium constant expression for this reaction to find the equilibrium concentration of Co2+ ions:

Kf = [Co(OH)S1U1B14S1U1B0S1U1P12S1S1P0¯]/[Co(NOS1U1B13S1U1B0)S1U1B12S1U1B0][OH¯]²

We are given the initial concentration and volume of Co(NOS1U1B13S1U1B0)S1U1B12S1U1B0, and we know that 4.50 moles of NaOH were added. The final volume of the solution will be 1.00 L + the volume of 4.50 moles of NaOH added. We can use this information to find the final concentration of OH¯ in the solution, which we can use to calculate the equilibrium concentration of Co2+ ions.

First, we need to find the final volume of the solution:

4.50 mol NaOH x (1 L/1 mol) = 4.50 L

Final volume = 1.00 L + 4.50 L = 5.50 L

Next, we can find the final concentration of OH¯ in the solution:

4.50 mol NaOH x (1 mol OH¯/1 mol NaOH) = 4.50 mol OH¯

[OH¯] = 4.50 mol / 5.50 L = 0.818 M

Now we can use the equilibrium constant expression to find the equilibrium concentration of Co2+ ions:

Kf = [Co(OH)S1U1B14S1U1B0S1U1P12S1S1P0¯]/[Co(NOS1U1B13S1U1B0)S1U1B12S1U1B0][OH¯]²

Kf = 5.0 F1F1F1S1F1F1F10 10S1U1P19S1S1P0

5.0 F1F1F1S1F1F1F10 10S1U1P19S1S1P0 = [Co2+]/(1.00 M)[0.818 M]²

[Co2+] = 3.17 F1F1F1S1F1F1F10 10¯S1U1P5S1S1P0 M ≈ 3.2 F1F1F1S1F1F1F10 10¯S1U1P5S1S1P0 M

Therefore, the equilibrium concentration of cobalt ions is approximately 3.2 F1F1F1S1F1F1F10 10¯S1U1P5S1S1P0 M. The best choice is C.

Question 2

Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 *10¯¹⁸

Accepted Answer

The answer of Calculate the solubility of silver phosphate, Ag₃PO₄,...

Question 3

Which of the following substances has the greatest solubility in water?

Accepted Answer

The answer of Which of the following substances has the...

Question 4

Consider the dissolution of MnS in water (K_sp = 3.0 * 10¯¹⁴). How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Accepted Answer

The dissolution of MnS in water involves the following equilibrium:

MnS (s) ⇌ Mn2+ (aq) + S2- (aq)

Adding aqueous potassium hydroxide (KOH) to the system will increase the concentration of hydroxide ions (OH-) in the solution. The OH- ions will react with the S2- ions to form hydroxide sulfide ions (HS-):

OH- (aq) + S2- (aq) ⇌ HS- (aq)

This will shift the equilibrium of the dissolution reaction to the left, decreasing the concentration of Mn2+ and S2- ions in the solution, and thus decreasing the solubility of MnS. Therefore, the correct answer is B.

Question 5

Calculate the solubility of lead(II) iodide, PbI₂, in 0.025 M KI. K_sp = 7.9 *10¯⁹

Accepted Answer

The solubility of PbI2 in a solution containing a common ion (I-) is calculated using the Ksp expression: Ksp = [Pb2+][I-]^2. In 0.025 M KI, [I-] is approximately 0.025 M. Solving for [Pb2+] gives a solubility of approximately 1.3 * 10^-5 M.

Question 6

Use the following information to calculate the solubility product constant, K_sp, for PbCl₂. A saturated solution of PbCl₂ in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid PbCl₂ residue recovered in the beaker amounted to 0.0162 moles.

Accepted Answer

The balanced chemical equation for the dissolution of PbCl2 in water is:
PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq)

The equation for the solubility product constant expression is:
Ksp = [Pb2+][Cl-]^2

To determine Ksp, we need to find the concentrations of Pb2+ and Cl- in the saturated solution. From the given information, we know that the amount of PbCl2 residue recovered in the beaker is 0.0162 moles. Since PbCl2 dissociates into one Pb2+ ion and two Cl- ions, the amount of Pb2+ in solution is 0.0162 moles and the amount of Cl- is 0.0324 moles.

The volume of the solution is 1.0 L, so the concentration of Pb2+ and Cl- ions in the saturated solution is:

[Pb2+] = 0.0162 mol/L
[Cl-] = 0.0324 mol/L

Substituting the values into the Ksp expression, we get:

Ksp = [Pb2+][Cl-]^2
Ksp = (0.0162 mol/L)(0.0324 mol/L)^2
Ksp = 1.72 x 10^-15 mol^3/L^3

Rounding off to two significant figures and using scientific notation, we get:

Ksp = 1.7 x 10^-15

Therefore, the best choice is C, with the correct value of Ksp.

Question 7

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO₃)₂. K_sp = 6.5 *10¯⁶ for Ca(OH)₂. Which of the following statements is correct?

Accepted Answer

The solubility product constant for Ca(OH)2 is given (Ksp = 6.5 x 10^-6), which allows us to calculate the maximum concentration of Ca2+ and OH- ions that can coexist in solution without precipitating. Since the initial concentration of Ca2+ ions (0.0010 M) is much smaller than this maximum concentration, the solution is unsaturated and no precipitate forms. The presence of KOH does not affect the solubility of Ca(OH)2 in this case. The concentration of calcium ions is not significantly reduced by the addition of a small amount of hydroxide ions. Information about the solubility product constant of calcium nitrate is not required to predict the outcome of this system.

Question 8

Use the following information to calculate the solubility product constant, K_sp, for CuCl. A saturated solution of CuCl in water was prepared and filtered. From the filtrate, 1.0 L was measured out into a beaker and evaporated to dryness. The solid CuCl residue recovered in the beaker was found to weigh 0.041g.

Accepted Answer

The answer of Use the following information to calculate the...

Question 9

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II) chloride solution without causing any precipitation of lead(II) chloride? Assume that addition of KCl does not affect the solution volume. For lead(II) chloride, K_sp = 1.6 * 10¯⁵

Accepted Answer

The answer of What is the maximum mass of KCl...

Question 10

Which of the following substances has the greatest solubility in water?

Accepted Answer

NiCO₃ has the highest Ksp value among the given substances, indicating it has the greatest solubility in water.

Question 11

Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂ solution. K_sp = 5.9 *10¯³

Accepted Answer

The solubility of magnesium sulfate in a 0.10 M MgCl2 solution is 4.2 * 10^-2 M. This is because the common ion effect decreases the solubility of magnesium sulfate.

Question 12

Calculate the solubility of zinc hydroxide, Zn(OH)₂, in 1.00 M NaOH.

Accepted Answer

The answer of Calculate the solubility of zinc hydroxide, Zn(OH)₂,...

Question 13

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO₃)₂. Which of the following statements is correct? K_sp = 6.44 * 10¯³ for CdF₂.

Accepted Answer

Cadmium fluoride precipitates until the solution is saturated.

Question 14

Barium sulfate (BaSO₄) is a slightly soluble salt, with K_sp = 1.1 * 10¯¹⁰. What mass of Ba²⁺ ions will be present in 1.0 L of a saturated solution of barium sulfate?

Accepted Answer

To solve this problem, we need to use the equilibrium constant expression for the dissolution of BaSO4:

BaSO4(s) ⇌ Ba2+(aq) + SO42-(aq)

The equilibrium constant expression is written as:

Ksp = [Ba2+][SO42-]

We are given the value of Ksp as 1.1 x 10^-10, which means that the product of the concentrations of Ba2+ and SO42- ions in a saturated solution of BaSO4 is equal to this value.

Let x be the concentration of Ba2+ and SO42- ions in the saturated solution. Since we assume that BaSO4 is only slightly soluble, we can assume that x is very small compared to the initial concentration of BaSO4, which is usually given as the solubility of BaSO4. Therefore, we can also assume that the initial concentration of BaSO4 is equal to its solubility.

Let S be the solubility of BaSO4. We know that:

[Ba2+] = x
[SO42-] = x
[BaSO4] = S

Substituting these values into the equilibrium constant expression, we get:

Ksp = x2(S - x)

We are asked to find the mass of Ba2+ ions present in 1.0 L of a saturated solution of BaSO4. To do this, we need to convert the concentration of Ba2+ ions into mass using the molar mass of Ba2+.

The molar mass of Ba2+ is:

137.327 g/mol

The concentration of Ba2+ ions is equal to x. Substituting the expression for x from the equilibrium constant equation, we get:

Ksp = x2(S - x)
1.1 x 10^-10 = x2(S - x)

Assuming that x is much smaller than S, we can simplify the equation to:

1.1 x 10^-10 = x2S

Solving for x, we get:

x = sqrt(Ksp/S) = sqrt(1.1 x 10^-10/1) = 1.05 x 10^-5 M

The mass of Ba2+ ions present in 1.0 L of the saturated solution is:

mass = concentration x volume x molar mass
mass = 1.05 x 10^-5 mol/L x 1.0 L x 137.327 g/mol
mass = 0.0014 g

Therefore, the best choice is C.

Question 15

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂ before precipitation of calcium sulfate begins? K_sp = 2.4 *10¯⁵ for calcium sulfate

Accepted Answer

The correct answer is A because the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3)2 before precipitation of calcium sulfate begins is 1.2 * 10^-2 mol. This is because the Ksp for calcium sulfate is 2.4 * 10^-5, which means that the concentration of Ca2+ and SO42- ions in solution must be less than this value in order to prevent precipitation. The addition of sodium sulfate will increase the concentration of SO42- ions in solution, which will in turn decrease the concentration of Ca2+ ions. This will eventually lead to the precipitation of calcium sulfate when the Ksp is exceeded.

Question 16

The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO₃)₃. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? K_f = 3.0 * 10³³ for Al(OH)₄¯

Accepted Answer

The answer of The lab technician Anna Lytic adds 2.20...

Question 17

Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 * 10¯¹²

Accepted Answer

The solubility of Ag₂CrO₄ in a solution containing a common ion (CrO₄²⁻) is calculated using the Ksp expression: Ksp = [Ag⁺]²[CrO₄²⁻]. Given [CrO₄²⁻] = 0.005 M, solve for [Ag⁺]: 2.6 * 10⁻¹² = [Ag⁺]²(0.005), resulting in [Ag⁺] = 1.1 * 10⁻⁵ M.

Question 18

The concentration of the complex ion in each of following solutions is 1.00 M. In which of the solutions will the concentration of the uncomplexed metal ion be the greatest?

Accepted Answer

The answer of The concentration of the complex ion in...

Question 19

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag⁺ ion in the solution after equilibrium has been reestablished. For AgCl, K_sp = 1.8 *10¯¹⁰

Accepted Answer

From the given equation: K_sp = 1.8 F1F1F1S1F1F1F10 10¯¹⁰ we can find the solubility product of AgCl, which is: K_sp = 1.8 × 10^-10 When KCl is added, it will react with Ag+ to form AgCl and K+. This will increase the concentration of Cl- in the solution, causing more AgCl to dissolve until equilibrium is reestablished. Since the volume does not change, we can assume that the concentration of Ag+ remains constant at equilibrium. Let x be the additional amount of AgCl that dissolves. Then, the concentration of Cl- in the solution is 0.200/(1000+x) mol/L. Since Ag+ and Cl- ions have a 1:1 stoichiometry, the concentration of Ag+ ions is also 0.200/(1000+x) mol/L. The total concentration of Ag+ ions in the solution is the sum of the initial concentration and the additional amount that dissolves: [Ag+] = 1.8 × 10^-10 mol/L + 0.200/(1000+x) mol/L Since [Ag+] = [Cl-], the total concentration of Ag+ and Cl- ions (i.e. AgCl) in the solution is: [AgCl] = 2[Ag+] = 2[Cl-] = 2 × 0.200/(1000+x) mol/L The molar solubility of AgCl is defined as the amount of AgCl that dissolves in one liter of solution, which is given by the expression: s = x/(1000+x) mol/L Using the solubility product equation for AgCl, we can express x in terms of s: K_sp = ([Ag+][Cl-])^2 1.8 × 10^-10 = (0.200/(1000+x))^2 x = 1.346 × 10^-8 mol/L Substituting this value of x into the expression for the molar solubility of AgCl, we get: s = 1.346 × 10^-8 / (1000 + 1.346 × 10^-8) = 1.345 × 10^-11 mol/L Since AgCl dissociates into Ag+ and Cl- ions in a 1:1 ratio, the concentration of Ag+ ions in the solution is also 1.345 × 10^-11 mol/L. Therefore, the number of moles of Ag+ ions in the solution is: 1.345 × 10^-11 mol/L × 1.0 L = 1.345 × 10^-11 mol Since the only ion that contains Ag in the solution is Ag+ ion, this is also the number of moles of Ag⁺ ion in the solution after equilibrium has been reestablished. Converting to scientific notation and rounding to one decimal place gives the final answer of 6.7 × 10^-12 mol Ag⁺. Therefore, the correct answer is D.

Question 20

Which of the following substances has the greatest solubility in water?

Accepted Answer

The answer of Which of the following substances has the...

Quiz 19: Ionic Equilibria in Aqueous Systems

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO₃) ₂. What is the equilibrium concentration of cobalt ions? K_f = 5.0 *10⁹ for Co(OH) ₄²¯

Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 *10¯¹⁸

Which of the following substances has the greatest solubility in water?

Consider the dissolution of MnS in water (K_sp = 3.0 * 10¯¹⁴) . How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Calculate the solubility of lead(II) iodide, PbI₂, in 0.025 M KI. K_sp = 7.9 *10¯⁹

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO₃) ₂. K_sp = 6.5 *10¯⁶ for Ca(OH) ₂. Which of the following statements is correct?

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II) chloride solution without causing any precipitation of lead(II) chloride? Assume that addition of KCl does not affect the solution volume. For lead(II) chloride, K_sp = 1.6 * 10¯⁵

Which of the following substances has the greatest solubility in water?

Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂ solution. K_sp = 5.9 *10¯³

Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH.

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO₃) ₂. Which of the following statements is correct? K_sp = 6.44 * 10¯³ for CdF₂.

Barium sulfate (BaSO₄) is a slightly soluble salt, with K_sp = 1.1 * 10¯¹⁰. What mass of Ba²⁺ ions will be present in 1.0 L of a saturated solution of barium sulfate?

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃) ₂ before precipitation of calcium sulfate begins? K_sp = 2.4 *10¯⁵ for calcium sulfate

The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO₃) ₃. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? K_f = 3.0 * 10³³ for Al(OH) ₄¯

Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 * 10¯¹²

The concentration of the complex ion in each of following solutions is 1.00 M. In which of the solutions will the concentration of the uncomplexed metal ion be the greatest?

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag⁺ ion in the solution after equilibrium has been reestablished. For AgCl, K_sp = 1.8 *10¯¹⁰

Which of the following substances has the greatest solubility in water?

Quiz 19: Ionic Equilibria in Aqueous Systems

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO3) 2. What is the equilibrium concentration of cobalt ions? Kf = 5.0 *109 for Co(OH) 42¯

Calculate the solubility of silver phosphate, Ag3PO4, in pure water. Ksp = 2.6 *10¯18

Which of the following substances has the greatest solubility in water?

Consider the dissolution of MnS in water (Ksp = 3.0 * 10¯14) . How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Calculate the solubility of lead(II) iodide, PbI2, in 0.025 M KI. Ksp = 7.9 *10¯9

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO3) 2. Ksp = 6.5 *10¯6 for Ca(OH) 2. Which of the following statements is correct?

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II) chloride solution without causing any precipitation of lead(II) chloride? Assume that addition of KCl does not affect the solution volume. For lead(II) chloride, Ksp = 1.6 * 10¯5

Which of the following substances has the greatest solubility in water?

Calculate the solubility of magnesium sulfate, MgSO4, when placed into a 0.10 M MgCl2 solution. Ksp = 5.9 *10¯3

Calculate the solubility of zinc hydroxide, Zn(OH) 2, in 1.00 M NaOH.

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO3) 2. Which of the following statements is correct? Ksp = 6.44 * 10¯3 for CdF2.

Barium sulfate (BaSO4) is a slightly soluble salt, with Ksp = 1.1 * 10¯10. What mass of Ba2+ ions will be present in 1.0 L of a saturated solution of barium sulfate?

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO3) 2 before precipitation of calcium sulfate begins? Ksp = 2.4 *10¯5 for calcium sulfate

The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO3) 3. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? Kf = 3.0 * 1033 for Al(OH) 4¯

Calculate the solubility of silver chromate, Ag2CrO4, in 0.005 M Na2CrO4. Ksp = 2.6 * 10¯12

The concentration of the complex ion in each of following solutions is 1.00 M. In which of the solutions will the concentration of the uncomplexed metal ion be the greatest?

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag+ ion in the solution after equilibrium has been reestablished. For AgCl, Ksp = 1.8 *10¯10

Which of the following substances has the greatest solubility in water?

A solution is prepared by adding 4.50 mol of sodium hydroxide to 1.00 L of 1.00 M Co(NO₃) ₂. What is the equilibrium concentration of cobalt ions? K_f = 5.0 *10⁹ for Co(OH) ₄²¯

Calculate the solubility of silver phosphate, Ag₃PO₄, in pure water. K_sp = 2.6 *10¯¹⁸

Consider the dissolution of MnS in water (K_sp = 3.0 * 10¯¹⁴) . How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Calculate the solubility of lead(II) iodide, PbI₂, in 0.025 M KI. K_sp = 7.9 *10¯⁹

A lab technician adds 0.015 mol of KOH to 1.00 L of 0.0010 M Ca(NO₃) ₂. K_sp = 6.5 *10¯⁶ for Ca(OH) ₂. Which of the following statements is correct?

What is the maximum mass of KCl that can be added to 1.0 L of a 0.010 M lead(II) chloride solution without causing any precipitation of lead(II) chloride? Assume that addition of KCl does not affect the solution volume. For lead(II) chloride, K_sp = 1.6 * 10¯⁵

Calculate the solubility of magnesium sulfate, MgSO₄, when placed into a 0.10 M MgCl₂ solution. K_sp = 5.9 *10¯³

Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH.

A lab technician adds 0.20 mol of NaF to 1.00 L of 0.35 M cadmium nitrate, Cd(NO₃) ₂. Which of the following statements is correct? K_sp = 6.44 * 10¯³ for CdF₂.

Barium sulfate (BaSO₄) is a slightly soluble salt, with K_sp = 1.1 * 10¯¹⁰. What mass of Ba²⁺ ions will be present in 1.0 L of a saturated solution of barium sulfate?

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃) ₂ before precipitation of calcium sulfate begins? K_sp = 2.4 *10¯⁵ for calcium sulfate

The lab technician Anna Lytic adds 2.20 mol KOH to 1.00 L of 0.5 M Al(NO₃) ₃. What is the concentration of aluminum ions after the aluminum nitrate has reacted with the potassium hydroxide? K_f = 3.0 * 10³³ for Al(OH) ₄¯

Calculate the solubility of silver chromate, Ag₂CrO₄, in 0.005 M Na₂CrO₄. K_sp = 2.6 * 10¯¹²

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag⁺ ion in the solution after equilibrium has been reestablished. For AgCl, K_sp = 1.8 *10¯¹⁰