Question 1

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? Hg(CN)₄²⁻ K_f = 9.3 × 10³⁸ Be(OH)₄²⁻ K_f = 4.0 × 10¹⁸ Zn(OH)₄²⁻ K_f = 3.0 × 10¹⁵ Cu(NH₃)₄²⁺ K_f = 5.6 × 10¹¹ CdI₄²⁻ K_f = 1.0 × 10⁶

Accepted Answer

The concentration of the uncomplexed metal ion is inversely related to the stability constant (Kf) of the complex ion. The complex with the lowest Kf value will have the greatest concentration of the uncomplexed metal ion. CdI4^2- has the lowest Kf value (1.0 × 10^6), indicating that Cd^2+ will have the greatest concentration of uncomplexed metal ion.

Question 2

What is the maximum amount of sodium sulfate that can be added to 1.00 L of 0.0020 M Ca(NO₃)₂before 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 precipitation of calcium sulfate when the Ksp is exceeded.

Question 3

The salts X(NO₃)₂and Y(NO₃)₂ (where X⁺ and Y⁺ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Using the K_sp values listed below, decide which aqueous reagent, if any, will definitely precipitate X⁺ before precipitating Y⁺ from solution. Given K_spvalues:XCl₂, 1 × 10⁻⁵ YCl₂, 1 × 10⁻¹⁰ X(OH)₂, 1 × 10⁻¹⁰Y(OH)₂, 1 × 10⁻⁵

Accepted Answer

Ammonia (NH₃) will increase the concentration of OH⁻ ions in solution, which will cause X(OH)₂ to precipitate first due to its lower Ksp value compared to Y(OH)₂.

Question 4

Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (K_sp for Ag₂CO₃ = 8.1 x 10^-12)

Accepted Answer

The molar solubility of Ag2CO3 in a 1.0 M Na2CO3 solution is calculated by considering the common ion effect. The presence of CO3^2- from Na2CO3 suppresses the solubility of Ag2CO3. The solubility product expression is Ksp = [Ag+]^2[CO3^2-]. Assuming x is the solubility of Ag2CO3, [Ag+] = 2x and [CO3^2-] = 1.0 M. Solving 8.1 x 10^-12 = (2x)^2(1.0) gives x = 1.4 x 10^-6 M.

Question 5

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 Ksp value given is for calcium hydroxide, not calcium nitrate. Since the concentration of calcium ions is much lower than the Ksp value for calcium hydroxide, the solution is unsaturated and no precipitate will form. The addition of KOH will neutralize some of the nitrate ions, but it will not affect the solubility of calcium hydroxide in the given solution.

Question 6

The salts X(NO₃)₂and Y(NO₃)₂ (where X⁺ and Y⁺ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Which of the answers gives the concentration of chloride ions will precipitate the most YCl₂ without precipitating any XCl₂? Given K_spvalues: XCl₂, 2 × 10⁻⁵YCl₂, 1 × 10⁻¹⁰

Accepted Answer

To find the concentration of chloride ions that will precipitate YCl2 without precipitating XCl2, we use the solubility product constant (Ksp) formula: Ksp = [Metal ion][Cl-]^2. For XCl2, Ksp = 2 × 10^-15, and for YCl2, Ksp = 1 × 10^-10. Since the solution is 0.1 M in each metal ion, we set up the equation for YCl2 to precipitate first. For YCl2, 1 × 10^-10 = (0.1)[Cl-]^2, solving for [Cl-] gives [Cl-] = √(1 × 10^-10 / 0.1) = √(1 × 10^-9) = 1 × 10^-4.5 M. The closest option that will precipitate YCl2 without affecting XCl2 is 0.001 M Cl-, as it is slightly higher than the calculated concentration, ensuring precipitation of YCl2 while not exceeding the solubility of XCl2.

Question 7

The salts X(NO₃)₂and Y(NO₃)₂ (where X⁺ and Y⁺ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Using the K_sp values listed below, decide which aqueous reagent, if any, will definitely precipitate X⁺ before precipitating Y⁺ from solution. Given K_spvalues:XCl₂, 1 × 10⁻⁵YCl₂, 1 × 10⁻¹⁰X(OH)₂, 1 × 10⁻¹⁰Y(OH)₂, 1 × 10⁻⁵

Accepted Answer

The answer of The salts X(NO₃)₂and Y(NO₃)₂ (where X⁺...

Question 8

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 (CdF2) will precipitate until the solution reaches saturation because the addition of NaF increases the concentration of fluoride ions in the solution, potentially exceeding the solubility product (Ksp) for CdF2. This does not increase the solubility of CdF2 nor does it involve the solubility of cadmium nitrate in the context of precipitation.

Question 9

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 10

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

The equilibrium constant (Kf) for the formation of Co(OH)4^- from Co2+ and OH^- is given as 5.0 × 10^19. When 4.50 mol of NaOH is added to 1.00 L of 1.00 M Co(NO3)2, the initial concentration of OH^- will be 4.50 M. The reaction will proceed until the equilibrium is established according to the Kf value. Since Kf is very large, it indicates that the reaction proceeds almost to completion, forming Co(OH)4^- and consuming Co2+ and OH^- ions. The equilibrium concentration of Co2+ ions can be calculated using the stoichiometry of the reaction and the Kf value, leading to a very low concentration of cobalt ions, consistent with the choice that indicates a concentration of 3.2 × 10^-19 M.

Question 11

Consider the dissolution of MnS in water (K_sp = 3.0 × 10⁻¹⁴). MnS(s) + H₂O(l) ⇄ Mn²⁺(aq) + HS⁻(aq) + OH⁻(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Accepted Answer

The addition of aqueous potassium hydroxide will increase the concentration of hydroxide ions in the system, which will increase the formation of the insoluble sulfide ion. This will shift the equilibrium to the left, decreasing the solubility of manganese(II) sulfide.

Question 12

Calculate the solubility of zinc hydroxide, Zn(OH)₂, in 1.00 M NaOH. K_sp = 3.0 × 10⁻¹⁶ for Zn(OH)₂, Kf = 3.0 × 10¹⁵ for Zn(OH)₄²⁻

Accepted Answer

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

Question 13

A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO₃)₂with 50.0 mL of 0.50 M Co(NO₃)₂. Sodium hydroxide is added to the mixture. Which hydroxide precipitates first and what concentration of hydroxide ions present in solution will accomplish the separation? K_sp = 2.2 × 10⁻²⁰ for Cu(OH)₂, K_sp = 1.3 × 10⁻¹⁵for Co(OH)₂

Accepted Answer

The correct answer is D because the Ksp value for Cu(OH)2 is smaller than that for Co(OH)2, indicating that Cu(OH)2 is less soluble and will precipitate first. The concentration of hydroxide ions required to precipitate Cu(OH)2 can be calculated using the Ksp expression:Ksp = [Cu2+][OH-]22.2 × 10^-20 = [Cu2+][OH-]2[OH-] = 1.1 × 10^-9 M

Question 14

The salts X(NO₃)₂and Y(NO₃)₂ (where X⁺ and Y⁺ are metal ions) are dissolved in water to give a solution which is 0.1 M in each of them. Using the K_sp values listed below, decide which aqueous reagent, if any, will definitely precipitate X⁺ before precipitating Y⁺ from solution. Given K_spvalues:XCl₂, 1 × 10⁻⁵YCl₂, 1 × 10⁻¹⁰X(OH)₂, 1 × 10⁻¹⁰Y(OH)₂, 1 × 10⁻⁵

Accepted Answer

To determine which reagent will definitely precipitate X before Y, we need to compare the Ksp values of their respective salts. The larger the Ksp value, the more soluble the salt is and the less likely it is to precipitate.
Comparing the Ksp values of X and Y:
Ksp of X(NOS1U1B13S1U1B0)S1U1B12S1U1B0 = 1 × 10S1U1P1−S1S1P0S1U1P110 S1S1P0
Ksp of Y(NOS1U1B13S1U1B0)S1U1B12S1U1B0S1U1B0 = 1 × 10S1U1P1−S1S1P0S1U1P15S1S1P0
Since the Ksp value of X is larger, it is less likely to precipitate than Y. Therefore, we need to find a reagent that will precipitate X but not Y.
Looking at the given reagents:
A) 1 M NaCl will not precipitate either X or Y, as both salts are soluble in NaCl.
B) 1 M HCl will not precipitate X, as X does not contain OH-. However, it will also precipitate Y as both Cl- and OH- ions are present in the solution.
C) 1 M HNO3 will not precipitate X or Y, as neither salt contains NO3-.
D) 1 M NaOH will precipitate X, as it contains OH- which will react with X to form a precipitate of X(OH)2. However, it will not precipitate Y, as Y does not contain OH-.
E) None of the given choices will only precipitate X without precipitating Y.
Therefore, the best choice(s) is D, 1 M NaOH, which will precipitate X before Y.

Quiz 19: Ionic Equilibria in Aqueous Systems

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

Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (K_sp for Ag₂CO₃ = 8.1 x 10^-12)

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?

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.

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⁻

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⁻

Consider the dissolution of MnS in water (K_sp = 3.0 × 10⁻¹⁴) . MnS(s) + H₂O(l) ⇄ Mn²⁺(aq) + HS⁻(aq) + OH⁻(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH. K_sp = 3.0 × 10⁻¹⁶ for Zn(OH) ₂, Kf = 3.0 × 10¹⁵ for Zn(OH) ₄²⁻

Quiz 19: Ionic Equilibria in Aqueous Systems

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.

Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (Ksp for Ag2CO3 = 8.1 x 10-12)

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?

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.

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−

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−

Consider the dissolution of MnS in water (Ksp = 3.0 × 10−14) . MnS(s) + H2O(l) ⇄ Mn2+(aq) + HS−(aq) + OH−(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Calculate the solubility of zinc hydroxide, Zn(OH) 2, in 1.00 M NaOH. Ksp = 3.0 × 10−16 for Zn(OH) 2, Kf = 3.0 × 1015 for Zn(OH) 42−

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

Calculate the molar solubility of silver carbonate in 1.0 M sodium carbonate solution. (K_sp for Ag₂CO₃ = 8.1 x 10^-12)

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?

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.

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⁻

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⁻

Consider the dissolution of MnS in water (K_sp = 3.0 × 10⁻¹⁴) . MnS(s) + H₂O(l) ⇄ Mn²⁺(aq) + HS⁻(aq) + OH⁻(aq) How is the solubility of manganese(II) sulfide affected by the addition of aqueous potassium hydroxide to the system?

Calculate the solubility of zinc hydroxide, Zn(OH) ₂, in 1.00 M NaOH. K_sp = 3.0 × 10⁻¹⁶ for Zn(OH) ₂, Kf = 3.0 × 10¹⁵ for Zn(OH) ₄²⁻