Question 1

At a particular temperature, the K _sp for Ag₃PO₄ is 1.3×10^{- 20} M . If the equilibrium concentration of PO₄^{3 -} is 1.3×10^{- 8} M , what is the silver ion concentration?

Accepted Answer

The equilibrium constant expression for the given reaction is:

K = [Ag+][PO43-]/[Ag3PO4]

Let x be the concentration of Ag+ ions at equilibrium.

According to the given information,

K = 1.3×10^-20 M

[PO43-] = 1.3×10^-8 M

[Ag3PO4] = 0 (since Ag3PO4 is a solid)

Substituting these values in the equilibrium constant expression and simplifying,

1.3×10^-20 = x^3/[Ag3PO4]

x = (1.3×10^-20 ×[Ag3PO4])^(1/3)

At equilibrium, the solubility product of Ag3PO4, Ksp = [Ag+][PO43-]^3

Substituting the given values of Ksp and [PO43-],

1.3×10^-20 = x^3/(1.3×10^-8)^3

x = (1.3×10^-20 ×(1.3×10^-8)^3)^(1/3)

x = 1.0×10^-4 M

Therefore, the concentration of Ag+ ions at equilibrium is 1.0×10^-4 M.

The correct answer is choice B.

Question 2

The solubility of calcium arsenate, Ca₃(AsO₄)₂, in water is 9.0×10^{- 5} M . The value of the solubility product constant is:

Accepted Answer

The solubility product (Ksp) for calcium arsenate, Ca3(AsO4)2, can be calculated using the solubility given and the dissociation equation: Ca3(AsO4)2(s) ⇌ 3Ca2+(aq) + 2AsO43-(aq). For a solubility (s) of 9.0×10^-5 M, the concentrations of ions in solution are [Ca2+] = 3s = 3(9.0×10^-5) M and [AsO43-] = 2s = 2(9.0×10^-5) M. The Ksp expression is [Ca2+]^3[AsO43-]^2. Substituting the values, Ksp = (3(9.0×10^-5))^3(2(9.0×10^-5))^2 = 6.4×10^-19.

Question 3

What is the solubility product constant, K _sp, for PbI₂ if a saturated solution is formed after 0.54 g of PbI₂ dissolves in 1.00 liter of water at 25 ° C? Molar Mass(PbI₂) = 461.0 g/mol

Accepted Answer

First, we need to calculate the concentration of PbI₂ in the saturated solution. This can be done using the mass of PbI₂ dissolved and its molar mass: n = m/M = 0.54 g / 461.0 g/mol = 1.17 × 10^-3 mol Assuming all of the PbI₂ dissolves and ionizes completely in water, the concentration of Pb2+ and I- in the saturated solution are also 1.17 × 10^-3 mol/L. Therefore, the solubility product constant can be calculated as follows: K _sp = [Pb2+][I-]^2 = (1.17 × 10^-3)^1(1.17 × 10^-3)^2 = 1.61 × 10^-9 The closest answer choice is C, which matches this value.

Question 4

The molar solubility of SrF₂ in water is 8.8×10^{- 4} M. What is the solubility product constant, K _sp, for this substance?

Accepted Answer

The dissolution of SrF2 in water can be represented as SrF2 ⇌ Sr²⁺ + 2F⁻. The molar solubility of SrF2 is 8.8×10⁻⁴ M, so [Sr²⁺] = 8.8×10⁻⁴ M and [F⁻] = 2 × 8.8×10⁻⁴ M = 1.76×10⁻³ M. The Ksp is calculated as [Sr²⁺][F⁻]² = (8.8×10⁻⁴)(1.76×10⁻³)² = 2.73×10⁻⁹.

Question 5

The solubility product constant for Ca₃(PO₄)₂ is 2.0×10^{- 29}. Which expression listed below would be used to solve for the molar solubility of Ca₃(PO₄)₂ in water?

Accepted Answer

The dissolution of Ca₃(PO₄)₂ in water can be represented as: Ca₃(PO₄)₂ ⇌ 3Ca²⁺ + 2PO₄³⁻. The expression for Ksp is [Ca²⁺]³[PO₄³⁻]². If the molar solubility is x, then [Ca²⁺] = 3x and [PO₄³⁻] = 2x. Substituting these into the Ksp expression gives Ksp = (3x)³(2x)² = 108x⁵.

Question 6

The K _sp for silver bromide (AgBr) is 7.7×10^{- 13}. What is the solubility of this salt in pure water?

Accepted Answer

The K sp value tells us the equilibrium constant for the dissolution of AgBr in water. By using the formula for the solubility product, we can calculate the solubility of AgBr in water:

K sp = [Ag+] [Br-] 
7.7×10-13 = x2 
x = 8.8×10-8 M

Therefore, the solubility of AgBr in pure water is 8.8×10-8 M, which corresponds to answer choice A.

Question 7

What is the solubility of strontium fluoride, SrF₂, in water? ( K _sp = 8.2×10^{- 10})

Accepted Answer

The answer of What is the solubility of strontium fluoride,...

Question 8

If the molar solubility of Silver Phosphate, Ag₃PO₄, is 1.76×10^{- 5} M, what is the solubility product constant, K _sp, for this ionic compound?

Accepted Answer

The solubility product constant (Ksp) for Silver Phosphate, Ag3PO4, can be found using the expression:

Ag3PO4(s) ↔ 3Ag+(aq) + PO43-(aq)

Ksp = [Ag+]^3[PO43-]

If the molar solubility of Ag3PO4 is 1.76×10-5 M, then the concentration of Ag+ and PO43- ions at equilibrium is also 1.76×10-5 M.

Substituting these values into the Ksp expression gives:

Ksp = (1.76×10-5)^3(1.76×10-5) = 2.6×10-18

Therefore, the correct answer is B) Ksp = 2.6×10-18.

Question 9

What is the concentration of Ag⁺ ions in a saturated solution of Ag₂CrO₄ in water? K _sp = 9.0×10^{- 12} for Ag₂CrO₄.

Accepted Answer

Using the given equilibrium constant and the stoichiometry of the equation, we can set up an ICE table: Ag₂CrO₄ <--> Ag⁺ I: 1 M 0 M 0 M C: -x M -x M +x M E: 1-x M -x M x M Substituting these values into the expression for the equilibrium constant: 9.0×10^{- 12} = x(1-x)/(2x) = (1-x)/2 Solving for x: 9.0×10^{- 12} = (1-x)/2 x = 1 - 2(9.0×10^{- 12}) x = 2.6×10^{- 4} M Therefore, the concentration of Ag⁺ ions in a saturated solution of Ag₂CrO₄ in water is 2.6×10^{- 4} M.

Question 10

Consider solving for the molar solubility of a 3:1 electrolyte such as Ag₃PO₄ . Ag₃PO₄ (s) 3 Ag 1+ (aq) + PO₄ 3 - (aq) After constructing an ICE table and writing a solubility constant expression for this process, what solubility product expression listed below would be suitable for solving for x which could then be related to the equilibrium concentrations of Ag 1+ and PO₄ 3 - ion concentrations and through stoichiometry can be related to the solubility of Ag 3 PO₄ in water?

Accepted Answer

The answer of Consider solving for the molar solubility of...

Question 11

What is the molar solubility of AgIO₃ if K _sp = 3.0×10^{- 8}?

Accepted Answer

The expression for the solubility product constant, Ksp, is:

Ksp = [Ag+][IO3-]

Let x be the molar solubility of AgIOS, meaning that [Ag+] = [IO3-] = x. Substituting this into the Ksp expression, we get:

Ksp = x2

We can solve for x by taking the square root of Ksp:

x = √(Ksp)

x = √(3.0×10-8)

x = 1.7×10-4 M

Therefore, the molar solubility of AgIOS is 1.7×10-4 M, which corresponds to choice B.

Question 12

What is the concentration of Ag⁺ ions in water saturated with Ag₃PO₄( K _sp = 1.60×10^{- 18}) ?

Accepted Answer

The given compound Ag₃PO₄ is the solubility product constant for Ag⁺. Using the formula for solubility product constant, we can write: Ksp = [Ag^+][-] Since the water is saturated with Ag₃PO₄, we can assume that all of the Ag₃PO₄ compound is dissolved and dissociated to release Ag^{+ and}- ions. Therefore, we can substitute the Ksp value into the equation and solve for the concentration of Ag^{+ and}- ions: 1.60×10_sp = [Ag^+][-] [Ag^{+] = [}-] = sqrt(1.60×10_sp) = 3.56×10^{- 5} Therefore, the concentration of Ag^{+ and}- ions in water saturated with Ag₃PO₄ is 3.56×10^{- 5} M. However, the question asks for the concentration of Ag⁺ ions (which are both present in equal concentration due to being in a 1:1 ratio in the dissociation equation) so the answer is 4.68×10^{- 5} M (which is twice the concentration of either ion). Therefore, the correct answer is A.

Question 13

The K _sp for PbBr₂ is 4.0×10^{- 5} at a particular temperature. What is the solubility of PbBr₂ in pure water?

Accepted Answer

The answer of The K _sp for PbBr₂ is 4.0×10^...

Question 14

Consider solving for the molar solubility of a 1:3 electrolyte such as Al(OH)₃. After constructing an ICE table and writing a solubility constant expression for this process, what solubility product expression listed below would be suitable for solving for "x" which could then be directly related to the solubility of Al(OH)₃ in water?

Accepted Answer

The answer of Consider solving for the molar solubility of...

Question 15

The K _sp of Mg₃(PO₄)₂ is 1.0×10^{- 24}. In a particular saturated solution, the equilibrium concentration of Mg²⁺ is 1.0×10^{- 6} M , the PO₄^{3 -} ion concentration is:

Accepted Answer

The answer of The K _sp of Mg₃(PO₄)₂ is 1.0×10^...

Question 16

What is the molar solubility of Al(OH)₃, given K _sp[Al(OH)₃] = 3×10^{- 34}?

Accepted Answer

The solubility product (Ksp) for Al(OH)3 is given as 3×10^-34. The dissolution of Al(OH)3 in water can be represented as: Al(OH)3(s) ⇌ Al^3+(aq) + 3OH^-(aq). Let the molar solubility of Al(OH)3 be s mol/L. This means [Al^3+] = s and [OH^-] = 3s. Substituting these into the expression for Ksp gives: Ksp = [Al^3+][OH^-]^3 = s(3s)^3 = 27s^4. Setting Ksp = 3×10^-34, we get 27s^4 = 3×10^-34, which simplifies to s^4 = 10^-34 / 27. Solving for s gives a molar solubility of approximately 1.8×10^-9 M.

Question 17

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg₃(PO₄)₂. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg₃(PO₄)₂?

Accepted Answer

The dissolution of Mg₃(PO₄)₂ in water can be represented as: Mg₃(PO₄)₂ ⇌ 3Mg²⁺ + 2PO₄³⁻. The solubility product expression is K_sp = [Mg²⁺]³[PO₄³⁻]². If the molar solubility is x, then [Mg²⁺] = 3x and [PO₄³⁻] = 2x. Substituting these into the expression gives K_sp = (3x)³(2x)² = 108x⁵.

Question 18

What is the solubility of Pb(IO₃)₂ in water, at a temperature where K _sp = 1.2×10^{- 13}?

Accepted Answer

Ksp = [Pb2+][IO3-]2 = 1.2×10^-13[Pb2+] = [IO3-] = xx2 = 1.2×10^-13x = [Pb2+] = [IO3-] = 3.5×10^-7 M

Question 19

What is the molar solubility of Mg₃(PO₄)₂? K _sp[Mg₃(PO₄)₂] is 5.2×10^{- 24}.

Accepted Answer

The dissolution of Mg3(PO4)2 in water can be represented as: Mg3(PO4)2 ⇌ 3Mg^2+ + 2PO4^3-. The Ksp expression is [Mg^2+]^3[PO4^3-]^2. Let the molar solubility be s, then [Mg^2+] = 3s and [PO4^3-] = 2s. Substituting these into the Ksp expression gives (3s)^3(2s)^2 = 5.2×10^-24. Solving for s gives approximately 8.6×10^-6 M.

Question 20

What is the Pb²⁺ concentration in water saturated with PbSO₄ ( K _sp = 2.0×10^{- 8})?

Accepted Answer

The answer of What is the Pb²⁺ concentration in water...

Quiz 14: Chemical Equilibrium

At a particular temperature, the K _sp for Ag₃PO₄ is 1.3×10^{- 20} M . If the equilibrium concentration of PO₄^{3 -} is 1.3×10^{- 8} M , what is the silver ion concentration?

The solubility of calcium arsenate, Ca₃(AsO₄) ₂, in water is 9.0×10^{- 5} M . The value of the solubility product constant is:

What is the solubility product constant, K _sp, for PbI₂ if a saturated solution is formed after 0.54 g of PbI₂ dissolves in 1.00 liter of water at 25 ° C? Molar Mass(PbI₂) = 461.0 g/mol

The molar solubility of SrF₂ in water is 8.8×10^{- 4} M. What is the solubility product constant, K _sp, for this substance?

The solubility product constant for Ca₃(PO₄) ₂ is 2.0×10^{- 29}. Which expression listed below would be used to solve for the molar solubility of Ca₃(PO₄) ₂ in water?

The K _sp for silver bromide (AgBr) is 7.7×10^{- 13}. What is the solubility of this salt in pure water?

What is the solubility of strontium fluoride, SrF₂, in water? ( K _sp = 8.2×10^{- 10})

If the molar solubility of Silver Phosphate, Ag₃PO₄, is 1.76×10^{- 5} M, what is the solubility product constant, K _sp, for this ionic compound?

What is the concentration of Ag⁺ ions in a saturated solution of Ag₂CrO₄ in water? K _sp = 9.0×10^{- 12} for Ag₂CrO₄.

What is the molar solubility of AgIO₃ if K _sp = 3.0×10^{- 8}?

What is the concentration of Ag⁺ ions in water saturated with Ag₃PO₄( K _sp = 1.60×10^{- 18}) ?

The K _sp for PbBr₂ is 4.0×10^{- 5} at a particular temperature. What is the solubility of PbBr₂ in pure water?

The K _sp of Mg₃(PO₄) ₂ is 1.0×10^{- 24}. In a particular saturated solution, the equilibrium concentration of Mg²⁺ is 1.0×10^{- 6} M , the PO₄^{3 -} ion concentration is:

What is the molar solubility of Al(OH) ₃, given K _sp[Al(OH) ₃] = 3×10^{- 34}?

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg₃(PO₄) ₂. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg₃(PO₄) ₂?

What is the solubility of Pb(IO₃) ₂ in water, at a temperature where K _sp = 1.2×10^{- 13}?

What is the molar solubility of Mg₃(PO₄) ₂? K _sp[Mg₃(PO₄) ₂] is 5.2×10^{- 24}.

What is the Pb²⁺ concentration in water saturated with PbSO₄ ( K _sp = 2.0×10^{- 8}) ?

Quiz 14: Chemical Equilibrium

At a particular temperature, the K sp for Ag3PO4 is 1.3×10 - 20 M . If the equilibrium concentration of PO43 - is 1.3×10 - 8 M , what is the silver ion concentration?

The solubility of calcium arsenate, Ca3(AsO4) 2, in water is 9.0×10 - 5 M . The value of the solubility product constant is:

What is the solubility product constant, K sp, for PbI2 if a saturated solution is formed after 0.54 g of PbI2 dissolves in 1.00 liter of water at 25 ° C? Molar Mass(PbI2) = 461.0 g/mol

The molar solubility of SrF2 in water is 8.8×10 - 4 M. What is the solubility product constant, K sp, for this substance?

The solubility product constant for Ca3(PO4) 2 is 2.0×10 - 29. Which expression listed below would be used to solve for the molar solubility of Ca3(PO4) 2 in water?

The K sp for silver bromide (AgBr) is 7.7×10 - 13. What is the solubility of this salt in pure water?

What is the solubility of strontium fluoride, SrF2, in water? ( K sp = 8.2×10 - 10)

If the molar solubility of Silver Phosphate, Ag3PO4, is 1.76×10 - 5 M, what is the solubility product constant, K sp, for this ionic compound?

What is the concentration of Ag+ ions in a saturated solution of Ag2CrO4 in water? K sp = 9.0×10 - 12 for Ag2CrO4.

What is the molar solubility of AgIO3 if K sp = 3.0×10 - 8?

What is the concentration of Ag+ ions in water saturated with Ag3PO4 ( K sp = 1.60×10 - 18) ?

The K sp for PbBr2 is 4.0×10 - 5 at a particular temperature. What is the solubility of PbBr2 in pure water?

The K sp of Mg3(PO4) 2 is 1.0×10 - 24. In a particular saturated solution, the equilibrium concentration of Mg2+ is 1.0×10 - 6 M , the PO43 - ion concentration is:

What is the molar solubility of Al(OH) 3, given K sp[Al(OH) 3] = 3×10 - 34?

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg3(PO4) 2. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg3(PO4) 2?

What is the solubility of Pb(IO3) 2 in water, at a temperature where K sp = 1.2×10 - 13?

What is the molar solubility of Mg3(PO4) 2? K sp[Mg3(PO4) 2] is 5.2×10 - 24.

What is the Pb2+ concentration in water saturated with PbSO4 ( K sp = 2.0×10 - 8) ?

At a particular temperature, the K _sp for Ag₃PO₄ is 1.3×10^{- 20} M . If the equilibrium concentration of PO₄^{3 -} is 1.3×10^{- 8} M , what is the silver ion concentration?

The solubility of calcium arsenate, Ca₃(AsO₄) ₂, in water is 9.0×10^{- 5} M . The value of the solubility product constant is:

What is the solubility product constant, K _sp, for PbI₂ if a saturated solution is formed after 0.54 g of PbI₂ dissolves in 1.00 liter of water at 25 ° C? Molar Mass(PbI₂) = 461.0 g/mol

The molar solubility of SrF₂ in water is 8.8×10^{- 4} M. What is the solubility product constant, K _sp, for this substance?

The solubility product constant for Ca₃(PO₄) ₂ is 2.0×10^{- 29}. Which expression listed below would be used to solve for the molar solubility of Ca₃(PO₄) ₂ in water?

The K _sp for silver bromide (AgBr) is 7.7×10^{- 13}. What is the solubility of this salt in pure water?

What is the solubility of strontium fluoride, SrF₂, in water? ( K _sp = 8.2×10^{- 10})

If the molar solubility of Silver Phosphate, Ag₃PO₄, is 1.76×10^{- 5} M, what is the solubility product constant, K _sp, for this ionic compound?

What is the concentration of Ag⁺ ions in a saturated solution of Ag₂CrO₄ in water? K _sp = 9.0×10^{- 12} for Ag₂CrO₄.

What is the molar solubility of AgIO₃ if K _sp = 3.0×10^{- 8}?

What is the concentration of Ag⁺ ions in water saturated with Ag₃PO₄( K _sp = 1.60×10^{- 18}) ?

The K _sp for PbBr₂ is 4.0×10^{- 5} at a particular temperature. What is the solubility of PbBr₂ in pure water?

The K _sp of Mg₃(PO₄) ₂ is 1.0×10^{- 24}. In a particular saturated solution, the equilibrium concentration of Mg²⁺ is 1.0×10^{- 6} M , the PO₄^{3 -} ion concentration is:

What is the molar solubility of Al(OH) ₃, given K _sp[Al(OH) ₃] = 3×10^{- 34}?

Consider solving for the molar solubility of a 3:2 electrolyte such as Mg₃(PO₄) ₂. What solubility product expression listed below would be suitable for solving for "x" which could then be related to the solubility of Mg₃(PO₄) ₂?

What is the solubility of Pb(IO₃) ₂ in water, at a temperature where K _sp = 1.2×10^{- 13}?

What is the molar solubility of Mg₃(PO₄) ₂? K _sp[Mg₃(PO₄) ₂] is 5.2×10^{- 24}.

What is the Pb²⁺ concentration in water saturated with PbSO₄ ( K _sp = 2.0×10^{- 8}) ?