Mg(OH)2 is a sparingly soluble salt with a solubility product constant, Ksp, of 5.61×10−11. It is...

Mg(OH)2 is a sparingly soluble salt with a solubility product constant, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.150 mol L−1 NaOH solution.

Expert Solution

If you have any query please comment

If you satisfied with the solution please like it thankxx

queen_honey_blossom answered 2 years ago

Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used...

Mg(OH)2 is a sparingly soluble salt with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. What is the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2dissolved in a 0.160 M NaOH solution? Express your answer numerically as the ratio of molar solubility in H2O to the molar solubility in NaOH.

Mg(OH)2 is a sparingly soluble compound, in this case a base, with a solubility product, Ksp,...

Mg(OH)2 is a sparingly soluble compound, in this case a base, with a solubility product, Ksp, of 5.61×10−11. It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Part A: Based on the given value of the Ksp, calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.160 M NaOH solution. Part B: What is the pH change of a 0.300 M solution of...

Mg(OH ) 2 is a sparingly soluble compound, in this case a base, with a solubility...

Mg(OH ) 2 is a sparingly soluble compound, in this case a base, with a solubility product, K sp , of 5.61× 10 −11 . It is used to control the pH and provide nutrients in the biological (microbial) treatment of municipal wastewater streams. Part C - Calculate how many times more soluble Mg(OH)2 is in pure water Based on the given value of the Ksp , calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2...

Cadmium hydroxide (Cd(OH)2) is a sparingly soluble salt with a Ksp value of 7.2 x 10-15....

Cadmium hydroxide (Cd(OH)2) is a sparingly soluble salt with a Ksp value of 7.2 x 10-15. a) What is the solubility of Cd(OH)2 in pure water? b) What is the solubility of Cd(OH)2 in a solution that is buffered to a pH of 4.60? c) Cadmium forms the complex ion [Cd(CN)4]2- with a Kf value of 3 x 1018. What is the solubility of Cd(OH)2 in a 0.100 M NaCN solution?

Use the solubility-product constant for Cr (OH) 3 ( Ksp = 6.7×10?31) and the formation constant...

Use the solubility-product constant for Cr (OH) 3 ( Ksp = 6.7×10?31) and the formation constant for Cr (OH) ?4 from the following table to determine the concentration of Cr (OH) ?4 in a solution that is buffered at pH= 11 and is in equilibrium with solid Cr (OH) 3. Table Formation Constants for Some Metal Complex Ions in Water at 25 ?C Complex Ion Kf Equilibrium Equation Ag(NH3)+2 1.7×107 Ag+(aq)+2NH3(aq)?Ag(NH3)+2(aq) Ag(CN)?2 1×1021 Ag+(aq)+2CN?(aq)?Ag(CN)?2(aq) Ag(S2O3)3?2 2.9×1013 Ag+(aq)+2S2O2?3(aq)?Ag(S2O3)3?2(aq) CdBr2?4 5×103 Cd2+(aq)+4Br?(aq)?CdBr2?4(aq)...

Q1. Assume the solubility product of Mg(OH)2 is 2.2 × 10−11 at a certain temperature. What...

Q1. Assume the solubility product of Mg(OH)2 is 2.2 × 10−11 at a certain temperature. What minimum OH− concentration must be attained (for example, by adding NaOH) to decrease the Mg2+concentration in a solution of Mg(NO3)2 to less than 1.1 × 10−10 M Q2. Calculate the molar solubility of AgBr in a 2.2 M NH3 solution. Q3.Calculate the molar solubility of AgBr in a 2.0 M NH3 solution. Q4. A 10.0−mL solution of 0.360 M NH3 is titrated with a...

The solubility of Mg(OH)2 in water is approximately 9 mg/L. (a) Calculate the Ksp of magnesium...

The solubility of Mg(OH)2 in water is approximately 9 mg/L. (a) Calculate the Ksp of magnesium hydroxide. (b) Calculate the hydroxide concentration needed to precipitate Mg2+ ions such that no more than 5.0 μg/L Mg2+ remains in solution. (c) Calculate the maximum concentration of Mg2+ (as M) that can exist in a solution of pH = 12.

Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in...

Based on the given value of the Ksp, what is the molar solubility of Mg(OH)2 in 0.160 M NaOH? Express your answer with the appropriate units. Calculate how many times more soluble Mg(OH)2 is in pure water Based on the given value of the Ksp, calculate the ratio of solubility of Mg(OH)2 dissolved in pure H2O to Mg(OH)2 dissolved in a 0.160 M NaOH solution. Express your answer numerically to three significant figure Ksp, of 5.61×10−11.

1. Write the solubility equilibrium and the solubility product expression for the following sparingly soluble salts....

1. Write the solubility equilibrium and the solubility product expression for the following sparingly soluble salts. CaCO3 Cu2S Sb2S3 2. The solubility of silver bromide, AgBr, at 25

(a) The solubility product, Ksp, of Sn(OH)4(s) is 1.0 x 10-57. What is its solubility (in...

(a) The solubility product, Ksp, of Sn(OH)4(s) is 1.0 x 10-57. What is its solubility (in g/L) in an aqueous solution of NaOH with a pH of 12.80 ? The temperature is 25oC. (b) For the reaction 2 A(g) ⇋ 3 B(g) + 2 C(g), we start off with just pure A(g) (there is no B(g) or C(g)). When we reach equilibrium, the partial pressure of C(g) is 4.19 atm. The equilibrium constant for this reaction is 8.39 . What...

Question