Question

Determine the concentration of Cu2+ and OH- present in a saturated Cu(OH)2 solution. Will the solubility...

Determine the concentration of Cu2+ and OH- present in a saturated Cu(OH)2 solution. Will the solubility change with the addition of acid? If so, will it increase or decrease?

Homework Answers

Answer #1

i) Solubility equillibrium of Cu(OH)2 is

Cu(OH)2(s) <------> Cu2+(aq) + 2OH-(aq)

Ksp = [Cu2+][OH-]2 = 2.20×10-20M2

If solubility of Cu(OH)2 is represented as S

[Cu2+] = S

[OH-] = 2S

Therefore,

S × (2S)2 = 2.20×10-20

4S3 = 2.20×10-20

S = 1.77×10-7

Therefore,

[Cu2+] = 1S= 1.77×10-7M

[OH-] = 2S = 3.54×10-7M

ii) Yes, Solubility will change with addition of acid

Solubility will increase with addition of acid

the OH- ion react with H+ ion so, the equillbrium will shift to the right.Thus the solubility of Cu(OH)2 increase with the addition of acid.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
What is the minimum concentration of Cu2+ required to begin precipitating Cu(OH)2(s) in a solution of...
What is the minimum concentration of Cu2+ required to begin precipitating Cu(OH)2(s) in a solution of pH 10.77? For Cu(OH)2, Ksp= 2.6 x 10–19.
2. For half-cell B, when NaOH(aq) is added to Cu2+(aq), a sparingly soluble solid, Cu(OH)2, will...
2. For half-cell B, when NaOH(aq) is added to Cu2+(aq), a sparingly soluble solid, Cu(OH)2, will form. a. Write the reaction for the formation of Cu(OH)2. The Ksp for Cu(OH)2 is 4.8 x 10^-20. b. Interpret the magnitude of Ksp. When NaOH(aq) is added to Cu2+(aq), what will happen to the "free" [Cu2+]? Choose one. [Cu2+] will increase [Cu2+] will decrease [Cu2+] will not change cannot be predicted. c. After the nearly insoluble solid forms, the next step in the...
What range of pH would permit the selective precipitation of Cu2+ as Cu(OH)2 from a solution...
What range of pH would permit the selective precipitation of Cu2+ as Cu(OH)2 from a solution that contains 0.088 M Cu2+ and 0.088 M Mn2+? For Mn(OH)2, Ksp = 1.6 × 10-13, and for Cu(OH)2, Ksp = 4.8 × 10-20. When pH = _____ – _____ Mn(OH)2 will be soluble, but some Cu(OH)2 will precipitate out of solution.
What is the pH of a saturated solution of Ni(OH)2 ? pH= What is the solubility...
What is the pH of a saturated solution of Ni(OH)2 ? pH= What is the solubility in grams of Ni(OH)2 /100 mL of solution? Solubility = g/100 mL
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL)...
Question Molar Solubility and solubility Product of Calcium Hydroxide: 1. Volume of Saturated Ca(OH)2 solution (mL) = 25.0 mL 2. Concentration of Standardized HCL solution (mol/L) = 0.05 mol/L 3. Buret reading, initial (mL) = 50.0 mL 4. Buret reading, final (mL) = 32.5 mL 5. Volume of HCL added (mL) = 17.5 mL 6. Moles of HCL added (mol) = (concentration of HCl)(Volume of HCl) = (0.05)(19.1) = 0.875 mol. 7.Moles of OH- in saturated solution (mol)=8.75x10^-4 8.the [OH-]...
1) The hydroxide ion concentration of a saturated solution of Fe(OH)2 is 1.6X10^-5M. What is the...
1) The hydroxide ion concentration of a saturated solution of Fe(OH)2 is 1.6X10^-5M. What is the solubility product constant for Fe(OH)2? 2)What is the Kb for the following equilibrium? Ka for HNO2 is 5.0X10^-4.; No2- + H2O --> HNO2 + OH-
A student measures the OH- concentration in a saturated aqueous solution of calcium hydroxide to be...
A student measures the OH- concentration in a saturated aqueous solution of calcium hydroxide to be 2.56×10-2 M.   Based on her data, the solubility product constant for calcium hydroxide is
What is the pH of a saturated solution of Ca(OH)2 if the solubility of calcium hydroxide...
What is the pH of a saturated solution of Ca(OH)2 if the solubility of calcium hydroxide is 1.50 g/L?
1. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved Ca(OH)2...
1. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved Ca(OH)2 solid on the bottom of the test tube. If you add an additional scope of Ca(OH)2 to this solution will the concentration of [OH-] in the solution increase, decrease, of be unchanged? (Briefly explain and assume we let the solution reach equilibrium again) 2. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved Ca(OH)2 solid on the bottom of...
A group of students conducted a titration of 25.00-mL saturated Ca(OH)2 solution with 0.0480M HCl. The...
A group of students conducted a titration of 25.00-mL saturated Ca(OH)2 solution with 0.0480M HCl. The students found that 10.10-mL of acid was required to reach the equivalence point. Calculate the molar concentration of OH- and Ca2+, the molar solubility, and Ksp of the analyte. Show detailed calculation for each. [OH-] in the analyte: [Ca2+] in the analyte: molar solubility of Ca(OH)2: Ksp of Ca(OH)2: