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It's part k and calculation 0.4067×0.4067=0.165
also I dont understand questions 1-4

k. Calculate the Ksp of KHP in 0.5 M KCl solution. Is there a difference between the Ksp in 0.5 M KCl and the Ksp in purified


4a. Look up the Ksp for Mn(OH)2 and provide the reference: 1.6 X10 reference: /.6 X10-13 Reference b. The pH of a saturated s

Questions 1. Use Le Chateliers principle to explain why the solubility of KHP when dissolved in 0.5 M KCI is less than the s

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Answer #1

Question 4.

Part a.

Literature Ksp of Mn(OH)2 = 1.6*10-13

Part b.

pH = 9.9, i.e. pOH = 14-9.9 = 4.1

i.e. [OH-] = 10-4.1 M = 7.94*10-5 M

[Mn2+] = [OH-]/2 = 1/2 * 7.94*10-5 M = 3.97*10-5 M

Now, Ksp of Mn(OH)2 = [Mn2+][OH-]2

i.e. Ksp = 4*(3.97*10-5)3 = 2.5*10-13

Part c.

Calculated Ksp (2.5*10-13) > literature Ksp (1.6*10-13)

The two values are close.

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