A lab technician adds 0.040 mol of KOH to 1.00 L of 0.0010 M Ca(NO3)2. Ksp = 6.5

Question

A lab technician adds 0.040 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)Calcium hydroxide precipitates until the solution is saturated.

b)The solution is unsaturated and no precipitate forms.

c)The concentration of calcium ions is reduced by the addition of the hydroxide ions.

d)One must know Ksp for calcium nitrate to make meaningful predictions on this system.

e)The presence of KOH will raise the solubility of Ca(NO3)2.

and please explain the answer

Explanation / Answer

b)The solution is unsaturated and no precipitate forms.

explanation:

[OH-] = 0.040 M

[Ca+2] = 0.001 M

Ca(OH)2 -----------------> Ca+2 + 2OH-

ionic product = [Ca+2][OH-]^2

                     = 0.001 x (0.04)^2

                   = 1.6 x 10^-6

ionic product < Ksp . so there is no precipitate is formed .

if ionic product exceeds solubility product there will be precipitate is formed

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