c. Calculate the Ksp value for Ca(OH)2 using this data. 5.86x10-* You are correc

Question

c. Calculate the Ksp value for Ca(OH)2 using this data. 5.86x10-* You are correct. Your recei 163-8364PreviousTries d. Calculate the pKsp value for Ca(OH)2(s) using this data 5.23 You are correct. Your receipt no. is 163-798 Previous Tries 4. In this experiment, you will also examine the solubility of Ca(OH)2(s) in a 0.200 M CaCl2 solution. a. Will the solubility of Ca(OH)2(s) in 0.200 M CaCl2 be equal to, smaller than, or larger than the solubility you calculated in question 3b? Incorrect equal to Correct: smaller than Incorrect larger thar You are correct. Your receipt no. is 163-65650 Previous Tries b. Using your calculated Ksp value from your answer to 3c, calculate the Ca(OH)2 solubility (grams per liter) in a 0.200 M CaCl2 solution g/L Tries 0/99 Submit Answer

Explanation / Answer

4b)

CaCl2 here is Strong electrolyte

It will dissociate completely to give [Ca2+] = 0.2 M

At equilibrium:

Ca(OH)2 <----> Ca2+ + 2 OH-

   0.2 +s 2s

Ksp = [Ca2+][OH-]^2

5.86*10^-6=(0.2 + s)*(2s)^2

Since Ksp is small, s can be ignored as compared to 0.2

Above expression thus becomes:

5.86*10^-6=(0.2)*(2s)^2

5.86*10^-6= 0.2 * 4(s)^2

s = 2.706*10^-3 M

Molar mass of Ca(OH)2 = 1*MM(Ca) + 2*MM(O) + 2*MM(H)

= 1*40.08 + 2*16.0 + 2*1.008

= 74.096 g/mol

Molar mass of Ca(OH)2= 74.096 g/mol

s = 2.706*10^-3 mol/L

To covert it to g/L, multiply it by molar mass

s = 2.706*10^-3 mol/L * 74.096 g/mol

s = 0.200 g/L

Answer: 0.200 g/L

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