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ScrubsFan
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70. The solubility product of calcium hydroxide, Ca(OH)2, is 7.9 x 10-6 at 25°C. Will a precipitate form when 100mL of 0.10 mol/L of CaCl2 solution and 50.0mL of 0.070 mol/L of NaOH solution are combined?
Solution
1. Determine the formula for the possible precipitate that might form, and write the Ksp expression of this insoluble salt. If the precipitate forms, it will be Ca(OH)2.
Ca(OH)2 <---> Ca2+ (aq) + 2OH- (aq)
Ksp = [Ca2+][OH-]2 = 7.9 x 10-6
2. Calculate the concentration of each of the Ca2+ and OH- ions available in solution:
[Ca2+] = number of mol of Ca2+ / total volume of solution
= 0.1 mol/L (1 x 10-1 L) / 0.05 L + 1 x 10-1 L
= 2.0 x 10-2 mol/L
[OH-]2 = 0.070 mol/L (0.05 x 10-3 L) / 0.1 L + 0.05 x 10-3 L
= 8.5 x 10-5 mol/L
3. Substitute the ion concentrations into an experimental ion product (Q) equation that is identical to the Ksp expression. This will allow you to compare two solubility product values and determine whether a precipitate will form.
Experimental ion product (Q)
= [Ca2+][OH-]2
= (2.0 x 10-2)(8.5 x 10-5)2
= 1.4 x 10-10
Since Q (1.4 x 10-10) is greater than Ksp (7.9 x 10-6), a precipitate will form.
Solution
1. Determine the formula for the possible precipitate that might form, and write the Ksp expression of this insoluble salt. If the precipitate forms, it will be Ca(OH)2.
Ca(OH)2 <---> Ca2+ (aq) + 2OH- (aq)
Ksp = [Ca2+][OH-]2 = 7.9 x 10-6
2. Calculate the concentration of each of the Ca2+ and OH- ions available in solution:
[Ca2+] = number of mol of Ca2+ / total volume of solution
= 0.1 mol/L (1 x 10-1 L) / 0.05 L + 1 x 10-1 L
= 2.0 x 10-2 mol/L
[OH-]2 = 0.070 mol/L (0.05 x 10-3 L) / 0.1 L + 0.05 x 10-3 L
= 8.5 x 10-5 mol/L
3. Substitute the ion concentrations into an experimental ion product (Q) equation that is identical to the Ksp expression. This will allow you to compare two solubility product values and determine whether a precipitate will form.
Experimental ion product (Q)
= [Ca2+][OH-]2
= (2.0 x 10-2)(8.5 x 10-5)2
= 1.4 x 10-10
Since Q (1.4 x 10-10) is greater than Ksp (7.9 x 10-6), a precipitate will form.