In: Chemistry
Copper(I) chloride has Ksp = 1.7 × 10-7. Calculate the molar solubility of copper(I) chloride in pure water and in various aqueous solutions.
a. Calculate the molar solubility of CuCl in pure water. b. Calculate the molar solubility of CuCl in 0.0200 M HCl solution. c. Calculate the molar solubility of CuCl in 0.200 M HCl solution. d. Calculate the molar solubility of CuCl in 0.300 M CaCl2 solution
a)
CuCl ---> Cu+ + Cl-
s
s
Ksp = s*s
1.7*10^-7 = s^2
s=4.12*10^-4 M
Answer: 4.12*10^-4 M
b)
0.02 M HCl will give 0.02 M Cl- from begining
CuCl ---> Cu+ + Cl-
s
0.02+s
Ksp = s*(0.02+s)
1.7*10^-7 = s*(0.02+s)
Since Ksp is very small, s will be very small and it can be ignored
as compared to 0.02
so above expression becomes,
1.7*10^-7 = s*0.02
s=3.4*10^-9 M
Answer: 3.4*10^-9 M
c)
0.2 M HCl will give 0.2 M Cl- from begining
CuCl ---> Cu+ + Cl-
s 0.2+s
Ksp = s*(0.02+s)
1.7*10^-7 = s*(0.2+s)
Since Ksp is very small, s will be very small and it can be ignored
as compared to 0.2
so above expression becomes,
1.7*10^-7 = s*0.2
s=3.4*10^-8 M
Answer: 3.4*10^-8 M
d)
0.3 M CaCl2 will give 2*0.3=0.6 M Cl- from begining
CuCl ---> Cu+ + Cl-
s 0.6+s
Ksp = s*(0.02+s)
1.7*10^-7 = s*(0.6+s)
Since Ksp is very small, s will be very small and it can be ignored
as compared to 0.6
so above expression becomes,
1.7*10^-7 = s*0.6
s=1.02*10^-7 M
Answer: 1.02*10^-7 M