Can someone help me with chemistry, Answer below is wrong!
pH = 3.96;
Hence, [H+] = 1.096 x 10^-4
HN3 --> H+ + N3-
Ka = [H+][N3-]/ [HN3]
= 2.2 x 10^-5
Ksp = [Cu+][N3-]
= 4.9 x 10^-9
CuN3(s) --> Cu+ + N3-
H+ + N3- --> HN3
Add the above two equations:
CuN3(s) + H+ --> Cu+ + HN3
Keq = [Cu+][HN3] / [H+]
Rearrange Ka to have [HN3] / [H+] [N3-]
Ka = [H+][N3-] / [HN3]
[HN3] / [H+][N3-] = 1/Ka
Keq = Ksp x 1/Ka = [Cu+][N3-] x [HN3] /[H+][N3-]
= [Cu+][HN3] / [H+]
Keq = 4.9 x 10^-9 / 2.2 x 10^-5 = 2.23 x 10^-4
Let Y = molar solubility of CuN3
Y = [Cu+] = [HN3]
Keq = 2.23 x 10^-4 = Y(Y) / [H+]
2.23 x 10^-4 = (Y)(Y) / 1.096 x 10^-4
Y^2 = 2.44 x 10^-8
Y = 1.56 x 10^-4
Hence molar solubility of CuN3 = 1.56 x 10^-4
Can someone help me with chemistry, Answer below is wrong! gnoring activities, determine the molar solubility...
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