Asked by Jackie
Ignoring activities, determine the molar solubility of copper (I) azide (CuN3) in a solution with a pH of 10.83. Ksp (CuN3) = 4.9 × 10–9; Ka (HN3) = 2.2 × 10–5.
Answers
Answered by
DrBob222
pH = 10.83; (H^+) = 1.48E-11
CuN3 ==> Cu^+ + N3^-
H^+ + N3^- ==> HN3 add the two eqns.
------------------- N3^- cancels.
CuN3 + H^+ ==> Cu^+ + HN3
Keq for this rxn is Ksp/Ka = 0.000223
..x....1.48E-11..x.....x
Keq = 0.000223 = (x)(x)/1.48E-11
Solve for x.
CuN3 ==> Cu^+ + N3^-
H^+ + N3^- ==> HN3 add the two eqns.
------------------- N3^- cancels.
CuN3 + H^+ ==> Cu^+ + HN3
Keq for this rxn is Ksp/Ka = 0.000223
..x....1.48E-11..x.....x
Keq = 0.000223 = (x)(x)/1.48E-11
Solve for x.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.