Ignoring activities, determine the molar solubility of copper (I) azide (CuN3) i

Question

Ignoring activities, determine the molar solubility of copper (I) azide (CuN3) in a solution with a pH of 3.447. Ksp (CuN3) = 4.9 × 10–9; Ka (HN3) = 2.2 × 10–5.

c Dwww.saplinglearning.ca/ibiscms/mod/ibis/view.php?id=185479 Gradebook o 2/9/2016 11 :00 PM 6.9/102/9/2016 04:48 PM Attempts Score Weight Periodic Table Incorrect Print Calculator Question 4 of 10 Incorrect 100 sapling leaming lgnoring activities, determine the molar solubility of copper (I) azide (CuN3) in a solution with a pH of 3.447. Kg, (CuNa) = 4.9 x 10-9%, (HN3,-2.2 x 10-5. 4 90 100 Number 1.32 x 10-5 100 10 100 ENG 6:26 PM US 2016-02-09

Explanation / Answer

Ksp = [Cu+][N3-]

Ka = [N3-][H+]/[HN3]

1/Ka = [HN3]/[H+][N3-]

pH = 3.447 = -log[H+]

[H+] = 3.57 x 10^-4 M

CuN3 <==> Cu+ + N3-

N3- + H+ <==> HN3

Add both equations,

CuN3 + H+ <==> Cu+ + HN3

let x be the molar solubility of CuN3, we have x amount of Cu+ and x amount of N3-

Keq = [Cu+][HN3]/[CuN3][H+] = Ksp/Ka = 4.9 x 10^-9/2.2 x 10^-5 = 2.23 x 10^-4

Keq = 2.23 x 10^-4 = x^2/[H+] = x^2/3.57 x 10^-4

x = 2.82 x 10^-4 M

Thus the molar solubility is 2.82 x 10^-4 M

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