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What is the major species? : HCNO (aq)
What is the minor species? : CNO- (aq)
What is the concentration of the minor species in the solution? : 3 x 10^-3 M
What is the concentration of the major species in the solution? : 0.0278 M
What is the concentration of H3O+ in the solution? : 3.1 x 10^-3 M
What is the concentration of OH- in the solution? : 3.2 x 10^-12 M
Find the pH : 2.5
Explanation
Given : initial concentration of HCNO = 0.0309 M
Ka = 3.5 x 10^-4
ICE table | HCNO (aq) | H2O (l) | CNO- (aq) | H3O+ (aq) | |
Initial conc. | 0.0309 M | - | 0 | 0 | |
Change | -x | - | +x | +x | |
Equilibrium conc. | 0.0309 M - x | - | +x | +x |
Ka = [CNO-]eq[H3O+]eq / [HCNO]eq
3.5 x 10^-4 = [(x) * (x)] / (0.0309 M - x)
Solving for x, x = 3.12 x 10^-3 M
[H3O+] = x = 3.12 x 10^-3 M
pH = -log[H3O+]
pH = -log(3.12 x 10^-3 M)
pH = 2.51
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