HCIO is a weak acid (Ka=4.0 × 10-8) and so the salt NaClO acts as a weak base, what is the pH of a solution that is 0.044 M in NaCIO at 25 °C?
pH = _______
Given,
[NaClO] = 0.044 M
Ka of weak acid (HClO) = 4.0 x 10-8
The equation for salt dissolved in water,
ClO-(aq) + H2O(l) HClO(aq) + OH-(aq)
Drawing an ICE chart,
ClO-(aq) | HClO(aq) | OH-(aq) | |
I(M) | 0.044 | 0 | 0 |
C(M) | -x | +x | +x |
E(M) | 0.044-x | x | x |
Ka x Kb = 1.0 x 10-14
4.0 x 10-8 x Kb = 1.0 x 10-14
Kb = 2.5 x 10-7
Kb = [OH-] [HClO] / [ClO-]
2.5 x 10-7 = x2 / 0.044-x
2.5 x 10-7 = x2 / 0.044 (0.044-x) 0.044 Since, x<<< 0.044
1.1 x 10-8 = x2
x = 1.048 x 10-4
x = [OH-] = 1.048 x 10-4
We know,
pOH = -log[OH-]
pOH = -log[1.048 x 10-4]
pOH = 3.979
pH + pOH = 14
pH + 3.979 = 14
pH = 10.
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