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HCN + H20 <-> H3o+ + CN-
Ka = 6.2 x 10^-10
ka = [h3o+][CN-]/[HCN] = x^2/0.1m
x^2 + 6.2 x 10^-10x - 6.2 x 10^-11
x = 7.87 x 10^-6
pH = -log[x] = -log[7.87x 10^-6 = 5.1
The pH of a 0.1 molar aqueous solution of HCl would be 1. HCl fully dissociates in water to form H+ ions, making the solution highly acidic.
- log(0.1 M)
= 1
14 - 1
= 13 pH
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It is a weak base.So pH depends on Kb value.
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The pH of a 0.1 molar aqueous solution of HCl would be 1. This is because HCl is a strong acid that completely dissociates in water to produce H+ ions, resulting in a high concentration of H+ ions in solution, leading to a low pH value.
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