What is the pH of 10^{-9} M aqueous HCl solu | vedclass

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(B) For a very dilute acid solution,the contribution of $H^{+}$ ions from the auto-ionization of water cannot be neglected.Given concentration of $HCl

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between $6$ to $7$

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(B) For a very dilute acid solution,the contribution of $H^{+}$ ions from the auto-ionization of water cannot be neglected.Given concentration of $HCl = 10^{-9} \ M$.Total $[H^{+}] = [H^{+}]_{HCl} + [H^{+}]_{H_2O}$.$[H^{+}] = 10^{-9} + 10^{-7} \ M$ (since $[H^{+}]$ from water is $10^{-7} \ M$ at $25^{\circ}C$).$[H^{+}] = 0.01 	imes 10^{-7} + 10^{-7} = 1.01 	imes 10^{-7} \ M$.$pH = -\log [H^{+}] = -\log (1.01 	imes 10^{-7})$.$pH = 7 - \log (1.01) \approx 7 - 0.0043 = 6.9957$.Thus,the $pH$ is between $6$ and $7$.

What is the $pH$ of $10^{-9} \ M$ aqueous $HCl$ solution?

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