The concentration of an aqueous HCl solution | vedclass

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(B) For a very dilute acid solution ($10^{-8} \ M$ or less),the contribution of $H^+$ ions from the auto-ionization of water cannot be ignored.Total $

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Between $6$ and $7$

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(B) For a very dilute acid solution ($10^{-8} \ M$ or less),the contribution of $H^+$ ions from the auto-ionization of water cannot be ignored.Total $[H^+] = [H^+]_{HCl} + [H^+]_{H_2O}$.Given $[H^+]_{HCl} = 10^{-9} \ M$.From water,$[H^+]_{H_2O} \approx 10^{-7} \ M$ (at $25^{\circ}C$).Total $[H^+] = 10^{-9} + 10^{-7} = 10^{-7} (0.01 + 1) = 1.01 	imes 10^{-7} \ M$.$pH = -\log[H^+] = -\log(1.01 	imes 10^{-7}) = 7 - \log(1.01) \approx 7 - 0.004 = 6.996$.Since $6.996$ is slightly less than $7$,the $pH$ lies between $6$ and $7$.

The concentration of an aqueous $HCl$ solution is $10^{-9} \ N$. What is the $pH$ of the solution?

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