Math, asked by vedansh527, 10 months ago

Calculate the pH of 10-6 M HCl solution. When 10-6 M HC and 10-5 M NaOH solutions are mixed
in equal amounts, what will be the pH of the mixed solution?

Answers

Answered by sonuvuce
1

pH of 10⁻⁶ M HCl is 6

pH of the mixed solution is 8.954

Explanation:

We know that

pH=-\log[H^+]

Given concentration of H^+ ions in HCl solution

[H^+]=10^{-6} mole/litre

Therefore, the pH of HCl solution

pH=-\log 10^{-6}

or, pH=6

When 10⁻⁶ M HCl is mixed with 10⁻⁵ M NaOH then the reaction is

HCl + NaOH ⇒ NaCl + H₂O

1 mole of HCl reacts with 1 mole of NaOH

Therefore, 10⁻⁶ mole HCl will react with 10⁻⁶ mole NaOH

Remaining moles of NaOH

=10^{-5}-10^{-6}

=10^{-6}(10-1)

=9\times 10^{-6}

Therefore concentration of OH⁻ ions

[OH^-]=9\times 10^{-6} mole/litre

We know that

[H^+][OH^-]=10^{-14}

\implies [H^+]=\frac{10^{-14}}{[OH^-]}

\implies[H^+] = \frac{10^{-14}}{9\times 10^{-6}}

\implies [H^+] =1.11\times 10^{-9}

Therefore, the pH of the solution is

pH=-\log(1.11\times 10^{-9})

\implies pH=9-0.046

\implies pH=8.954

Hope this answer is helpful.

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