Question

calculate pH of the solution obtaained when 1ml of 13.6M HCL is diluted with water to give 1litre of the solution

Answer 1

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Answer 2

The pH of the solution obtained when 1 ml of 13.6 M HCl is diluted with water to give 1litre of the solution is 1.86.

Given:

$M_1$ = 13.6

$V_1$ = 1 ml

$V_2$ = 1 L = 1000 ml

To find:

pH of the solution = ?

Formula to be used:

• $M_1V_1 = M_2V_2$
• pH = $-log[H^+]$

Calculation:

As per the molarity formula,

$M_1V_1 = M_2V_2$

Let $M_2$ be the molarity of HCl

13.6 × 1 = $M_2$ × 1000

$M_2 =$$\frac{13.6\times1}{1000}$

$M_2$ = 0.0136

$M_2$ = $1.36\times10^{-2}$

We know that

pH = $-log[H^+]$

pH = $-log[1.36\times10^{-2}]$

pH = $-[log 1.36+ log 10^{-2}]$

pH = - [0.1335 - 2]

pH = 1.8665

pH = 1.87

Conclusion:

The pH of the given solution is calculated as 1.87.

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