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Henderson Hassleback Equation

1 ml of 13.6 ...

Question

1 ml of 13.6 M HCl is diluted with water to give 1 litre of the solution. Calculate Ph of the resulting solution.

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Solution

Moles of HCl in the original solution = $0.001 \times 13.6 = 0.0136$ moles.
Now concentration of HCl in 1 liter solution $= \frac{0.0136}{1} = 0.0136 M$
Concentration of H+ = 0.0136M
$p H = - l o g [H +] = - l o g (0.0136) = 1.886$

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