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Calculate the Ph of the Following Solutions: 1ml of 13.6 M Hcl is Diluted with Water to Give 1 Litre of Solution. - CBSE (Science) Class 11 - Chemistry

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Question

Calculate the pH of the following solutions:

1mL of 13.6 M HCl is diluted with water to give 1 litre of solution.

Solution 1

For 1mL of 13.6 M HCl diluted with water to give 1 L of solution:

13.6 × 1 mL = M2 × 1000 mL

(Before dilution) (After dilution)

13.6 × 10–3 = M2 × 1L

M2 = 1.36 × 10–2

[H+] = 1.36 × 10–2

pH = – log (1.36 × 10–2)

= (– 0.1335 + 2)

= 1.866 ∼ 1.87

Solution 2

`M_1V_1 = M_2V_2`

`:. 13.6 M xx  1m L = M_2 xx 1000 mL`

`:. M_2 = 1.36 xx 10^(-2) M`

`[H^+]= [HCl] = 1.36 xx 10^(-2) M`

`pH  = -log (1.36 xx 10^(-2)) = 2 - 0.1335 ~~ 1.87`

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Solution Calculate the Ph of the Following Solutions: 1ml of 13.6 M Hcl is Diluted with Water to Give 1 Litre of Solution. Concept: Ionization of Acids and Bases - The pH Scale.
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