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Assuming Complete Dissociation, Calculate the Ph of the Following Solutions: 0.005 M Naoh - CBSE (Science) Class 11 - Chemistry

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Question

Assuming complete dissociation, calculate the pH of the following solutions:

0.005 M NaOH 

Solution

0.005MNaOH:

`NaOH_(aq) ↔ Na_(aq)^+  + HO_(aq)^(-)`

`[HO^-] = [NaOH]`

`=> [HO^-] = .005`

`pOH = -log[HO^(-)] = -log(.005)`

pOH = 2.30

:. pH = 14 - 2.30

= 11.70

Hence, the pH of the solution is 11.70.

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Solution Assuming Complete Dissociation, Calculate the Ph of the Following Solutions: 0.005 M Naoh Concept: Ionization of Acids and Bases - The pH Scale.
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