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Determine the pH of the following soluti...

Determine the pH of the following solutions:
(1) 0.1 (N) NaOH (2) 0.005(M) `Ca(OH)_(2)`

Text Solution

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(1) 0.1`(N)NaOH-=0.1(M)NaOH` [`becauseNaOH` is a monoacidic base]
In 0.1(M)NaOH solution, `[OH^(-)]=0.1(M)`
`therefore`For an aqueous 0.1(M)NaOH solution,
`pOH=-log_(10)[OH^(-)]=-log_(10)(0.1)=1.0`
`therefore pH=14-pOH=14-1=13`
(2) In case of 0.005(M) `Ca(OH)_(2)` solution,
`[OH^(-)]=2xx0.005=0.01(M)`
[`because` Each `Ca(OH)_(2)` molecule ionises to give 2 `OH^(-)` ions]
`therefore ` In case of 0.005(M) Ca`(OH)_(2)` solution,
`pOH=-log_(10)[OH^(-)]=-log_(10)(0.01)=2`
`therefore pH=14-pOH=14-2=12`
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