What is the pH of resulting solution when equal volume of 0.1 M Naoh and 0.01 M HCL are mixed?

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Text Solution

(a) `12.65`(b) `2.0`(c) `7.0`(d) `1.04`

Answer : A

Solution : Key Concept - When equal volumes of acid and base are mixed, then resulting solution become alkaline if concentration of base is taken high. Let normality of the solution after mixing 0.1 M NaOH and 0.01 M HCl is N. <br> `therefore N_(1)V_(1)-N_(2)V_(2)=NV` <br> or `0.1xx1-0.01xx1=Nxx2` <br> Since, normality of NaOH is more than that of HCl. Hence, the resulting solution is alkaline. <br> or `[overset(-)(O)H]=N=(0.09)/(2)=0.045 N` <br> or `pOH=-log(0.045)=1.35` <br> `therefore pH=14-pOH=14-1.35=12.65`

9.

The formation of the oxide ion O2- (g), from oxygen atom requires first an exothermic and then an endothermic step as shown below,

• electron repulsion outweighs the stability gained by achieving a noble gas configuration

• O- ion has comparatively smaller size that oxygen atom

• oxygen is more electronegative

• oxygen is more electronegative

A.

electron repulsion outweighs the stability gained by achieving a noble gas configuration

Electron repulsion predominates over the stability gained by achieving noble gas configuration. Hence, the formation of O2- in the gas phase is unfavourable.