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25 mL (M/10) HCl solution is mixed with ...

25 mL (M/10) HCl solution is mixed with 50 mL 2/25(M)KOH solution. What will be the pH of the resulting solution?

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`25mL((M)/(10))HCl -=(1)/(10)xx25-=2.5` millimol HCl and 50 mL `(2)/(25)(M)KOH-=(2)/(25)xx50-=4` millimol KOH.
2.5 millimol HCl reacts completely with 2.5 millimol of KOH to form KCl and `H_(2)O` leaving behind (4-2.5)=1.5 millimol of KOH in the mixed solution.
The total volume of mixed solution`=(25+50)mL=75mL`
`therefore`The concentration of the remaining KOH present in the mixed solution`=(1.5)/(75)=0.02(M)`
Hence, in the mixed solution, `[OH^(-)]=0.02(M)`
`=-log_(10)(0.02)=1.7`
and `pH=14-pOH=14-1.7=12.3`
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