1.

Calculate the pH of solution obtained by mixing 10mL of 0.1M HCl and 40mL of 0.2M H_(2)SO_(4) take log3.4=0.53

Answer»

Solution :Given is the CASE of a mixture of `2` strong acids.
MILL moles of `H^(+)` form `HCl =10xx0.1=1`
MILLI moles of `H^(+)` form `H_(2)SO_(4)=40xx0.2xx2=16`
,.TOTAL millimoles of `H^(+)` in solution =`1+16=17`
`:.[H^(+)]=(17)/(50)=3.4xx10^(-1)( :.[H^(+)]_(f)=(("Millmoles"_("Total"))/(V))`
`:.pH=-log[H^(+)]=-log0.34`
`pH=0.47`


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