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PH of solution containing 0.2M H2CO3 and 0.1M CO3 2- is (for H2CO3 ka 1 =4*10-7and ka 2=4*10-11.)
PH of solution containing 0.2M H2CO3 and 0.1M CO3 2- is
(for H2CO3 ka 1 =4*10-7and ka 2=4*10-11.)
1 Answer
Vikas TU
Dear student
Dissociation constant of n acid is the rati of its molar concentrations
[H+][A-]/[HA]=Ka
[H+][A-]/[HA]=Ka
On the case of your question,
[H+][CO3^2-]/[HCO3-]=4×10^(-7) , so
[H+]=([HCO3-]/[CO3^2-])×4×10^(-7)=2.0×4×10^(-7)=8×10^(-7) .
pH=-log([H+])=-log(8.0×10^(-7)) => aproximately equal to 6.40
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