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Find the DeltapH( initial pH - final pH)...

Find the `DeltapH(` initial `pH -` final `pH)` when `100 ml 0.01M HCl` is added in a solution containing `0.1m` moles of `NaHCO_(3)` solution of negligible volume `(k_(a_(1))=10^(-7),k_(a_(2))=10^(-11)` for `H_(2)CO_(3)) :`

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Find DeltapH when 100 ml of 0.01 M HCl is added in a solution containing 0.1 m moles of NaHCO_(3) solution of negligible volume. (Ka_(1)=10^(-7), Ka_(2)=10^(-11) for H_(2)CO_(3))

Find DeltapH when 100 ml of 0.01 M HCl is added in a solution containing 0.1 m moles of NaHCO_(3) solution of negligible volume. (Ka_(1)=10^(-7), Ka_(2)=10^(-11) for H_(2)CO_(3))

Find the pH of " 0.1 M NaHCO_(3)" . Use data (K_(1)=4xx10^(-7),K_(2)=4xx10^(-11) for H_(2)CO_(3), log 4=0.6) :

Find the pH of " 0.1 M NaHCO_(3)" . Use data (K_(1)=4xx10^(-7),K_(2)=4xx10^(-11) for H_(2)CO_(3), log 4=0.6) :

50 ml of 0.2 M HCl is added to 30 ml of 0.1 MKOH solution. Find the pH of the solution.

The pH of the a solution containing 0.4 M HCO_(3)^(-) is : [K_(a_(1)) (H_(2)CO_(3)) = 4 xx 10^(-7), K_(a_(2)) (HCO_(3)^(-)) = 4 xx 10^(-11)]

In a solution of 0.1M H_(3)PO_(4) acid (Given K_(a_(1))=10^(-3),K_(a_(2))=10^(-7),K_(a_(3))=10^(-12)) Concentration of H_(2)PO_(4)^(-) is

Calculate the pH of 0.010M NaHCO_(3) solution. K_(1)=4.5xx10^(-7) , K_(2)= 4.7xx10^(-11) for carbonic acid.

The pH of a solution containing 0.4 M HCO_(3)^(-) and 0.2 M CO_(3)^(2-) is : [K_(a1)(H_(2)CO_(3))=4xx10^(-7) , K_(a2)(HCO_(3)^(-))=4xx10^(-11)]