PH of solution containing 0.2M H 2 CO 3 and 0.1M CO 3 2- is (for H 2 CO 3 k a 1 =4*10 -7 and k a 2=4*10 -11 .)

Question

PH of solution containing 0.2M H 2 CO 3 and 0.1M CO 3 2- is (for H 2 CO 3 k a 1 =4*10 -7 and k a 2=4*10 -11 .)

Vikas TU · Answer

Dear student

Dissociation constant of n acid is the rati of its molar concentrations
[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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PH of solution containing 0.2M H 2 CO 3 and 0.1M CO 3 2- is (for H 2 CO 3 k a 1 =410 -7 and k a 2=410 -11 .)

PH of solution containing 0.2M H₂CO₃ and 0.1M CO₃^2- is
(for H₂CO₃ k_a1 =410^-7and k_a2=410^-11.)

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