Given the following `K_(a)` values, determine which species is the strongest base ?
`HSO_(4)^(-)=1.2xx10^(-2),H_(2)PO_(4)^(-)=6.3xx10^(-8),HCO_(3)^(-)=4.7xx10^(-11)`

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)]

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)]

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)]

Calculate the concentration of all species of significant concentrations presents in 0.1 M H_(3)PO_(4) solution. lf K_(1) = 7.5 xx 10^(-3), K_(2) = 6.2 xx 10^(-8), K_(3) = 3.6 xx 10^(-13)

Find the number : a. (4xx10^(5))+(3xx10^(2))+(7xx10^(0)) b. (3xx10^(6))+(8xx10^(3))+(1xx10^(1))