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))`
`pH` of solution is

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

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 HPO_(4)^(2-) is

Hin is an acidic indicator (K_(Ind) =10^(-7)) which dissociates into aqueous acidic solution of 30mL of 0.05M H_(3)PO_(4) (K_(1) = 10^(-3), K_(2) = 10^(-7), K_(3) = 10^(-13)) If this solution is treated with 30mL of NaOH solution, then what molarity of NaOH is needed to reach the equivalence point with indicator?

Ratio of [HA^(+)] in 1L of 0.1M H_(3)A solution [K_(a_(1))=10^(-5),K_(a_(2))=10^(-8)K_(a_(3))=10^(-11)] & upon addition of 0.1 mole HCl to it will be :

Acidic solution is defined as a solution whose [H^(o+)] gt [overset(Theta)OH] . Base solution has [overset(Theta)OH] gt [H^(o+)] . During acid-base titrations, pH of the mixture will change depending on the amount base added. This variation is shown in the form of graph by making plot as titration curves 100mL of 1.0 M H_(3)A (K_(a_(1)) = 10^(-3), K_(a_(2)) = 10^(-5), K_(a_(3)) = 10^(-7)) is titrated against 0.1M NaOh . The titration curve is as follows. What is the pH at point A?

Acidic solution is defined as a solution whose [H^(o+)] gt [overset(Theta)OH] . Base solution has [overset(Theta)OH] gt [H^(o+)] . During acid-base titrations, pH of the mixture will change depending on the amount base added. This variation is shown in the form of graph by making plot as titration curves 100mL of 1.0 M H_(3)A (K_(a_(1)) = 10^(-3), K_(a_(2)) = 10^(-5), K_(a_(3)) = 10^(-7)) is titrated against 0.1M NaOh . The titration curve is as follows. What will be the change in pH from point B to point C?

Hin is an acidic indicator (K_(Ind) =10^(-7)) which dissociates into aqueous acidic solution of 30mL of 0.05M H_(3)PO_(4) (K_(1) = 10^(-3), K_(2) = 10^(-7), K_(3) = 10^(-13)) If Hin and Ind^(Theta) posses colour P and Q , respectively, and concentration of HIn is 120 times than that of Ind^(Theta) . colour Q predominates over P when concnetration of Ind^(Theta) is 127 times of HIn . What is the pH range of the indicator.

Hin is an acidic indicator (K_(Ind) =10^(-7)) which dissociates into aqueous acidic solution of 30mL of 0.05M H_(3)PO_(4) (K_(1) = 10^(-3), K_(2) = 10^(-7), K_(3) = 10^(-13)) Calculate the [(Ind^(Theta))/(Hin)]

Calculate the changes in pH of 0.1MNaHA solution after diluting it to ten times the original volume.(Given that for H_(3)A:K_(a_(1))=10^(-4),K_(a_(2))=10^(-7),K_(a_(3))=10^(-11))

In a solution containing 0.1M HCl & 0.1M H_(3)PO_(4) (having dissociation constants K_(a_(1)),K_(a_(2)),K_(a_(3))) assuming alphaltlt1 for H_(3)PO_(4) ,