# Answer on Inorganic Chemistry Question for Al

Question #19507

Consider a solution that is 0.10 M in a weak triprotic acid which is represented by the gen- eral formula H3A with ionization constants K1 = 1.0×10−3, K2 = 1.0×10−8, and K3 = 1.0×10−12. What is the pH of the solution?

Expert's answer

K

H

K

H

H

K

[H

[H

pH = -log [H

_{3}is very small,so K_{2}and K_{1}is resulting infinding pHH

_{2}A^{-}= H^{+}+ HA^{-}K

_{2}= [H^{+}]^{2}/H_{2}A^{-}H

_{2}A^{-}= [H^{+}]^{2}/K_{2}H

_{3}A = H^{+}+ [H^{+}]^{2}/K_{2}K

_{1}= ([H^{+}]^{2}/K_{2})^{2}/[H_{3}A][H

^{+}]^{4}= K_{1}*K_{2}^{2}[H_{3}A][H

^{+}] = (K_{1}*K_{2}^{2}[H_{3}A])^{1/4}= (1.0×10^{−3}*(1.0×10^{−8})^{2}* 0.10)^{1/4}= 1x10^{10}pH = -log [H

^{+}] = 10Need a fast expert's response?

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