Calculate the pH and the percent dissociation of the hydrated cation in 0.017M s

Question

Calculate the pH and the percent dissociation of the hydrated cation in 0.017M solutions of the following substances.

See table below for values of equilibrium constants.

Fe 2+ K a = 3.2 Calculate the pH and the percent dissociation of the hydrated cation in 0.017M solutions of the following substances. Fe(NO3)2 pH= ? Express your answer using two decimal places. Express your answer using two significant figures. % dissociation = ? Fe(NO3)3 pH= ? Express your answer using two decimal places. Express your answer using two significant figures. % dissociation = ?

Explanation / Answer

pH = -log(H+)

[H+] = sqrt(kakb)

as Kb is very small then Kb = Kw = 10^-14

A): 11.74

B): 0.05

C): 8.10

D): 1.25*10^-4

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