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QUESTION

# Calculate the pH of a buffer when sodium hydrogen sulfate 0.1M and sodium sulfate has a concentration of 0.230M. (Give that Ka of hydrogen sulfate ion is 1.2*10^-2)?

The of the will be 2.28.

When dealing with , you always have to be aware of the fact that you can use the Henderson-Hasselbalch equation to solve for if you know the concentrations of the weak acid and its .

pH_"sol" = pK_a + log((["conjugate base"])/(["weak acid"]))

In your case, the weak will be sodium bisulfate, NaHSO_4, and its conjugate base will be sodium sulfate, NaSO_4. More accurately, you're going to be dealing with hydrogen sulfate, HSO_4^(-), and the sulfate ion, SO_4^(2-).

The acid dissociation constant will give you pK_a

pK_a = -log(K_a) = -log(1.2 * 10^(-2)) = 1.92

Now just plug and play

pH_"sol" = pK_a + log(([SO_4^(2-)])/([HSO_4^(-)]))

pH_"sol" = 1.96 + log((0.230cancel("M"))/(0.1cancel("M"))) = color(green)(2.28)