A .175 M weak acid solution has a pH of 3.25. Calculate the Ka for the acid. (hint your answer should contain three significant figures and be written in scientific notation ex. 4.67E-2 )
PH = 3.25
-log[H^+] = 3.25
[H^+] = 10^-3.25 = 0.000562
HA(aq) ------------------> H^+ (aq) + A^- (aq)
I 0.175 0 0
C -0.000562 0.000562 0.000562
E 0.174438 0.000562 0.000562
Ka = [H^+][A^-]/[HA]
= 0.000562*0.000562/0.174438
= 1.81*10^-6 >>>>>answer
A .175 M weak acid solution has a pH of 3.25. Calculate the Ka for the...
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