Use the titration curve for the weak acid to calculate the pH of a 0.150 M solution of that weak acid.
Round the pKa to the nearest whole number for the calculation, and enter your answer for the pH to two significant figures.
Match the provided labels to the appropriate point on the titration curve.
pH = 3.4
Explanation
The pKa value rounded to nearest whole number is 6.0
pKa = 6.0
Ka = 10-pKa
Ka = 10-6.0
Ka = 1.0 x 10-6
initial concentration of acid = 0.150 M
ICE table | HA (aq) | H+ (aq) | A- (aq) | |
Initial conc. | 0.150 M | 0 | 0 | |
Change | -x | +x | +x | |
Equilibrium conc. | 0.150 M - x | +x | +x |
Ka = [H+]eq[A-]eq / [HA]eq
1.0 x 10-6 = [(x) * (x)] / (0.150 M - x)
Solving for x, x = 3.87 x 10-4 M
pH = -log[H+]
pH = -log(3.87 x 10-4 M)
pH = 3.41
Use the titration curve for the weak acid to calculate the pH of a 0.150 M solution of that weak acid.
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