Part 1 (1 point) i See Periodic Table Q See Hint Match the provided labels to th

Question

Part 1 (1 point) i See Periodic Table Q See Hint Match the provided labels to the appropriate point on the titration curve Buffering region 14 12 10 8 6 4 2 Excess titrant Equivalence point Volume of strong base (my) Part 2 (1 point) See Hint Use the titration curve for the weak acid to calculate the pH of a 0.15 Msolution of that weak acid. Enter your answer with two significant figures. Round the pKa to the nearest whole number for the calculation, and use two significant figures for your final answer.

Explanation / Answer

PART 2

pH of a 0.15 M weak acid concentration

from buffer region

pH= pKa + loG(a-/HA)

half equivalence point --> 50/50%

pKa approx = 6

pH = 6

then...

Ka = 10^-6

Ka = [H+][A-]/[HA]

10^-6 = x*x/(0.15-x)

x = [H+] = 3.867*10^-4

pH = -log(3.867*10^-4)

pH = 3.41

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