5.00 mL of a solution of a diprotic acid, H2X, is titrated with 0.100 M NaOH, re

Question

5.00 mL of a solution of a diprotic acid, H2X, is titrated with 0.100 M NaOH, resulting in the titration curve below. What was the initial concentration of the H2X solution? Please explain how you get you're answer

Question 21 5.oo mL of a solution of a diprotic acid, H2X, is titrated with o.1oo M NaOH, resulting in the titration curve below. What was the initial concentration of the H2X solution? 14.0 12.0 10.0 8.0 pH 6.0 4.0 2.0 5.0 10.0 15.0 20.0 25.0 30.0 Volume of 0.100 M NaOH, ml. A. o.200 M B. o.100 M C. o.4oo M D. o.o4oo M

Explanation / Answer

H2X . one mole of H2X , gives 2H+ ions

Thus meq of acid = meq of base at second neutralization point

2 x 5.00mL x M = 20x 0.10

thus molarity of acid = 20x0.1 /2x5

= 0.2 M

Thus option A

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