QuestionDetails: 105.0 mL of a solution of quinine contains 126.0×10 3 mol of qu

Question

QuestionDetails: 105.0 mL of a solution of quinine contains 126.0×103 mol of quinine. Quinine is monobasic with Kb = 7.90× 106

a, If this is titrated with 0.200 M HCl, what is the pH half-way to thestoichiometric point ?    b. For the titration in the above question,what is the pH at thestoichiometric point ? QuestionDetails: 105.0 mL of a solution of quinine contains 126.0×103 mol of quinine. Quinine is monobasic with Kb = 7.90× 106

a, If this is titrated with 0.200 M HCl, what is the pH half-way to thestoichiometric point ?    b. For the titration in the above question,what is the pH at thestoichiometric point ?    b. For the titration in the above question,what is the pH at thestoichiometric point ? QuestionDetails: 105.0 mL of a solution of quinine contains 126.0×103 mol of quinine. Quinine is monobasic with Kb = 7.90× 106

a, If this is titrated with 0.200 M HCl, what is the pH half-way to thestoichiometric point ?    b. For the titration in the above question,what is the pH at thestoichiometric point ?

Explanation / Answer

Quinine is monobasic so at the stoichiometricpoint 126x 10^-3 mole of HCl have been used.
Volume of HCl = 126x 10^-3 / 0.0200 = 6.3 L

total volume = 6.3 L + 0.105 L= 6.405 L
Concentration X- = 126 x 10^-3 / 6.405 = 0.0197 M
K = 1 x 10^-14 / 7.90 x 10^-6 = x^2 / 0.0197-x
x = 4.99 x 10^-6 M = [H+] log(4.99 x 10^-6 M) = 5.301
>>>pH = 5.30 :) :)

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