At the stoichiometric point in the titration of 0.130 MHCOOH(aq) with 0.130 M KO

Question

At the stoichiometric point in the titration of 0.130 MHCOOH(aq) with 0.130 M KOH(aq), A) [HCO_2^-] = 0.0650 M B) [HCO_26-] = 0.130 M C) the pH is less than 7. D) the pH is 7.0. E) [HCOOH] = 0.0650 M At the stoichiometric point in the titration of 0.260 M CH_3NH_2(aq) with 0.260 M HCl(aq), A) [CH_3NH_2] = 0.130 M. B) the pH is greater than 7. C) [CH_3NH_3^+] = 0.260 M D) the pH is 7.0. E) [CH_3NH_3^+] = 0.130 M What is the pH at the stoichiometric point for the titration of 0.100 M CH_3COOH(aq) with 0.100 M KOH(aq)? The value of K_a for acetic acid is 1.8 times 10^-5. Can use approximation. A) 8.72 B) 5.28

Explanation / Answer

This is titration between weak acid HCOOH and strong base KOH

Let see

HCOOH + NaOH ------------ [ HCOO- Na+] [H2O]

As monobasic acid it need same amount of acid

So after titration concentration of formate ion will be 0.136 M that is option B is correct

At stochometric point there will equal amount of acid and base but as base is more stronger than acid the pH will be greater than 7.00

Option C and D are false

At stochometric point all the acid will neutralize hence there will be no HCOOH therfore option E aslo false

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