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Calculate the pH at the halfway point and at the equivalence point for each of the following titrations. (Assume that the temperature is 25°C.) (a) 104.6 mL of 0.19 M HNO2 (Ka= 4.0 ✕ 10−4) titrated with 0.19 M KOH halfway point equivalence point (b) 104.5 mL of 0.18 M (C2H5)3N (Kb = 4.0 ✕ 10−4) titrated with 0.36 M HCl halfway point equivalence point

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Sixta Kovacek
Sixta KovacekLv2
30 Sep 2019
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Related questions

A 20. mL sample of a 0.10 M weak acid (KA= 1.3×10−4 ) is titrated with 0.20 M NaOH. If 10.0 mL of NaOH are needed to reach the equivalence point, what is the pH after addition of 5.0 mL of NaOH (halfway to the equivalence point)?

a. 10.0

b. 8.71

c. 5.35

d. 4.57

e. 3.89

An 80 mL sample of 0.200 M ammonia is titrated with 0.100 M HCl. Kb for ammonia is 1.8*10-5. Calculate the pH of the solution at each of the following points of the titration:

a) before the addition of any HCl

b) halfway to the equivalence point

c) at the equivalence point

d) after the addition of 175 mL of 0.100 M HCl

(1) A 40.0 mL sample of 0.134 M HNO2 is titrated with 0.262 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH

(2) Consider the titration of a 25.0-mL sample of 0.110 M HC2H3O2 with 0.130 M NaOH. (The value of Ka for HC2H3O2 is 1.8×10−5.) Determine the pH after adding 4.0 mL of base beyond the equivalence point.

(3) Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2 with 0.145 M HBr. (The value of Kb for CH3NH2 is 4.4×10−4.) (a) Determine the pH at one-half of the equivalence point. (b) Determine the pH after adding 5.0 mL of acid beyond the equivalence point.

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