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13 Dec 2019

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2. The Ka for HC7H5O2 is 6.5 x 10-5.

4.31
4.49
10.51
4.19
9.69

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Lelia Lubowitz
Lelia LubowitzLv2
17 Dec 2019

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Related questions

Consider the titration of a 25.0 −mL sample of 0.110 M HC7H5O2 with 0.120 M KOH. Determine each of the following.

The Ka of HC7H5O2 is 6.5 × 10−5.

Part A: the pH at 5.00 mL of added base pH= ?

Calculate the pH at the halfway point and at the equivalence point for each of the following titrations.

a. 100.0 mL of 0.10 M HC7H5O2 (Ka = 6.4 × 10–5) titrated by 0.10 M NaOH

b. 100.0 mL of 0.10 M C2H5NH2 (Kb = 5.6 × 10–4) titrated by 0.20 M HNO3

c. 100.0 mL of 0.50 M HCl titrated by 0.25 M NaOH

Calculate the pH at the halfway point and at the equivalence point for each of the following titrations.

(a) 100.0 mL of 0.10 M HC7H5O2 (Ka = 6.4 x 10-5) titrated by 0.10 M NaOH.

(b) 100.0 mL of 0.10 M C2H5NH2 (Kb = 5.6 x 10-4) titrated by 0.20 M HNO3. 

(c) 100.0 mL of 0.50 M HCl titrated by 0.25 M NaOH.

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