Question

In: Chemistry

Calculate the pH at the equivalence point in titrating 0.120 M solutions of each of the...

Calculate the pH at the equivalence point in titrating 0.120 M solutions of each of the following with 9.0×10−2 MNaOH.

Part A

hydrobromic acid (HBr)

Part B

chlorous acid (HClO2)

Part C

benzoic acid (C6H5COOH)

Solutions

Expert Solution

Part A.Since HBr and NaOH are a strong acid and a strong base, the net ionic equation for the reaction is just:

H+ + OH- --> H2O. So, the pH of that solution at the equivalence point will be pH = 7.00.

Part B. Chlorous acid, HClO2, Ka = 1.1 x 10-2

The volumes are not given but this should still be solvable. At equivalence point, mmoles of acid equal mmoles of base. That is,

Mbase x Vbase = Macid x Vacid

thus Vacid = (Mbase x Vbase) / Macid

What we need to solve this problem is the total volume at the equivalence point and the number of mmoles of the salt that is formed:

[ClO2-] = (Mbase x Vbase )/(Vbase + Vacid)

= (Mbase x Vbase) / (Vbase + (Mbase x Vbase) / Macid)

The remaining V term, Vbase will cancel out:

[ClO2-] = Mbase /(1 + (Mbase/Macid)) = MbaseMacid/(Mbase+Macid)
[ClO2-] = (0.120)(9 * 10-2)/0.21 = 0.051

ClO2-(aq) + H2O(l) <====> HClO2 (aq) + OH-(aq)
Kb = Kw/Ka= (1.0 x 10-14)/(1.1 x 10-2) = [HC3H5O3][OH-]/[ C3H5O3-]

9.1 x 10-13 = [OH-]2/0.051
[OH-] = 2.2 x 10-7, pOH = 6.7, pH = 7.3

Part C. Benzoic acid, HC7H5O2, Ka = 6.46 x 10-5

The volumes are not given but this should still be solvable. At equivalence point, mmoles of acid equal mmoles of base. That is,

Mbase x Vbase = Macid x Vacid

thus Vacid = (Mbase x Vbase) / Macid

What we need to solve this problem is the total volume at the equivalence point and the number of mmoles of the salt that is formed:

[C7H5O2-] = (Mbase x Vbase )/(Vbase + Vacid)

= (Mbase x Vbase) / (Vbase + (Mbase x Vbase) / Macid)

The remaining V term, Vbase will cancel out:

[C7H5O2-] = Mbase /(1 + (Mbase/Macid)) = MbaseMacid/(Mbase+Macid)
[C7H5O2-] = (0.120)(9 * 10-2)/0.21 = 0.051

C7H5O2-(aq) + H2O(l) <====> HC7H5O2 (aq) + OH-(aq)
Kb = Kw/Ka= (1.0 x 10-14)/(6.46 x 10-5) = [HC7H5O2][OH-]/[ C7H5O2-]

1.55 x 10-10 = [OH-]2/0.051
[OH-] = 2.8 x 10-6, pOH = 5.5, pH = 8.5


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