A 25.0-mL sample of 0.20 M CH3NH2 (methanamine, a weak base) is titrated with 0.25 M...

A 25.0-mL sample of 0.20 M CH3NH2 (methanamine, a weak base) is titrated with 0.25 M HCl. What is the pH of the solution after 13.0 mL of HCl have been added to the base? The pKb of methanamine is 4.6 x 10-4 .

What is the pH of the solution after 23.0 mL of HCl have been added to the base?

Expert Solution

queen_honey_blossom answered 2 years ago

A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate...

A 25.0 mL of a weak acid is titrated with a strong base (0.1 M). Calculate the pH of the solution during the titration if the weak acid concentration is 0.10 M and its Ka = 1.8 x 10-5 and 10.0 mL of base has been added. (Hint: use Henderson-Hasselbach equation). a) pH = 4.56 b) pH= 5.28 c) pH= 4.74

A 25.0 mL sample of 0.30 M HCOOH is titrated with 0.20 M KOH. What is...

A 25.0 mL sample of 0.30 M HCOOH is titrated with 0.20 M KOH. What is the pH of the solution after 25.0 mL of KOH has been added to the acid? Ka = 1.8x10^-4

A 100.0 mL sample of 0.20 M HF is titrated with 0.20 M KOH. Determine the...

A 100.0 mL sample of 0.20 M HF is titrated with 0.20 M KOH. Determine the pH of the solution after the addition of 50.0 mL of KOH. The Ka of HF is 3.5 × 10-4. A. 2.08 B. 3.15 C. 4.33 D. 3.46 E. 4.15

A 10.00 mL sample of 0.150 M sodium azide, NaN3, a weak base, is titrated with...

A 10.00 mL sample of 0.150 M sodium azide, NaN3, a weak base, is titrated with 0.100 M HCl. Calculate the pH after the addition of the following volumes of acid: (a) 0.00 mL; (b) 9.00 mL; (c) 15.00 mL; (d) 27.00 mL The Ka of HN3 is 1.9 x 10–5

A) A 29.0 mL sample of 0.274 M methylamine, CH3NH2, is titrated with 0.238 M hydroiodic...

A) A 29.0 mL sample of 0.274 M methylamine, CH3NH2, is titrated with 0.238 M hydroiodic acid. The pH before the addition of any hydroiodic acid is ______. B) A 24.5 mL sample of 0.220 M ethylamine, C2H5NH2, is titrated with 0.399 M hydroiodic acid. At the titration midpoint, the pH is ______. C) A 28.2 mL sample of 0.293 M dimethylamine, (CH3)2NH, is titrated with 0.273 M hydrochloric acid. After adding 13.6 mL of hydrochloric acid, the pH is...

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A 25.0 mL sample of a 0.110 M solution of acetic acid is titrated with a 0.138 M solution of NaOH. Calculate the pH of the titration mixture after 10.0, 20.0, and 30.0 mL of base have been added. The Ka for acetic acid is 1.76x10^-5.

A 25.0 mL sample of a 0.3400 M solution of aqueous trimethylamine is titrated with a...

A 25.0 mL sample of a 0.3400 M solution of aqueous trimethylamine is titrated with a 0.4250 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C.

Consider the titration of 70.0 mL of 0.0300 M CH3NH2 (a weak base; Kb = 0.000440)...

Consider the titration of 70.0 mL of 0.0300 M CH3NH2 (a weak base; Kb = 0.000440) with 0.100 M HNO3. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 5.3 mL pH = (c) 10.5 mL pH = (d) 15.8 mL pH = (e) 21.0 mL pH = (f) 27.3 mL pH =

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the...

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Ka of HF is 3.5 × 10-4. Answer: 8.14 but how do I get this?? I'm so lost!

A 25.0 mL sample of 0.150 M hydrazoic acid (HN3) is titrated with a 0.150 M...

A 25.0 mL sample of 0.150 M hydrazoic acid (HN3) is titrated with a 0.150 M NaOH solution. Calculate the pH at equivalence and the pH after 26.0 mL of base is added. The Ka of hydrazoic acid is 1.9x10^-5.

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