A 25.0 mL sample of a 0.2400 M solution of aqueous trimethylamine is titrated with a 0.3000 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.
mostly need help with part 3. I keep doing it incorrectly
part 1: pH after 10 ml acid added
part 2: pH after 20 ml acid added
part 3: pH after 30 ml acid added
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A 25.0 mL sample of a 0.2400 M solution of aqueous trimethylamine is titrated with a...
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home / study / science / chemistry / chemistry questions and answers / a 25.0 ml sample of a 0.1700 m solution of aqueous trimethylamine is titrated with a 0.2125 ... Question: A 25.0 mL sample of a 0.1700 M solution of aqueous trimethylamine is titrated with a 0.2125 M sol... A 25.0 mL sample of a 0.1700 M solution of aqueous trimethylamine is titrated with a 0.2125 M solution of HCl. Calculate the pH of the solution after 10.0,...
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25.0 ml of a 0.100 M trimethylamine (CH3)3N (a base like ammonia) Kb = 6.3×10−5, are transferred in an Erlenmeyer flask and titrated with 0.100 M of HCl. Predict pH, pOH, concentration of trimethylamine, concentration of the conjugated acid (CH3)3NH+, and concentration of HCl in the Erlenmeyer flask when: (a) 0 mL of HCl solution are added to the Erlenmeyer flask (a) 12.5 mL of HCl solution are added to the Erlenmeyer flask (c) 25 mL of HCl solution are...
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