A 50.00-mL solution of 0.0350 M trimethylamine (Kb = 6.5 × 10^–5) is titrated with a 0.0228 M solution of hydrochloric acid as the titrant. What is the pH at the equivalence point? (Kw = 1.0 × 10^–14)
a) 9.81
b) 8.16
c) 3.02
d) 4.19
e) 5.84
Ans: e
A 50.00-mL solution of 0.0350 M trimethylamine (Kb = 6.5 × 10^–5) is titrated with a...
20. A 50.00-mL solution of 0.0350 M benzoic acid (Ka 6.4 x 10) is titrated with a 0.0134 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution after 15.00 mL of titrant have been added? (Kw 1.00 x 10-14) A) 2.83 B) 9 C) 4.19 D) 3.37 E) 1.46 9.6
A 25.0 mL sample of a 0.2800 M solution of aqueous trimethylamine is titrated with a 0.3500 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. pH after 20.0 mL of acid have been added =
A 25.0 mL sample of a 0.1300 M solution of aqueous trimethylamine is titrated with a 0.1625 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.
A 25.0-mL sample of a 0.250 M solution of aqueous trimethylamine is titrated with a 0.313 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 25degreeC. pH after 10.0 mL of acid have been added; 4.19 Number Did you find the pH or the pOH of this solution? pH after 20.0 mL of acid have been added: Number 3.65 pH after 30.0...
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
A 20.00-mL solution of 0.120 M nitrous acid (Ka = 4.0 × 10–4) is titrated with a 0.215 M solution of sodium hydroxide as the titrant. What is the pH of the acid solution at the equivalence point of titration? (if needed: Kw = 1.00 × 10–14)
24. 50.00 mL of 0.10 M CH3COOH (Ka = 1.8 x 10-5) is titrated with a 0.10 M KOH solution. After 50.00 mL of the KOH solution is added, the pH in the titration flask will be A) 4.28 B) 8.72 C) 9.41 D) 11.24 E) 12.08 [Kb = 5.6 x 10-10 for acetate ion] 0.0025 - 0.25 .
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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A 35.00−mL solution of 0.2500 M HF is titrated with a standardized 0.1825 M solution of NaOH at 25°C. Be sure to answer all parts. A 35.00-mL solution of 0.2500 M HF is titrated with a standardized 0.1825 M solution of NaOH at 25° C. (a) What is the pH of the HF solution before titrant is added? 1.9 (b) How many milliliters of titrant are required to reach the equivalence point? mL (e) What is the pH at 0.50...