Assume that a 50.00 mL sample of 0.1000 M HCl in an Erlenmeyer flask is titrated...
A 50.00 ml aliquot of 0.1000 M NaOH is titrated with 0.1000 M HCL. Calculate the pH of the solution after the addition of 0.00, 10.00, 25.00, 40.00, 45.00, 49.00, 50.00, 51.00, 55.00, and 60.00 ml of acid and prepare a titration curve from the data.
Construct a curve for the titration of 50.00 mL of a 0.1000 M solution of compound A with a 0.2000 M solution of compound B in the following table. For each titration, calculate the pH after the addition of 0.00, 12.50, 20.00, 24.00, 25.00, 26.00, 37.50, 45.00, 49.00, 50.00, 51.00, and 60.00 mL of com- pound B. A (a) H2SO3 (b) ethylenediamine (c) H2SO4 B NaOH HCl NaOH
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...
A 25.00 mL sample of 0.310 M NaOH is titrated with 0.750 M HCl at 25 °C. Calculate the initial pH before any titrant is added. Calculate the pH of the solution after 5.00 mL of the titrant is added.
1. If 40.00 mL of 0.050 M HCl is titrated with 0.100 M NaOH, what is the pH at the following "times?" (9 pts) a. Before any NaOH is added. b. After 20.00 mL of NaOH is added. c. After 500 mL of NaOH is added. 2. If 50.00 mL of 0.050 M formic acid, HCHO, (yes, you need to look up the Ka for formic acid) is titrated with 0.050 M NaOH, what is the pH at the following...
Titrations 1. A 50.00-ml NaOH sample of unknown concentration was titrated with 0.1274 M HCI. if 33.61 mL of the HCl solution were required to neutralize the NaOH sample, what is the molarity of the NaOH sample? Show the steps in your calculation 2. A 25.00-ml HCl sample of unknown concentration was titrated with 0.5631 M Al(OH)3. If 37.62 mL of the Al(OH) solution were required to neutralize the HCl sample, what is the molarity of the HCl sample? (Assume Al(OH)3 is...
50.00 mL of 0.100M of a weak acid (Ka=1.3x10-5) is titrated with 0.100M NaOH. a. Compute the volume of NaOH required to reach the equivalence point. b. Calculate the pH of the original solution before any NaOH has been added. c. After 30.00 mL of NaOH has been added, what is the pH of the solution? d. What is the pH at the equivalence point? e. Write a brief explanation as to why it is...
A 50.00 mL aliquot of 0.1548 M benzoic acid is titrated with 0.1325 M sodium hydroxide. Find (a) V. (b) the initial pH, (c and d) the pH after 10.00 and 30.00 mL are added, (e) the pH at Vand (1) the pH at V. + 10.00 mL. Sketch the titration curve. You may use all usual "assumptions" for the pH calculations. Benzoic acid is a weak acid. Write the numeric answers here: Sketch the titration curve here: a. mL...
A student performs a titration in the laboratory. A 20.0 mL sample of 0.080 M HCl is titrated with 0.10 M NaOH. What would be the pH of the solution after 25.0 mL of the base has been added? __ 13.05 __ 9.80 __ 10.00 __ 12.30
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH(aq) with 0.2000 M NaOH(aq) after 2.5 mL of the base have been added. Ka of acetic acid = 1.8 x 10-5. QUESTION 9 Calculate the pH during the titration of 30.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.1000 M HCl(aq) after 26 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4. QUESTION 10 Calculate the pH during the titration of 20.00...