50 ml sample of 0.0950 M acetic acid (ka: 1.8* 10-5) isbeing titrated with 0.106 M...
A 50.00 mL sample of 0.0950 M acetic acid (Ka = 1.8 x 10-5) is being titrated with 0.106 M NaOH. What is the pH at the half-way point of the titration? (22.41 mL of 0.106 M NaOH has been added) A) 3.06 B) 5.04 C) 4.44 D) 3.18 E) 4.74
A sample of 0.100 M acetic acid (Ka = 1.8 × 10−5) in 50.0 mL of solution is titrated with standard 0.100 M NaOH. What is the pH in the titration flask after addition of 15.0 mL of NaOH?
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
Determine the pH during the titration of 29.5 mL of 0.324 M acetic acid (Ka = 1.8×10-5) by 0.414 M NaOH at the following points. (a) Before the addition of any NaOH ________ (b) After the addition of 5.70 mL of NaOH _______ (c) At the half-equivalence point (the titration midpoint) _______ (d) At the equivalence point _______ (e) After the addition of 34.6 mL of NaOH ________
2. A sample of 50 ml of nitrous acid (KA = 5.6 x 10“) is titrated with 0.070 M NaOH. The equivalence point is reached after the addition of 43.2 ml of the strong base. a) (3 marks) What is the pH of the solution at the equivalence point? b) (3 marks) What is the pH of the solution after 50 ml of NaOH has been added to the original nitrous acid solution?
When a 29,8 mL sample of a 0.322 M aqueous acetic acid solution is titrated with a 0,434 M aqueous sodium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 33.2 mL of sodium hydroxide have been added?
When a 23.8 mL sample of a 0.491 M aqueous acetic acid solution is titrated with a 0.381 M aqueous potassium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 46.0 mL of potassium hydroxide have been added
A 32.44 mL sample of 0.202 M acetic acid is titrated with 0.185 M sodium hydroxide. Calculate the pH of the solution for each the following. You will need to look up values for ionization constants. Using your answers for 1-5, sketch the titration curve. Be sure to label axes, midpoint, and equivalence point, and to identify each of the five data points on the curve. before any NaOH is added. at the midpoint after 24.00 mL of NaOH is added. at the equivalence...
Consider the titration of 50 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 0.200 M NaOH solution. Show all calculations for full credit. a) Write the titration reaction: b) Calculate the pH after 5.00 mL of NaOH: c) Calculate the pH after 12.5 mL of NaOH: d) Calculate the pH after 25 mL of NaOH:
Consider the titration of 50 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 0.200 M NaOH solution. Show all calculations for full credit. a) Write the titration reaction: b) Calculate the pH after 5.00 mL of NaOH: c) Calculate the pH after 12.5 mL of NaOH: d) Calculate the pH after 25 mL of NaOH: