Answer:-
Firstly ionization equation is written then using the expression of Ka and its value, pH is calculated at different points during titration.
The answer is given in the image,
IV. Acid-Base Titration (15 points). A 50 mL of 0.200 M HNO2, (Ka= 4.0 x 10)...
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:
a) An unknown indicator (called “HIn”) has a Ka of 4.0 x 10-6. The color of the neutral form is green, and that of ionized form is red. The indicator is added to a HCl solution, which is then titrated against a NaOH solution. At what pH will the indicator change color? b) 350. mL of a NaOH solution was added to 500. mL of 2.50 M HNO2. The pH of the mixed solution was 1.75 units greater than that...
50.0 mL of 0.090 M nitrous acid (HNO2, Ka = 7.1 x 10-4), is titrated with 0.100 M NaOH, requiring 45.0 mL of strong base to reach the equivalence point. (a) What will be the pH after 35.0 mL of NaOH have been added? (b) What will be the pH at the equivalence point? (c) What will be the pH after 60.0 mL of NaOH have been added?
1.A 25.00 ml smaple of 0.523 M nitrous acid, HNO2, solution is titrated with a 0.213 M NaOH. For HNO2, Ka = 4.0 X 10^-4 a) What is the pH before any NaOH is added? b) Write the reaction that takes place as KOH solution is added to the HNO2 solution. c) write the reaction that determines the pH at the equivialnce point. -What is the pH at the equivilance point -what is the pH at the 1/2 equivilance point...
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:
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?
a) A 41.0 mL sample of 0.194 M HNO2 is titrated with 0.220 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH. b) A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 56.7 mL 0.200 M HNO3.
Consider the titration of 100.0 mL of 0.200 M acetic acid ( Ka = 1.8 x 10-5) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a 0.0 mL pH= 50.0 mL pH = C 100.0 mL pH = 140.0 mL pH= C 200.0 mL pH = f 240.0 mL pH=
(ueak acid/shing base 3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka-1.80 x 10") with 0.100 M NaOH: VNOH 0.00 mL, 15.00 mL, 25.00 mL, 40.00 mL. Draw a graph of pH vs. VaoH. (30 points) (b) Buffer capacity can be thought of as how well a solution resists changes in pH after a strong base/acid is added. A buffer is most effective to resisting pH changes when what...
Acid HX is a weak acid with Ka = 1.0 x 10–6 . A 50.0 mL sample of 1.00 M HX(aq) is titrated with 1.00 M NaOH(aq). What is the pH of the solution at the points listed below during the titration? For each question, write the letter of the correct choice from the choices given below. A) 0.0 B) 1.0 C) 3.0 D) 6.0 E) 6.6 F) 7.0 G) 8.0 H) 9.85 I) 12.0 J) 13.0 12. Before any...