Answer:-
this question solved by first writing the ionization equation of acetic acid and the expression of Ka for acetic acid and using approximation.
the answer is given in the image.
11. For a solution that is 0.150 M in acetic acid, HC2lH3O2, calculate the [H30'] based on the reaction below given that Ka- 1.75 x 103 for this weak acid. Use the approximation method Also, c...
Calculate the Ka of a weak acid if a 0.150 M solution of this acid has a pH of 3.80
in an experiment, 5.00 mL 0.100 M acetic acid (Ka = 1.75 x 10^-5 at 25 C) was titrated with 0.100 M NaOH solution. The system will attain this pH after 10.0 mL of the titrant has been added
(a) HA (aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a 0.061 M solution in A- (aq)? The temperature is 25oC. (b) For the reaction A (g) ⇋ B (g) + C (g), the equilibrium constant is 1.80 at 25.0oC and 4.46 at 75.0oC. Making the approximation that ΔH and ΔS do not change with temperature, calculate the value of the equilibrium constant at 50.0oC as well as the...
1. Calculate the pH at 25°C of a 0.757 M solution of a weak acid that has Ka = 9.28 x 10 2. Determine the Kb of a weak base if a 2.50 M solution of the base has a pH of 9.595 at 25°C. 3. The overall dissociation of malonic acid, H2C3H2O4, is represented below. The overall dissociation constant is also indicated. H2C3H204 = 2 H+ + C3H2042- K = 3.0 x 10-9 To a 0.025-molar solution of malonic...
Calculate the pH of a .30 M solution of acetic acid (CH3COOH, Ka= 1.8 x 10^-5) at 25 degrees Celsius.
a) A solution contains 0.34 M of a weak acid HA (Ka = 2.0 x 10-7) and 0.17 M NaA. What is the pH after 0.05 M of HCl is added to this solution (assume no volume change) b) The pH of a solution containing 0.1 M of a weak acid HA is 6. Calculate Ka for this acid. Note the acids are unrelated for the two problem parts.
Weak-Acid Strong-Base Titrations. These next questions relate to a 25 mL aliquot of 0.35 M acetic acid (Ka = 1.77 x 10) that is titrated with 0.20 M potassium hydroxide (KOH). (f) What is the pH of the acetic acid solution before the titration begins? (g) What is the pH after 14 mL of 0.20 M KOH has been added to the solution? Use the Henderson-Hasselbalch equation. (h) What is the pH at the equivalence point?
a) (4 marks) HA (aq) is a weak acid with a dissociation constant, Ka, of 1.0 x 10-11. What is the pH of a 0.061 M solution in A- (aq)? The temperature is 25oC. (b) (4 points) For the reaction A (g) ⇋ B (g) + C (g), the equilibrium constant is 1.80 at 25.0oC and 4.71 at 75.0oC. Making the approximation that ΔH and ΔS do not change with temperature, calculate the value of the equilibrium constant at 50.0oC...
12. Given that Ka = 1.8 x 10- for acetic acid. in order for an acetic acid solution to have a pH of 3.50, its molar concentration must be a. 5.7 x 10-3 M b. 5.6 x 10-3M c. 3.2 x 10-4M d. 2.3 x 10-M 13. If enough base is added to a solution to cause the pH to increase from 7.50 to 8.50, this means that А a. [OH-] increases by a factor of 10 b. [H'] increases...
#3 (a) HA (aq) is a weak acid with a dissociation constant, Ka, of 2.0 x 10-15. What is the pH of a 0.04 M solution in A- (aq)? The temperature is 25oC. (b) For the reaction A (g) ⇋ B (g) + C (g), the equilibrium constant is 2 at 25.0oC and 3 at 75.0oC. Making the approximation that ΔH and ΔS do not change with temperature, calculate the value of the equilibrium constant at 50.0oC as well as...