Question

In: Chemistry

Use the data from the most concentrated solution of acetic acid to calculate the Ka value...

Use the data from the most concentrated solution of acetic acid to calculate the Ka value for acetic acid. Clearly show all of your work below. mot concentrated solution of acetic acid is 0.116m..ph = 2.85

Expert Solution

Let a be the dissociation of the weak acetic acid
HA <---> H ⁺ + A^-

initial conc. c 0 0

change -ca +ca +ca

Equb. conc. c(1-a) ca ca

Dissociation constant , K_a = ca x ca / ( c(1-a)

= c a² / (1-a)

In the case of weak acids α is very small so 1-a is taken as 1

So K_a = ca²

==> a = √ ( K_a / c )

Given c = concentration = 0.1 M

pH = 2.85

- log[H⁺] = 2.85

[H⁺] = 10^-2.85

= 1.41x10^-3 M

But [H⁺] = ca

1.41x10^-3 = 0.116 x a

a = 0.0122

K_a = ca² = 0.116x(0.0122)²

= 1.72x10^-5

Therefore K_a = 1.72x10^-5

queen_honey_blossom answered 1 year ago

Calculate the percent ionization of 1.50 M aqueous acetic acid solution. For acetic acid, Ka =...

Calculate the percent ionization of 1.50 M aqueous acetic acid solution. For acetic acid, Ka = 1.8 × 10−5 . (a) 2.71% (b) 3.55% (c) 1.78% (d) 0.35% (e) None of the above

Calculate the pH and pOH of a 0.50 M solution of Acetic Acid. The Ka of...

Calculate the pH and pOH of a 0.50 M solution of Acetic Acid. The Ka of HOAc is 1.8 x10-5 [H3O+]/(0.50-0.00095)=1.8x10-5 where did they get the .00095, its said to take that as the second assumption [H3O+]=9.4x10-4 [H3O+]/(0.50-0.00094)=1.85x10-5 [H3O+]=9.4x10-4 (this is said to be the third assumption) Please, please help I really dont understand this, please show all steps and be as descriptive as possible.

Calculate the pH of a 0.100M NaCH3COO solution. Ka for acetic acid, HC2H3O2 is 1.8x10-5

Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8...

Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8 × 10-5. If someone could list the steps and calculations that would be helpful. Thank you!

Calculate the pH of a 0.100 M sodium benzoate, NaC6H5CO2, solution. The Ka of acetic acid...

Calculate the pH of a 0.100 M sodium benzoate, NaC6H5CO2, solution. The Ka of acetic acid is 6.3 x 10-5

Calculate the pH of a 0.51 M CH3COOK solution. (Ka for acetic acid = 1.8×10−5.)

Calculate the pH of a 0.800M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8×10^-5.

Calculate the pH of 0.10 M sodium acetate solution ( Ka, acetic acid = 1.76 x...

Calculate the pH of 0.10 M sodium acetate solution ( Ka, acetic acid = 1.76 x 10-5 ).

pH of acetic acid solutions. Remember, acetic acid is a weak acid, with a Ka =...

pH of acetic acid solutions. Remember, acetic acid is a weak acid, with a Ka = 1.8 x 10−5. Obtain 10.0 mL of 0.10 M acetic acid and place in a clean dry 50.0 mL beaker. Predict the value of the pH. Measure the pH with the pH meter. Record the value. Take 1.00 mL of the 0.10 M CH3COOH(aq) in the previous step, and put it in another clean beaker. Add 9.00 mL of deionized water and stir. What...

3. a) Calculate the pH of a sodium acetate-acetic acid buffer solution (Ka= 1.78 x 10-5)...

3. a) Calculate the pH of a sodium acetate-acetic acid buffer solution (Ka= 1.78 x 10-5) in which the concentration of both components is 1.0 M. What would be the pH of the solution if 1.5 mL of 0.50 M NaOH was added to 35.0 mL of the buffer? How much does the pH change? b) If the same amount and concentration of NaOH was added to 35.0 mL of pure water (initial pH = 7), what would be the...