A single extraction with 100 mL of CHCl3 extracts or removes 88.5% of the weak acid,...

A single extraction with 100 mL of CHCl₃ extracts or removes 88.5% of the weak acid, HA, from 50 mL of aqueous solution. What is the Distribution coefficient, D, for HA at a pH = 3.00? The K_a for HA is 3.5 x 10^-5.

Expert Solution

queen_honey_blossom answered 9 months ago

You mix 50.0 mL of a weak monoprotic acid with 50.0 mL of NaOH solution in...

You mix 50.0 mL of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions (and the calorimeter) were initially at 22.0C. The final temperature of the neutralization reaction was determined to be 22.5C. a) What is the total amount of heat evolved in this reaction? Show all work. b) If 0.135 moles of the monoprotic acid were neutralized in this reaction, what is the molar heat of neutralization (enthalpy) for this reaction?

Formic acid is a weak acid with pKa = 3.75. How many mL of 0.10 M...

Formic acid is a weak acid with pKa = 3.75. How many mL of 0.10 M NaOH solution should be added to 100.0 mL of 0.10 M formic acid solution to make a buffer solution with pH = 3.27 A) 0 B) 25 C) 50 D) 75 E) 100

You are titrating 25.00 mL of a 0.100 M solution of a weak acid with a...

You are titrating 25.00 mL of a 0.100 M solution of a weak acid with a 0.250 M solution of potassium hydroxide. Assume the pKa of the weak acid is 5.6. A. What is the pH after adding 3.0 mL of 0.250 M potassium hydroxide? B. What is the pH at the midpoint of the titration? C. What is the pH at the equivalence point of the titration?

500.0 mL of 0.140 M NaOH is added to 565 mL of 0.250 M weak acid...

500.0 mL of 0.140 M NaOH is added to 565 mL of 0.250 M weak acid (Ka = 8.39 × 10-5). What is the pH of the resulting buffer? HA(aq)+OH^-(aq)=H2O(l)+ A^-(aq) pH=?

500.0 mL of 0.150 M NaOH is added to 605 mL of 0.200 M weak acid...

500.0 mL of 0.150 M NaOH is added to 605 mL of 0.200 M weak acid (Ka = 5.15 × 10-5). What is the pH of the resulting buffer?

6. You mix 50.0 mL of a weak monoprotic acid with 50.0 mL of NaOH solution...

6. You mix 50.0 mL of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions (and the calorimeter) were initially at 22.0OC. The final temperature of the neutralization reaction was determined to be 22.5OC. a) What is the total amount of heat evolved in this reaction? Show all work. b) If 0.135 moles of the monoprotic acid were neutralized in this reaction, what is the molar heat of neutralization (enthalpy) for this...

500.0 mL of 0.140 M NaOH is added to 595 mL of 0.200 M weak acid...

500.0 mL of 0.140 M NaOH is added to 595 mL of 0.200 M weak acid (Ka = 2.29 × 10-5). What is the pH of the resulting buffer? HA (aq) + OH (aq) ---> H2O (L) + A (aq)

The solubility of benzoic acid in water is 6.80g per 100 mL at 100 ℃, and 0.34g per 100 mL at 25 ℃.

The solubility of benzoic acid in water is 6.80g per 100 mL at 100 ℃, and 0.34g per 100 mL at 25 ℃.(a) Calculate the min. volume of water needed to dissolve 1.00g of benzoic acid at 100 ℃. (b) Calculate the maximum theoretical percent recovery from the recrystallization of 1.00g benzoic acid from 15 mL of water assuming the solution is filtered at 25 ℃?

1.) Acetic acid is a weak monoprotic acid with Ka=1.8*10^-5. In an acid base titration, 100...

1.) Acetic acid is a weak monoprotic acid with Ka=1.8*10^-5. In an acid base titration, 100 mL of 0.100M acetic acid is titrated with 0.100M NaOH. What is the pH of the solution: a.)Before any NaOH is added b.)Before addition of 15.0mL of 0.100M NaOH c.)At the half-equivalence point d.)After addition of total of 65.0mL of 0.100M NaOH e.)At equivalence point f.)After addition of a total of 125.0mL of 0.100M NaOH

Jackie diluted 7.5 mL weak acid with 7.5 mL distilled water. Then she titrated the diluted...

Jackie diluted 7.5 mL weak acid with 7.5 mL distilled water. Then she titrated the diluted weak acid with 0.100 M NaOH. It takes 22.52 mL of NaOH to reach the equivalence point. What is the original concentration of the weak acid? What is the diluted concentration of the weak acid?

Question