The pH of a 0.053 M weak monoprotic acid is 3.05. Calculate the K, of the...

Question

Question

Answer 1

Answer #1

Q1. K_a = 1.52 x 10^-5

Q2. percentage = 1.59 %

Explanation

Q1. pH = 3.05

[H⁺] = 10^-pH

[H⁺] = 10^-3.05

[H⁺] = 8.9 x 10^-4 M

K_a = [H⁺]² / (C - [H⁺])

where C = initial concentration of acid = 0.053 M

K_a = (8.9 x 10^-4 M)² / (0.053 M - 8.9 x 10^-4 M)

K_a = 1.52 x 10^-5

Answer 2

Similar Homework Help Questions

Be sure to answer all parts. The pH of a 0.051 M weak monoprotic acid is...

Be sure to answer all parts. The pH of a 0.051 M weak monoprotic acid is 3.41. Calculate the K, of the acid. x 10 K = Enter your answer in scientific notation.
The K, of a monoprotic weak acid is 0.00687. What is the percent ionization of a...

The K, of a monoprotic weak acid is 0.00687. What is the percent ionization of a 0.100 M solution of this acid? percent ionization: If the K, of a weak base is 6.1 x 10, what is the pH of a 0.50 M solution of this base?
++ ++ ++ ++ ++ The K, of a monoprotic weak acid is 0.00677. What is...

++ ++ ++ ++ ++ The K, of a monoprotic weak acid is 0.00677. What is the percent ionization of a 0.120 M solution of this acid? percent ionization: If the Ka of a monoprotic weak acid is 6.4 x 10-6, what is the pH of a 0.21 M solution of this acid? pH =

A buffer containing acetic acid and sodium acetate has a pH of 5.55. The K, value...

A buffer containing acetic acid and sodium acetate has a pH of 5.55. The K, value for CH3CO,H is 1.80 x 10. What is the ratio of the concentration of CH3CO H to CH3CO,t? [CH,CO,H1 CH2C0, 1 = Calculate the pH of a solution that has an ammonium chloride concentration of 0.054 M and an ammonia concentration of 0.053 M. Kb = 1.8 x 10-5 pH = What is the pH of 0.35 M acetic acid to 1.00 L of...
This problem deals with Acid-base titrations and pH scale for a weak acid and a weak...

This problem deals with Acid-base titrations and pH scale for a weak acid and a weak base. Calculate the pH of the solution that results from adding 7.5 [ml] of Ammonia (NH3) to a beaker that contains, 100 ml of distilled water and 15 ml of 0.1 M Acetic acid (HC2H3O2). A buret containing 50 mL of 0.1 M Ammonia (NH3) is being used as the titrant. The beaker containing 100 ml of distilled water, and 15 ml of 0.1...
If the K, of a monoprotic weak acid is 1.3 x 10 , what is the pH of a 0.27 M solution of this acid? pH =

If the K, of a monoprotic weak acid is 1.3 x 10 , what is the pH of a 0.27 M solution of this acid? pH =

Ammonia, NH3, is a weak monoprotic base with Kb = 1.76 × 10−5. Calculate the pH...

Ammonia, NH3, is a weak monoprotic base with Kb = 1.76 × 10−5. Calculate the pH of a 0.00779 M solution of this base. Report your answer to TWO places past the decimal.
What is the percent ionization of a monoprotic weak acid solution that is 0.179 M? The...

What is the percent ionization of a monoprotic weak acid solution that is 0.179 M? The acid-dissociation (or ionization) constant, K,, of this acid is 2.32 x 10-
2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M...

2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M 0.100 M 0.0500 M 0.00100 M b. NaOH (strong base) 0.100 M 0.0500 M 0.0100 M Experiment 4 с. НС2Н3О2 (weak acid) (Ka 1.8 x 10-5) 0.100 M 0.0500 M 0.0100 M d. K2CO3 (weak base) (K, = 2.1 x 10-4) 0.100 M 0.0500 M 0.0100 M 2. Calculate the pH expected for the following monoprotic substances. a. HCl (strong acid) 0.0100 M 0.100...

A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What...

A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+ (aq) + A (aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, K ? Answer in scientific...