# Chemistry pH

A 0.60 M solution of a weak acid, HA, has a pH of 3.72. What is the percentage ionization of the acid? What is the value of Ka for the acid?

1. 👍 0
2. 👎 0
3. 👁 162
1. pH = -log(H^+)
pH = 3.72; (H^+) = approx 2E-4 but that's an approximation. You should do this more accurately as well as all of the calculations that follow.

%ion = [(H^+)/Msample]*100

...........HA ==> H^+ + A^-
I.........0.6.....0......0
C...........-x....x......x
E........0.6-x....x......x

You know x is approx 2E-4, Substitute that for x into the Ka expression for HA and solve for Ka.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

Select the statements that correctly describe buffers.? 1) The pH of a buffer solution does not change significantly when any amount of a strong acid is added. 2) The Ka of a buffer does not change when any amount of an acid is

2. ### CHEMISTRY

HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a

3. ### chemistry

A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka

4. ### chemistry

a 5.55g sample of a weak acid with ka=1.3*10^-4 was combined with 5.00ml of 6.00 M NAOH and the resulting solution was diluted to 750mL. The measured pH of the solution was 4.25. what is the molor mass of the weak acid. if used

1. ### chemistry

Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka of the acid. 2.) The pH of 0.100M solution of weak monoprotic acid HA is 2.85. What is the Ka of the acid?

2. ### chemistry

In acidic solution MnO4- oxidizes H3AsO3, a weak acid, to H3AsO4, a weak acid, and is reduced to Mn2+. Write the balanced net ionic equation for this reaction. How many H+ are there in the balanced equation

3. ### Chem

In acidic solution MnO4- oxidizes H3AsO3, a weak acid, to H3AsO4, a weak acid, and is reduced to Mn2+. Write the balanced net ionic equation for this reaction. How many H+ are there in the balanced equation? Question 8 answers

4. ### chemistry

A 15.00 mL sample of an unknown monoprotic weak acid solution is titrated with 0.35 M NaOH. The initial buret reading is 0.23 mL. The phenolphthalein indicator turns the solution light pink when the buret reads 29.58 mL. A. what

1. ### Chemistry- Acids and Buffers

Cyanic Acid is a weak acid HOCN + H2O H3O+ +OCN- ka= 3.5*10^-4 a) if 2.5ml of 0.01 M cyanic acid solution is added to 25.0 ml of a formis acid buffer with ph = 3.70, what is the ratio of [OCN-]/[HOCN] in the resulting solution? b)

2. ### chemistry

Lactic acid is a weak acid with the formula , HCH3H5O3, the Ka for lactic acid is 1.38 x 10-4. In aqueous solution, lactic acid partially dissociates according to the following reaction: HCH3H5O3 ⇔ CH3H5O3- + H+ Use the Ka

3. ### Chemistry

A 5.55g sample of a weak acid with Ka=1.3 x10^-4 was combined with 5.00 mL of 6.00 M NaOH and the resulting solution was diluted to 750 mL. The measured pH of the solution was 4.25. What is the molar mass of the weak acid?

4. ### Biochemistry

weak acid, HA, is 0.1 % ionized in a 0.2 M solution. (a) What is the equilibrium constant for the dissociation of the acid (Ka)? (b) What is the pH of the solution?