What is the ph of a buffer solution upon mixing 15.0 ml of 0.40 m hcl and 20.0 ml of 0.50 m nh? kb (nh3) = 1.8 x 10 e. 7.00 a. 9.43 b. 9.26 c. 9.08 d. 8.11

The pH of resulting solution is 9.08

Explanation:

To calculate the number of moles for given molarity, we use the equation:

      ........(1)

Molarity of HCl = 0.40 M

Volume of solution = 15.0 mL

Putting values in equation 1, we get:

Molarity of ammonia = 0.50 M

Volume of solution = 20.0 mL

Putting values in equation 1, we get:

The chemical reaction for hydrochloric acid and ammonia follows the equation:

Initial:          0.006      0.01

Final:             -         0.004              0.006

Volume of solution = 15.0 + 20.0 = 35.0 mL = 0.035 L    (Conversion factor:  1 L = 1000 mL)

We are given:

= negative logarithm of base dissociation constant of ammonia =

pOH = ?

Putting values in above equation, we get:

To calculate pH of the solution, we use the equation:

Hence, the pH of the solution is 9.08

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