<u>Answer:</u> The pH of resulting solution is 9.08
<u>Explanation:</u>
To calculate the number of moles for given molarity, we use the equation:
........(1)
- <u>For HCl:</u>
Molarity of HCl = 0.40 M
Volume of solution = 15.0 mL
Putting values in equation 1, we get:
- <u>For ammonia:</u>
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)
- To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:
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
