# A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.

Question
1876 views

A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5.

check_circle

Step 1

HNO3 and NH3 react to give NH4+ and NO3-.

Step 2

Number of moles HNO3 and NH3 is determined using the formula for molarity.

Step 3

Volume of NH3 is 100mL whereas the volume of HNO3 is 150mL. It implies that HNO3 is in excess and hence all NH3 present in the gets converted to NH4+. The ionization of NH4+ is suppressed by HNO3 since it is a strong acid. Therefore, pH depends only on the c...

### Want to see the full answer?

See Solution

#### Want to see this answer and more?

Solutions are written by subject experts who are available 24/7. Questions are typically answered within 1 hour.*

See Solution
*Response times may vary by subject and question.
Tagged in

### Solutions 