# How can I calculate the titration of a weak acid and a strong base?

##### 1 Answer

There are some critical pH values you will need to calculate

- At the very beginning
- At the equivalence point
- Between neutralization and the equivalence point
- After the equivalence point

Assume that you are titrating 25 mL of 0.1 mol/L

**At the beginning**

You know from your ICE table that

**At the equivalence point**

You know that the equivalence point will be at 25 mL of

The

**At points between 0 mL and the equivalence point**

Use the Henderson-Hasselbalch Equation.

Calculate the moles of

For example, at 12.5 mL, you will have added 0.001 25 mol of base. You will have neutralized 0.001 25 mol of

**After the equivalence point**

You will just be adding excess moles of

Calculate the excess moles, divide by the volume to get the molarity. Then calculate the pOH and the pH.

For example, after 40 mL of base, you will have added 0.004 mol of

You will have 0.0015 mol of

Your calculated values should match the graph below.