100 mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point/endpoint.

1.) 150 mL of 1 M NaOH
2.) 200 mL of 1 M NaOH
3.) 50 mL of 1 M NaOH
4.) 100 mL of 1 M NaOH
5.) 5.00 mL of 1 M NaOH
6.) 10.0 mL of 1 M NaOH

1. After Equivalence Point

2. After Equivalence Point

3. Before Equivalence Point

4. At the Equivalence Point

5. Before Equivalence Point

6. Before Equivalence Point

Explanation:

First let's write down the balanced equation for this reaction:

The above equation proves that we need one mole of NaOH to reach the equivalence point with one mole of HCL.

Thus for 100 ml of the 1 mole solution of HCL, we would need a corresponding 100 ml of 1 mole NaOH solution.

So anything less than 100 ml will be before the equivalence point, and anything larger than 100 ml will be after the equivalence point.

The equivalence point will be reached at exactly 100ml.

The answers reflect the above statements.