Question

1)

A 10.0 mL sample of 0.25 M NH₃(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH₃). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.

K_b of NH₃ is 1.8 × 10⁻⁵.

Henderson–Hasselbalch equation:

Part a):

1) After adding 10 mL of the HCl solution, the mixture is   [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.

2) The pH of the solution after adding HCl is [ Select ] ["8.65", "9.16", "7.00", "4.74"]         .

Part b):

3) After adding 12.5 mL of the HCl solution, the mixture is [ Select ]["after", "at", "before"]         the equivalence point on the titration curve.

4) The pH of the solution after adding HCl is [ Select ] ["2.85", "5.11", "7.00", "4.93"]         .

Part c):

5) After adding 30.0 mL of the HCl solution, the mixture is [ Select ] ["after", "before", "at"] the equivalence point on the titration curve.

6)) The pH of the solution after adding HCl is [ Select ]["1.06", "7.00", "9.16", "2.46"]      

2)The titration curve shown below represents a 25 mL aqueous solution that is titrated with another solution at the same molarity.

Determine if each of the following statements regarding the titration curve is True or false.

1) The curve could represent the titration of NaOH with HCl (adding HCl to NaOH).   

2) At point A, the pH of the solution only depends on the concentration of the acid.   

3) Point B is in a buffer region.

4) Point C is the equivalence point.   

5) There is excess base present at Point D

Answer 1

The answer is attach below