Question

Consider the following two buffers:

(i) 10.0 mL of a buffer that contains 0.10 M HClO and 0.10 M NaClO

(ii) 10.0mL of a buffer that contains 0.050 M HClO and 0.10 M NaClO

b.) 8 drops of 1.0 M NaOH (aq) is added to each of these buffers.

1.)Give the balanced net-ionic equation for the reaction that occurs when the NaOH (aq) is added.

2.)For which buffer (i or ii) does the pH change the greatest amount when the NaOH (aq) is added? Explain why.

c.) Now consider a fresh 20.0 mL sample of buffer (i): 0.10 M HClO and 0.10 M NaClO. What component of the buffer must be added to change the pH to 7.95? What mass of this component must be added? You can assume negligible volume change.

Edit: Ka of HClO 2.9 * 10^-8

This was all that was provided on the paper.

Answer 1