# 1) A solution is prepared with 0.55 M HNO2 and 0.75 M KNO2. Fill in the ICE Table with the appropriate values

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Based on the calculations through the ICE table, the pH of the buffer solution is equal to 3.30.

Given the following data:

• Concentration of = 0.55 M.
• Concentration of = 0.75 M.
• Rate constant =

### How to determine the pH of the buffer solution.

First of all, we would write the properly balanced chemical equation for this chemical reaction:

Initial cond.                       0.55M              0          0.75M

-x                   x               x

At equib.                           0.55M - x         0 + x      0.75M + x

From the ICE table, the Ka for this chemical reaction is given by:

Now, we can calculate the pH of the buffer solution:

pH = 3.30.

Alternatively, you can calculate the pH of this buffer solution by applying Henderson-Hasselbalch equation:

Where:

• HA is acetic acid.
•  is acetate ion.