A buffer was prepared by dissolving 22.61g of NaCLO2 into 0.100L of 4.00M aqueous HCLO2. Calculate the pH of the original Chlorous acid/chlorite ion buffer. Ka= 1.1 x 10^-2.

Please do not answer this question until after 5pm. Thank you.

5 pm what day. And is that EDT, CDT, PDT, MDT, or some other time.

The Henderson-Hasselbalch equation is what you want to use.

Hi Dr. Bob,

5pm Dec. 3rd EDT. Can you simply tell me if pH=1.75? I was just needing to see if I had the right answer. Thanks.

To calculate the pH of the chlorous acid/chlorite ion buffer, we need to consider the dissociation of chlorous acid (HCLO2) and the reaction with the chlorite ion (CLO2-) to form the chlorous acid/chlorite ion buffer.

First, let's calculate the number of moles of HCLO2 and CLO2- in the buffer solution:

Number of moles of HCLO2:
Moles = concentration (M) × volume (L)
Moles = 4.00 M × 0.100 L
Moles = 0.400 mol

Number of moles of NaCLO2:
Moles = mass (g) / molar mass (g/mol)
Moles = 22.61 g / 90.45 g/mol (molar mass of NaCLO2)
Moles = 0.250 mol

Since HCLO2 and CLO2- react in a 1:1 ratio, the number of moles of CLO2- in the buffer is also 0.250 mol.

Next, we need to determine the concentration of HCLO2 and CLO2- in the buffer solution:

Concentration of HCLO2:
Concentration = moles / volume (L)
Concentration = 0.400 mol / 0.100 L
Concentration = 4.00 M

Concentration of CLO2-:
Concentration = moles / volume (L)
Concentration = 0.250 mol / 0.100 L
Concentration = 2.50 M

Now, we can set up the expression for the acid dissociation constant (Ka) for chlorous acid:

Ka = [H+][CLO2-] / [HCLO2]

Since the concentration of CLO2- equals the concentration of HCLO2 in the buffer solution, we can substitute these values into the Ka expression:

Ka = [H+][CLO2-] / (Concentration of HCLO2)

To calculate [H+] and determine the pH, we rearrange the equation:

[H+] = Ka × (Concentration of HCLO2) / [CLO2-]

[H+] = (1.1 x 10^-2) × (4.00 M) / (2.50 M)

[H+] = 0.0176 M

To calculate the pH from the [H+] concentration, we use the equation:

pH = -log[H+]

pH = -log(0.0176)

After evaluating this expression, we find that the pH of the original chlorous acid/chlorite ion buffer is approximately 1.75.