A buffer solution contains HC2H3O2 at a concentration of 0.225 M NaC2H3O at a concentration of 0.164 M. The value of Ka for acetic acid is 1.75 × 10-5. Calculate the pH of this solution using the Henderson-Hasselbalch equation. Could you please show steps...thanks a bunch...:)

If you can read and substitute there is nothing to this.

pH = pKa + log[(base)/(acid)]
Calculate pKa from pKa = -log Ka. I think that is something like 4.76. Then
(base) = the acetate = 0.164M
(acid) = the acetic acid = 0.225M
Plug and chug.

Sure! The Henderson-Hasselbalch equation is:

pH = pKa + log([A-]/[HA])

First, we need to find the concentrations of acetic acid (HA) and acetate ion (A-).

Given:
[HA] = 0.225 M (concentration of acetic acid)
[A-] = 0.164 M (concentration of acetate ion)
Ka = 1.75 × 10^(-5)

To find pKa, take the negative logarithm of Ka:
pKa = -log(Ka)

Now, we can calculate pKa:

pKa = -log(1.75 × 10^(-5))

Next, let's substitute the values into the Henderson-Hasselbalch equation:

pH = pKa + log([A-]/[HA])

pH = pKa + log(0.164/0.225)

Now, solve for pH:

pH = (-log(1.75 × 10^(-5))) + log(0.164/0.225)

pH = (-(-4.756)) + log(0.727)

pH = 4.756 + (-0.135)

pH = 4.62

Therefore, the pH of the buffer solution is 4.62.

Sure! To calculate the pH of a buffer solution using the Henderson-Hasselbalch equation, you need to know the concentrations of the acid and its conjugate base, as well as the acid dissociation constant (Ka).

The Henderson-Hasselbalch equation is given by:

pH = pKa + log ([conjugate base] / [acid])

In this case, the acid is acetic acid (HC2H3O2) and its conjugate base is sodium acetate (NaC2H3O2).

Step 1: Find the pKa
To find the pKa of acetic acid, take the negative logarithm of the Ka value:
pKa = -log(Ka) = -log(1.75 × 10^-5)

Step 2: Calculate the ratio of conjugate base to acid
The ratio [conjugate base] / [acid] is given by the concentrations of the conjugate base and acid in the buffer solution. In this case, [conjugate base] = 0.164 M (concentration of NaC2H3O2) and [acid] = 0.225 M (concentration of HC2H3O2).

Step 3: Plug the values into the Henderson-Hasselbalch equation
pH = pKa + log ([conjugate base] / [acid])
= pKa + log (0.164 / 0.225)

Step 4: Calculate the pH
Use a calculator or logarithm table to calculate the logarithm result:
Log (0.164 / 0.225) = -0.249

Now, substitute the value of pKa and the logarithm into the equation:
pH = -log (1.75 × 10^-5) - 0.249

Using a calculator, find the pKa value and add -0.249 to it to get the pH value of the buffer solution.

Remember to round your final pH value to the appropriate number of decimal places.