Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.0 M acetic acid.

a. What would be the initial pH of Buffer C? HOW???????

(Acetate ion) = ?

moles = grams/molar mass
M = moles/0.1L
(acetic acid) = 1M

pH = pKa + log(acetate)/(acetic acid)
pKa = -logKa

Yeah i know it now it is the henderson Hasselbach equation

To determine the initial pH of Buffer C, you need to consider the acid-base equilibrium reaction between acetic acid (CH3COOH) and sodium acetate (NaC2H3O2). The equation for this reaction is:

CH3COOH + H2O ↔ CH3COO- + H3O+

The initial pH of the buffer solution depends on the concentrations of acetic acid and acetate ions. To calculate the pH, you can use the Henderson-Hasselbalch equation, which is given by:

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

Where:
- pH is the measure of acidity or alkalinity of the solution.
- pKa is the logarithmic value of the acid dissociation constant (Ka) for acetic acid, which is equal to the pH at which half of the acid is dissociated into ions and half is unionized.
- [A-] is the concentration of the acetate ion.
- [HA] is the concentration of the acetic acid.

In this case, the initial concentration of acetic acid is 1.0 M, and you mixed 8.203 g of sodium acetate in 100.0 mL of solution. To determine the concentration of acetate ion ([A-]), you need to convert grams to moles and then divide by the total volume of the solution.

1. Convert grams of sodium acetate to moles:
molecular weight of sodium acetate (NaC2H3O2) = 82.03 g/mol
moles of NaC2H3O2 = 8.203 g / 82.03 g/mol

2. Convert mL to L:
total volume = 100.0 mL / 1000 mL/L

3. Calculate the concentration of acetate ion ([A-]):
[A-] = moles of NaC2H3O2 / total volume

Once you have the concentration values for [A-] and [HA], you can substitute them into the Henderson-Hasselbalch equation to find the initial pH of Buffer C.