An unknown weak acid, HA, it titrated with 1.2 M NaOH. The pH at the halfway point of this titration was found to be 4.081. If the initial pH of the weak acid solution (before titration) has a pH of 2.348, what was the concentration of the weak acid solution

The initial concentration of weak acid solution is 0.243 M

Explanation:

We are given:

pH of unknown acid at the halfway point of titration = 4.081

We know that:

    (At halfway point)

To calculate the , we use the equation:

Putting values in above equation, we get:

As, the initial pH of the acid is 2.348

Putting values in above equation, we get:

The chemical equation for the ionization of weak acid follows:

The expression of for above equation:

As,

Putting values in above equation, we get:

Hence. the initial concentration of weak acid solution is 0.243 M

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.

the answer is a! (2.9 x 10^-18 j) hope i could someone. : )