i posted this question previously and got help however im still having some confusion. can u clarify ?
what's the pH of the acid HC2H3O2 with concentration of .15?
Bob Pursley worked that problem for you and gave it as
[x^2/0.15] = Ka.
What is it you don't understand? You know Ka, solve for x which is H^+, and convert to pH.
Sure, I'd be happy to clarify.
In the given problem, you have an acid with the formula HC2H3O2 and a concentration of 0.15. The first step to finding the pH of this acid is to find the concentration of H+ ions in the solution. To do this, you can use the equilibrium constant expression for the acid dissociation reaction.
The equilibrium constant (Ka) for the dissociation of the acid HC2H3O2 can be given as:
Ka = [H+][C2H3O2-] / [HC2H3O2]
Now, let's consider that the initial concentration of HC2H3O2 is 0.15 M, and assuming that it is a strong acid, it dissociates completely into H+ and C2H3O2-. Therefore, the concentration of HC2H3O2 at equilibrium is 0 M, and the concentration of C2H3O2- is also 0 M.
So, the equilibrium constant expression can be simplified to:
Ka = [H+][C2H3O2-] / 0
Since the concentration of HC2H3O2 at equilibrium is 0 M, it can be ignored.
Therefore, the equation becomes:
Ka = [H+](0)
From this equation, we can understand that the concentration of H+ ions must be determined in order to calculate the pH of the solution.
To solve for the concentration of H+, you need to rearrange the equation:
[H+] = Ka / [C2H3O2-]
The dissociation constant Ka is a known value for HC2H3O2, and [C2H3O2-] is zero in this case. So, you can substitute these values into the equation to calculate the [H+] concentration.
Once you have the H+ concentration, you can convert it to pH using the formula:
pH = -log[H+]
By plugging in the value for [H+], you can find the pH of the solution.
I hope this explanation clarifies the steps involved in finding the pH of HC2H3O2. If you have any further questions or need additional clarification, feel free to ask!