a 2.0M solution of Hbr will have what pH?
HBr is a strong acid. It ionizes 100%; therefore, 2.0 M HBr has (H^+) = 2.0
Then pH = -log(H^+). Don't be surprised when the answer comes out negative.
thank you!
To determine the pH of a 2.0M solution of HBr (hydrobromic acid), you need to know the acid dissociation constant (Ka) and the concentration of the acid.
The acid dissociation constant (Ka) is a measure of the extent to which an acid donates a proton (H+) in an aqueous solution. For HBr, which is a strong acid, its Ka is very high, meaning it dissociates almost completely in water.
To find the pH of a strong acid solution, you can use the formula:
pH = -log[H+]
In this case, the concentration of H+ is equal to the concentration of HBr because it fully dissociates. Therefore, the concentration of H+ in a 2.0M HBr solution is also 2.0M.
Substituting this concentration into the formula, we have:
pH = -log(2.0)
Using a calculator, we find that the pH of a 2.0M solution of HBr is approximately 0.3.
So, the pH of a 2.0M solution of HBr is approximately 0.3.