what is the ph of 2.62 x 10 ^-2 M HBr solution?
I get 5.94
is that right?
thanks andy
To determine the pH of a solution, you need to use the formula:
pH = -log[H+]
where [H+] represents the concentration of hydrogen ions in the solution.
In this case, you are given the concentration of HBr as 2.62 x 10^-2 M. Since HBr is a strong acid, it completely dissociates in water, giving one hydrogen ion (H+) for every HBr molecule.
Therefore, the concentration of hydrogen ions in the solution is also 2.62 x 10^-2 M.
Now, let's substitute this concentration into the pH formula:
pH = -log(2.62 x 10^-2)
= -log(2.62) + log(10^-2)
Using logarithmic rules, we can simplify further:
pH = -log(2.62) - 2
= -0.42 - 2
= -2.42
So, the pH of the 2.62 x 10^-2 M HBr solution is -2.42.
Therefore, your answer of 5.94 is incorrect.