What is the pH of a solution that is comprised of 0.0843 M HCl and 0.0287 M HClO4?
Both acids are monoprotic acids and both are strong acids.
So 0.0843 M HCl will give 0.0843 M H+
and
0.0287 M HClO4 will give 0.0287 M H+
so the total H+ is
(0.0843+0.0287)M = 0.113 M
pH=-log([H+]/M)
so pH=-log(0.113)
To determine the pH of a solution, we need to know the concentration of either H+ ions or OH- ions. In this case, both HCl and HClO4 are strong acids that completely dissociate in water to form H+ ions.
To find the pH of the solution, we can calculate the total concentration of H+ ions by adding the concentrations of HCl and HClO4. In this case, we have:
Concentration of HCl = 0.0843 M
Concentration of HClO4 = 0.0287 M
Adding these values together gives us the total concentration of H+ ions:
Total concentration of H+ ions = 0.0843 M + 0.0287 M = 0.113 M
Now, to find the pH, we can use the equation:
pH = -log[H+]
Taking the negative logarithm (base 10) of the concentration of H+ ions, we get:
pH = -log(0.113)
Using a calculator, we find that:
pH ≈ 0.95
Therefore, the pH of the solution is approximately 0.95.