What is the pH of a 0.01 M solution of the strong acid HNO3 in water?
I bet it is 2
pH=-log(H concentraion)=-log (.02)
To determine the pH of a solution, we need to know the concentration of hydrogen ions (H+) in that solution. Strong acids, such as HNO3, completely dissociate in water, meaning they release all of their hydrogen ions. Therefore, the concentration of H+ ions in a 0.01 M solution of HNO3 is also 0.01 M.
The pH scale is a logarithmic scale that ranges from 0 to 14. pH values less than 7 indicate an acidic solution, while pH values greater than 7 indicate a basic (or alkaline) solution. To calculate the pH, we use the formula:
pH = -log[H+]
where [H+] represents the concentration of H+ ions in moles per liter (M).
In this case, [H+] = 0.01 M.
So, we can substitute this value into the formula:
pH = -log(0.01)
Calculating the logarithm of 0.01 gives us -2.
Therefore, the pH of a 0.01 M solution of HNO3 is 2.