calculate the pH of 0.10 M HCI solution?
first find the concentration of the [OH-] ions in the solution. You do this by using the formula:
[OH]=1x10^-14/[H]
the [h] equals 0.1 bc the M of HCL = the M of H and M of Cl
then you would find the POH. You do this by using the formula: pOH=-log[OH-]
Once you have found the POH you can find pH because PH=14-[pOH]
I don't readily see anything wrong with the answer by anonymous; however, it's a lot of unnecessary work. You don't need to go through the OH or pOH.
pH = -log(H^+)
pH = -log(0.1)
solve.
pH = 1
To calculate the pH of an HCl (hydrochloric acid) solution with a concentration of 0.10 M (molar), we can use the following steps:
Step 1: Write the balanced chemical equation for the ionization of HCl in water:
HCl(aq) → H+(aq) + Cl-(aq)
Step 2: Since HCl is a strong acid, it dissociates completely in water, meaning that the concentration of H+ ions and Cl- ions will be the same.
Step 3: Calculate the concentration of H+ ions in the solution. For a 0.10 M HCl solution, the concentration of H+ ions will also be 0.10 M.
Step 4: Calculate the pH using the formula: pH = -log[H+]
In this case, pH = -log(0.10) = 1.
Therefore, the pH of a 0.10 M HCl solution is 1.