Read the problem and identify the values given.
Step 2 :
Substitute the value in the corresponding formula to calculate the unknown values.
pH = -log[H3O+]
pOH = - log[OH-]
[H+] = 10-pH
[OH-] = 10-pOH
Step 3 :
Using the value of pH identify the type of the given solution.
A 0.1M solution of acetic acid has a hydrogen ion concentration of 1.3 $\times$ 10-3M. Find the pH of the solution.
Step 1 :The hydrogen ion concentration is 1.3 $\times$ 10-3M.
Step 2 :pH = -log[1.3 $\times$ 10-3]
pH = -(2.89)
pH = 2.89
Step 3 :The pH of 2.89 in this example is less than 7. This value indicates that the solution is definitely acidic.
Answer :The value of pH of the given solution is 2.89
Calculate the concentration of the given soultion whose pH value is given as 3.60.
Step 1 :The pH value is given as pH = 3.60
Step 2 :Substitute the value of pH in the respective formula to find the concentration of hydrogen ions.
[H+] = 10-pH
[H+] = 10-3.60
[H+] = 0.00025 = 2.5 $\times$ 10-4M
Step 3 :The concentration of [H+] ion is 2.5 $\times$ 10-4M
Answer :The concentration value of [H+] ion 2.5 $\times$ 10-4M