Question

Two solutions, one with pH = 1 andQuantity = 100 ml is another With a solution whose pH = 2 more Quantity = 200 ml is mixed is. Know the resulting pH of the mixture Please do.​

Answer 1

Explanation:

pH = -log[H+]

Assume equal volumes of two HCl volumes as 1L each.

Concentration = moles / volume

Find the moles of [H+] in the pH 3 solution.

HCl(aq) -> H+(aq) + Cl-(aq)

HCl fully dissociates because it is a strong acid.

pH = -log[H+]

[H+] = 10^-3 = 0.001 moles

Find the moles of [H+] in the pH5 solution.

pH = -log[H+]

[H+] = 10^-5 = 0.00001 moles

Find the total moles of H+ when mixing both solutions of HCl.

moles = 10^-3 + 10^-5 = 0.00101 moles of H+

Find the new volume of solution

New volume = 2 Litres

Find the concentration of H+ in the mixed solution

Concentration = moles / volume

= 0.00101 moles / 2L

= 0.00505 M

Find the pH of the mixed solution

pH = -log[H+]

= -log(0.000505)

= 3.2967…

= 3.30 (2dp)