What is the pH pOH andOH- of a solution that has a hydronium ion concentration of 8.0 times 10 negative 6 M?

Answer 1

Important Notice: pH = negative value of the log10 of the hyronium concentration, which is very low, mostly << 1. The answer is corrected now, accordingly.

We know that pH= -log[H3O+] so the concentration of the solution is 10-pH which is equal to 10-6 (not 10+6 !!)

For the concentration of hydroxide we'll use the reasoning that pH + pOH=14 and since we know the pH we can deduce that pOH is 8 and once we know the pOH of the solution, we know that pOH=-log[OH]= 8.0

So we can use the sameprinciple as that of the pH to find the concentration of hydroxide ions!! [OH-] = 10-pH = 10-8

Answer 2

Use these three calculus formula:

• pH = -log[H3O+] = -log(8*10-6)= 5.1
• (at 25oC) always valid: pH + pOH = 14.0, so pOH = (14-5.1) = 8.9
• [OH-] = 10-pOH= invlog(-pOH) = 10-8.9 = invlog(-8.9) = 1.3*10-9 mol/L

Answer 3

Ph=-log(H30+ concentration) so,

6=-Log([H30+]) can be rewritten as, 10-6. Hydronium ion concentration = 0.000001 or 1E-6

Answer 4

- log (6.7x10-3) = pH