What are the concentrations of hydroxide and hydronium ions in a solution with a ph of 4.6?

1.3 × 10–4 m h3o+ and 7.7 × 10–11 m oh–

2.5 × 10–5 m h3o+ and 4.0 × 10–10 m oh–

7.9 × 10–6 m h3o+ and 1.3 × 10–9 m oh–

8.7 × 10–7 m h3o+ and 1.1 × 10–8 m oh–

2.5 × 10–5 M H3O+ and 4.0 × 10–10 M OH–

Explanation:

pH = - log[H3O+]

Therefore;

pH = - log[H3O+] = 4.6

Hence;

[H3O+]  = 10^-4.6

             = 2.51 ×10^-5 M

             = 2.5 ×10^-5 M

Additionally;

pH + pOH = 14

Thus; pOH = 14 -pH

                  = 14 -4.6

                  = 9.4

but; pOH = - log [OH-]

Therefore;

[OH-] = 10^-9.4

        = 3.98 × 10^-10 M

        =  4 × 10^-10 M

i think its 100.

hope this !