Solution A has pH of 4.6 and solution B has a pH of 8.0

1- What is the (H3O+) in solution A?

2- What is the (OH-) in solution B ?

To determine the (H3O+) concentration in solution A, we can use the pH value provided. The pH is a logarithmic scale that quantifies the concentration of (H3O+) ions in a solution. The formula to convert pH to (H3O+) concentration is:

[H3O+] = 10^(-pH)

1- To find the (H3O+) concentration in solution A, we can substitute the given pH value of 4.6 into the formula:

[H3O+] = 10^(-4.6)

Calculating this expression, we find that the (H3O+) concentration in solution A is approximately 2.51 x 10^(-5) M.

2- To find the (OH-) concentration in solution B, we can use the fact that in water, the product of the (H3O+) and (OH-) concentrations is constant at 1.0 x 10^(-14) M^2. This relationship is known as the ion product of water.

[H3O+] x [OH-] = 1.0 x 10^(-14)

We already know the (H3O+) concentration of solution B, which is not explicitly given. However, we can calculate it using the formula:

[H3O+] = 10^(-pH)

Substituting the given pH value of 8.0 into the formula, we find that the (H3O+) concentration in solution B is approximately 1.0 x 10^(-8) M.

Now, we can substitute this (H3O+) concentration into the equation for the ion product of water to find the (OH-) concentration.

(1.0 x 10^(-8)) x [OH-] = 1.0 x 10^(-14)

Rearranging the equation, we find that the (OH-) concentration in solution B is approximately 1.0 x 10^(-6) M.

pH = -log (H^+)

4.6 = -log(H^+)
-4.6 = log(H^+)
Take antilog both side. To do that on your calculator, key in 4.6, change to - 4.6, then hit the 10x key. That will give you 2.51 x 10^-5.
For #2, convert pH 8.0 to pOH by remembering that pH + pOH = 14. Then
pOH = -log(OH^-).