If solution A has a pH that is four pH units greater than that of solution B, how much greater is the H3O+ concentration in solution B than in solution A?

If solution A has a pH that is four pH units greater than that of solution B, the H₃O⁺ concentration in solution B is 10⁴ times greater than that of solution A.

The pH of a solution is given by:

Solution A has a pH that is four pH units greater than that of solution B, so:

or      

The H₃O⁺ concentration of solution B is related to that of solution A as follows:

Therefore, the H₃O⁺ concentration in solution B is 10⁴ times greater than that of solution A.

Learn more here:

I hope it helps you!

10⁴

Explanation:

There is usually a 10-time fold change in H₃O+ ions from one pH level to the other. The lower the pH level the higher the H₃O+ ions. Therefore for  solution A that has a pH that is four pH units greater than that of solution B, then solution B will have;

10⁴ more H₃O+ ions than solution A

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.