H+ ions increase in concentration at lower pH values.
Calculate how many more H+ ions there are in a solution
at a pH = 2 than in a solution at a pH = 6. Find the
concentration of H+ ions at a pH = 2 and at a pH = 6 in
Table B. Then divide the concentration of H+ ions at a
pH = 2 by the of H+ ions at a pH = 6. Record your
answer in Table C.
What is the concentration of H+ ions at a pH = 2?
mol/L
What is the concentration of H+ ions at a pH = 6?
mol/L
How many more Htions are there in a solution at a
pH = 2 than in a solution at a pH = 6?

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.