Which of the following solutions will have the highest pH, assuming complete dissociation? Remember: pH = -log10[H3O+(aq)], pOH = -log10[OH-(aq)] and pH + pOH = 14.00 Group of answer choices 1 M solution of RbOH 1 M solution of H2SO4 1.7 M solution of HClO3 0.6 M solution of Ba(OH)2

The pH of a solution is determined by the concentration of hydronium ions (H3O+) in the solution. The higher the concentration of these ions, the lower the pH of the solution. Conversely, the lower the concentration of hydronium ions, the higher the pH of the solution.

1. RbOH is a strong base, which means it will dissociate completely in solution to form Rb+ and OH- ions. The concentration of OH- ions will be 1 M. Using the formula pOH = -log10[OH-(aq)], we find that the pOH of this solution is 0. Therefore, the pH of the solution is 14 - pOH = 14 - 0 = 14.

2. H2SO4 is a strong acid, which means it will dissociate completely in solution to form 2H+ and SO4^2- ions. The concentration of H+ ions will be 2 M. Using the formula pH = -log10[H3O+(aq)], we find that the pH of this solution is -log10(2) = -0.3.

3. HClO3 is also a strong acid, which means it will dissociate completely in solution to form H+ and ClO3- ions. The concentration of H+ ions will be 1.7 M. Using the formula pH = -log10[H3O+(aq)], we find that the pH of this solution is -log10(1.7) = -0.23.

4. Ba(OH)2 is a strong base, which means it will dissociate completely in solution to form Ba2+ and 2OH- ions. The concentration of OH- ions will be 2*0.6 = 1.2 M. Using the formula pOH = -log10[OH-(aq)], we find that the pOH of this solution is -log10(1.2) = -0.08. Therefore, the pH of the solution is 14 - pOH = 14 - (-0.08) = 14.08.

Therefore, the 0.6 M solution of Ba(OH)2 will have the highest pH.