Which of the following solutions will have the lowest pH, assuming complete dissociation?Remember: pH = -log10[H3O+(aq)], pOH = -log10[OH-(aq)] and pH + pOH = 14.00Group of answer choices1 M solution of HClO32M solution of HBr2 M solution of KOH1.8 M solution of Sr(OH)2

The pH of a solution is determined by the concentration of hydronium ions [H3O+(aq)] present in the solution. The lower the pH, the higher the concentration of hydronium ions, and thus the more acidic the solution is.

1. A 1 M solution of HClO3: HClO3 is a strong acid, which means it completely dissociates in water to form H3O+ and ClO3-. Therefore, the concentration of H3O+ ions in this solution is 1 M. The pH of this solution is -log10(1) = 0.

2. A 2 M solution of HBr: HBr is also a strong acid, which means it completely dissociates in water to form H3O+ and Br-. Therefore, the concentration of H3O+ ions in this solution is 2 M. The pH of this solution is -log10(2) = -0.3.

3. A 2 M solution of KOH: KOH is a strong base, which means it completely dissociates in water to form K+ and OH-. The concentration of OH- ions in this solution is 2 M. The pOH of this solution is -log10(2) = -0.3. Since pH + pOH = 14, the pH of this solution is 14 - pOH = 14 - (-0.3) = 14.3.

4. A 1.8 M solution of Sr(OH)2: Sr(OH)2 is a strong base, which means it completely dissociates in water to form Sr2+ and 2 OH-. Therefore, the concentration of OH- ions in this solution is 2 * 1.8 = 3.6 M. The pOH of this solution is -log10(3.6) = -0.56. Since pH + pOH = 14, the pH of this solution is 14 - pOH = 14 - (-0.56) = 14.56.

Therefore, the solution with the lowest pH is the 2 M solution of HBr.