Which of the following statements is(are) true? Correct the false statements. a. When a base is dissolved in water, the lowest possible pH of the solution is \(7.0 .\) b. When an acid is dissolved in water, the lowest possible \(\mathrm{pH}\) is 0 c. A strong acid solution will have a lower \(p H\) than a weak acid solution. d. \(A 0.0010-M B a(O H)_{2}\) solution has a pOH that is twice the pOH value of a 0.0010-M KOH solution.

This statement is false. When a base is dissolved in water, the pH is greater than 7.0 (not equal to 7), and we can have pH values up to 14. We could correct the statement with: "When a base is dissolved in water, the pH of the solution is greater than 7.0."

This statement is true. When an acid is dissolved in water, the pH can range from 0 to 7.0 (not inclusive). The strongest acids have pH values closest to 0.

This statement is true. A strong acid is one that completely ionizes in a solution. The higher the concentration of hydrogen ions (\(H^{+}\)) in a solution, the lower the pH value. Weak acids partially ionize, resulting in a higher pH value compared to strong acids.

This statement is false. To understand why, let's first understand the concept of pOH. pOH is the measure of hydroxide ions (\(OH^{-}\)) in a solution, and can be calculated using \(pOH = -\log_{10}[OH^-]\). In a 0.0010-M Ba(OH)\(_2\) solution, there are 2 moles of \(OH^{-}\) for every mole of \(Ba(OH)_{2}\). Therefore, the concentration of \(OH^{-}\) ions in the solution will be 2 times the given concentration: 0.0020 M. pOH of 0.0010-M Ba(OH)\(_2\) solution: \(pOH = -\log(0.0020)\) = 2.70. For a 0.0010-M KOH solution, we have a concentration of \(OH^{-}\) ions equal to the given concentration: 0.0010 M. pOH of the 0.0010-M KOH solution: \(pOH = -\log(0.0010)\) = 3.00. Thus, the pOH of the \(Ba(OH)_{2}\) solution (2.70) isn't twice the pOH of the KOH solution (3.00). We can correct the statement with: "A 0.0010-M \(Ba(OH)_{2}\) solution has a lower pOH than a 0.0010-M KOH solution."