2/20/25, Mon An HBr solution has a concentration of 0.0150 M. What are the [H^+],[OH], pH, and pOH of this solution? A KOH solution has a concentration of 0 .0450 M What are the [OH],[H^+] pOH and oH of this

1. For the HBr solution: - The concentration of ions in an acidic solution is equal to the concentration of the acid. Therefore, . - The concentration of ions in an acidic solution is calculated using the ion product constant for water, . \([OH^-] = \frac{K_w}{[H^+]^2} = \frac{1.0 \times 10^{-14}}{(0.0150)^2} = 4.44 \times 10^{-12} \text{ M}\). - The pH of the solution is calculated using the formula . \(pH = -\log(0.0150) = 1.82\). - The pOH of the solution is calculated using the formula . \(pOH = -\log(4.44 \times 10^{-12}) = 11.35\).2. For the KOH solution: - The concentration of ions in a basic solution is equal to the concentration of the base. Therefore, . - The concentration of ions in a basic solution is calculated using the ion product constant for water, . \([H^+] = \frac{K_w}{[OH^-]^2} = \frac{1.0 \times 10^{-14}}{(0.0450)^2} = 4.41 \times 10^{-12} \text{ M}\). - The pOH of the solution is calculated using the formula . \(pOH = -\log(0.0450) = 1.35\). - The pH of the solution is calculated using the formula . .