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 00450 M What are the [OH^-],[H^+] pOH, and pH of this solution? Calculate the [H+],[OH-] pH, and pOH of a solution.

To calculate the , , pH, and pOH of a solution, we need to know the concentration of the solution and whether it is an acid or a base.For the HBr solution with a concentration of 0.0150 M:Since HBr is a strong acid, it will dissociate completely in water to produce ions. Therefore, the concentration of ions will be equal to the concentration of the HBr solution, which is 0.0150 M.The concentration of ions can be calculated using the ion product constant for water (Kw), which is at 25°C. The formula is: Substituting the values, we get: The pH of the solution can be calculated using the formula: Substituting the value of , we get: The pOH of the solution can be calculated using the formula: Substituting the value of , we get: For the KOH solution with a concentration of 0.0450 M:Since KOH is a strong base, it will dissociate completely in water to produce ions. Therefore, the concentration of ions will be equal to the concentration of the KOH solution, which is 0.0450 M.The concentration of ions can be calculated using the ion product constant for water (Kw), which is at 25°C. The formula is: Substituting the values, we get: The pOH of the solution can be calculated using the formula: Substituting the value of , we get: The pH of the solution can be calculated using the formula: Substituting the value of pOH, we get: In summary, for the HBr solution with a concentration of 0.0150 M:- - - pH = 1.82- pOH = 11.18For the KOH solution with a concentration of 0.0450 M:- - - pOH = 1.35- pH = 12.65