Final answer:
The solubility of mn(oh)2 in a buffer solution at pH=7.0 is 5.494 x 10^-6 g/L.
Step-by-step explanation:
The solubility of mn(oh)2 in grams per liter when buffered at ph=7.0 can be calculated using the Henderson-Hasselbalch equation. The concentration of hydroxide ion, [OH-], in the buffered solution can be determined by subtracting the concentration of hydrogen ion, [H+], from the pOH value, which is the negative logarithm of the hydroxide ion concentration.
In this case, the pH of the solution is 7.0, which means that the concentration of hydrogen ion is 10^-7 M. The pOH value is 14 - pH = 14 - 7 = 7. The concentration of hydroxide ion can be calculated as 10^-pOH = 10^-7 = 1 x 10^-7 M.
Therefore, the solubility of mn(oh)2 in grams per liter is the product of the hydroxide ion concentration and the molar mass of mn(oh)2: 1 x 10^-7 M * (54.94 g/mol) = 5.494 x 10^-6 g/L.