KOH is a strong base in aqueous solution; therefore, the (KOH) = (OH%-).
For pH = 11.53, use pH + pOH = pKw = 14 to solve for pOH, then from
pOH = -log (OH^-), solve for OH^-. That will give you the molarity of the KOH you want for that pH.
Then M = moles/L. Substitute L and solve for moles.
Then moles = grams/molar mass, solve for grams.
What mass of KOH is necessary to prepare 799.9 mL of a solution having a pH = 11.53?
4 answers
112. 57
105. 84
4. 5×10^-13