Assume that there is a solution of 1L and convert into grams to find the molarity of solution LiOH.
Density = 1.091 g/mL
(1L)(1000mL/1.0L) (1.091g/mL) = 1091 g solution.
It will contain 1091 g solution (7.53 g LiOH/100 g solution) = 82.15 g of LiOH
# of moles of LiOH will be 82.15 g/23.95 g/mol = 3.43 moles
We assumed that we took 1L of solution, so molarity is = 3.43 mol/1L = 3.43 M
LiOH is a strong base as it fully dissociates in water, producing 3.43 moles of OH-
Conc. of OH- ions= 3.43 M
Calculate pOH of the basic solution
pOH= -log[OH-]= -log(3.43)= -0.535
pH+pOH= 14
pH= 14+.535 = 14.535
