Calculate the pH of the following solutions.
(a) 5.00 g of HBr in 100 mL of aqueous solution
(b) 1.50 g of NaOH in 50 mL of aqueous solution
(a) 5.00 g of HBr in 100 mL of aqueous solution.
Mass of HBr= 5.00 g.
Volume =100 mL.
5 g HBr = ?
Before going to know the concentration we can calculate the number of moles of solute present in the given solution .
=mass /molar mass .
=5.0 g/80.91 g/mol.
= 0.06179 mol.
Concentration of HBr = number of moles solute present in the 1L solution.
Concentration of HBr=0.06179 mol/0.1L
=0.6179 mol / L(M).
Hence [H3O+]=0.6179 mol L -2
there are 0.062moles in 0.1L = 0.62M
in HBr, there are 0.62 M H+ and 0.62 M Br
pH = -log[H+] = -log [0.62] = .2
(b) 1.50 g of NaOH in...