Step 1 of 2
(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 = 0.6179 mol
there are 0.062 moles in 0.1 L = 0.62M
in HBr, there are 0.62 M and 0.62 M Br
pH = -log = -log [0.62] = .2