Concentrated sulphuric acid is $98%$ w/w $H X_{2} SO X_{4}$ (molar mass $98 g mo l^{- 1}$ ) with density $1.84 g m L^{- 1}$ . What volume of it (in mL, one decimal place) is needed to prepare $500 mL$ of $0.50 M$ $H X_{2} SO X_{4}$ ?

Numerical answer type, answer in mL, tolerance 0.1.

Answer: 13.6 mL

Molarity of the concentrated acid

= 0.98 \times 1.84 \times 1000/98 = 18.4

M. Moles needed

= 0.50 \times 0.500 = 0.250

mol.

V = 0.250/18.4 = 0.01359

= 13.6

mL.