What is the molarity of a solution formed by mixing 10.0 g of #H_2SO_4# with enough water to make 0.100 L of solution?

1 Answer
Aug 27, 2016

Answer:

#(10.0*g)/(98.08*g*mol^-1)xx1/(0.100*L)=??*mol*L^-1#.

Approx. #1*mol*L^-1#.

Explanation:

#"Molarity"="Moles of solute"/"Volume of solution"#, the which operation gives an answer in #mol*L^-1#.

This question would have more realistic if it proposed that #8*g# of #SO_3# were dissolved in #80*mL# of water to give a specific volume of solution (likely #80*mL#). As an acidic oxide, sulfur trioxide dissolves in water to give stoichiometric #H_2SO_4#.