Concentrated sulfuric acid (18.4-molar H_{2}SO_{4}) has a density of 1.84 grams per milliliter. After dillution with water to 5.20-molar, the substance has a density of 1.38 grams per millilter and can be used as an electrolyte in lead storage batteries for automobiles.

a) Calculate the volume of concentrated acid required to prepare 1.00 L of 5.20-molar H_{2}SO_{4}.

b) Determine the mass percent of H_{2}SO_{4} in the original concentrated solution.

c) Calculate the volume of 5.20-molar H_{2}SO_{4} that can be completely reacted with 10.5 grams of sodium bicarbonate, NaHCO_{3}, in the reaction: 2NaHCO_{3} + H_{2}SO_{4} --> 2H_{2}0 + Na_{s}SO_{4 } + 2 CO_{2}

d) What is the molality of the 5.20-molar H_{2}SO_{4}?

Work

a) (5.20M)(1.00L)= moles H_{2}SO_{4}

= 5.20 moles H_{2}SO_{4}

(5.20 moles)/(18.4M) = **0.28L** ?

-I'm sorry, this is a confusing chapter for me. Can someone help me out with b,c, and d? And was my A correct? Sorry. I really need help.