Concentrated sulfuric acid (18.4-molar H2SO4) 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 H2SO4.
b) Determine the mass percent of H2SO4 in the original concentrated solution.
c) Calculate the volume of 5.20-molar H2SO4 that can be completely reacted with 10.5 grams of sodium bicarbonate, NaHCO3, in the reaction: 2NaHCO3 + H2SO4 --> 2H20 + NasSO4 + 2 CO2
d) What is the molality of the 5.20-molar H2SO4?
a) (5.20M)(1.00L)= moles H2SO4
= 5.20 moles H2SO4
(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.