# Chemical Forums

## Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Lizzie2686 on May 17, 2004, 06:31:03 PM

Title: Normality and Neutralization
Post by: Lizzie2686 on May 17, 2004, 06:31:03 PM
My teacher was not here today and left us with a worksheet without any explanations, and it is due tomorrow.
Does anyone know how to calculate the normalities of solutions such as 98.0g H2SO4/L solution or 126g HNO3/L...how to determine the mass of solute needed to prepare 1.00L of 1.00N NaOH and 2.00 of .250N H2SO4...how to determine a 1M solution of HCl contains ???g of HCl...a 1.00M HCl solution is ???N
I have many more of these problems, but if someone can explain to me how to come up with an answer, it would be greatly appreciated.
My last question is 25.0mL of .500M NaOH is neutralized by 15.0mL of H2SO4. The molarity of the acid is ???M. (Hint: Use NaVa=NbVb; then calculate M for the acid)

can anyone explain this to me by tonight? Thank you. :'( ???
Title: Re:Normality and Neutralization
Post by: Mitch on May 17, 2004, 08:18:56 PM
Normality is the same thins as Molarity except when you calculate normality you have to multiply the final answer by the number of free protons the acid can give off. H2SO4 can give off 2 for example.