1. A 0.9812 g sample of pure KHP required 39.76 mL of NaOH for neutralization.

a) What is the normality of the NaOH?

b) 65.76 mL of this NaOH was needed to titrate a 50.00 mL aliquot of HCl. What is the normality of the HCl?

2. A 1.0000 g sample of soda ash was dissolved in water and titrated to the methyl purple end point with 42.80 mL of 0.1209 N HCl. After boiling, 1.53 ml of 0.1543 N NaOH was used in the back titration.

a) What is the % Na₂CO₃ in the sample?

b) How many meq of NaOH, HCl, and Na2CO3 are there in this titration.

3. Derive the equation you would use to calculate the Normality of NaOH by titration of a known sample of KHP. Start with equation: eqacid = eqbase

4. Write down the structure of KHP and indicate its acid protons.

5. In the general chemistry lab the students determine the % acetic acid in vinegar by titration with NaOH. What formula would you use to do the calculations for this experiment?

6. Concentrated sulfuric acid is 18 M. What volume of conc. sulfuric would you use to make 2 L of 3 N solution.

7. Write a balanced equation that describes the following chemical facts:

a) Laboratory amounts of gaseous HCl may be made by adding conc. sulfuric to sodium or potassium chloride.

b) Benzoic acid is slightly soluble in water but very soluble in NaOH.

c) The amino acid, luecine, is slightly soluble in water but soluble in either acid or basic solutions.