1.  What is the equivalent weight of the following substances?  In each case explain why.  The best explanation is to write a balanced chemical reaction with H⁺ if the substance is a base and OH^-if the substance is an acid.
a) H₂SO₄
b) Phthalic acid
c) NaOH
d) Ca(OH)₂

e) Na₂O
f) SO₃
g) NaHSO₄
h) KHP  (if your answer is 71 you're wrong)
i) Acetic Acid  (C₂H₃O₂H)

2. 20.0 mL of 0.10N NaOH = __________g H₂SO₄

3. How could you decide on the correct indicator to use in an acid base titration.

a) Calculate a theoretical titration curve and choose an appropriate indicate based on the equivalence point pH.

b) Measure the pH vs volume of titrant and from the experimental titration curve and choose an appropriate indicate based on the equivalence point pH.

c) Take a standard sample and try various indicators and choose the one that gives the correct percent analyte.

d) all of these ways would be appropriate.

4. ________ mL of 0.15 N NaOH = 0.341 g H₂SO₄

5._________ mL of 0.12 N NaOH = 8.26 meq H₂SO₄

6. 4.7 x 10^-3 eq of NaOH = __________ eq H₂SO₄

7. 36.78 mL of 0.154 N NaOH were used to titrate a 1.3452 sample containing citric acid (EW= 63 g/eq). What % citric acid is in the sample?  Explain why the equivalent weight of citric acid is 63.  Draw its structure and circle the acid protons.

8. 34.5 mL of 0.0987 N NaOH is used to titrate 48.5 mL of HCl. What is the N of the HCl?

9. Write down the net ionic equation for the reaction of KHP with NaOH.

10. 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?