W9_titrations_salts

W9_titrations_salts - a Calculate the initial pH You may...

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Chem 125 Dr. Retsek Winter 2007 Worksheet 9: Acids and Bases and Titrations 1. A 25.00-mL sample of 0.100 M HCl is titrated with with 0.100 M NaOH. a. What is the pH before the addition of any NaOH? b. How much NaOH is required to reach the equivalence point? c. What is the pH at the equivalence point? 2. A 25.00-mL sample of 0.100 M HC 2 H 3 O 2 is titrated with 0.100 M NaOH. a. What volume of base is needed to reach the equivalence point? b. At what volume, does the pH = pK a c. Given K a for HC 2 H 3 O 2 is 1.8 x 10 -5 , calculate the pH before the addition of any NaOH d. What is the pH at the equivalence point? 3. For the titration of 25.00 mL of 0.150 M HCl with 0.250 M NaOH: a. Calculate the initial pH. b. Is the solution neutral, acidic, or basic at the equivalence point? c. How much NaOH is required to reach the equivalence point? d. Estimate the pH of the solution after the addition of 25.00 mL of NaOH. 4. For the titration of 20.00 mL of 0.150 M HF with 0.250 M NaOH.
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Unformatted text preview: a. Calculate the initial pH. You may need to consult your text for a needed constant. b. Is the solution neutral, acidic or basic at the equivalence point? c. How much NaOH is required to reach the equivalence point? d. Estimate the pH of the solution after the addition of 25.00 mL of NaOH? 5. A 60.0 mL sample of a monoprotic acid is titrated with 0.150 M NaOH. If 20.0 mL of base is required to reach the equivalence point, what is the concentration of the acid? 6. A 25.0 mL sample of a diprotic acid is titrated with 0.240 M KOH. If 60.0 mL of base is required to reach the second equivalence point, what is the concentration of the acid? 7. Predict whether each of the following aqueous solutions is acidic, basic, or neutral. Write out the reaction showing why the solution would be acidic, basic, or neutral. a. NaOCl b. KCl c. NH 4 NO 3 d. NaI e. NaNO 2 f. CH 3 NH 3 NO 3 Chem 125 Dr. Retsek Winter 2007...
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