2 Nov 2009 Recitation - (a.) 0 mL (b.) 10.0 mL (c.) 40.0 mL...

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Recitation 2 November 2009 1. Sketch a titration curve for a weak acid titrated with a strong base. Identify the following points on the curve. Group Problems a. The equivalence point b. The buffering region c. pH = pKa d. pH depends only on [HA] e. pH depends only on [A - ] f. pH depends only on the amount of excess strong base added. 2. Consider the titration of 50 – mL of 1.0 M benzoic acid with standardized 0.5 M NaOH. (a.) Identify the halfway to the equivalence point, (b.) Identify the equivalence point, and (c.) Calculate the pH at the following points during the titration: i. At the starting point in which no NaOH has been added. ii. After 25 – mL of 0.5 M NaOH has been added. iii. After 50 – mL of 0.5 M NaOH has been added. iv. After 100 – mL of 0.5 M NaOH has been added. v. After 150 – mL of 0.5 M NaOH has been added. The K a for Benzoic Acid is 6.4 x 10 -5 . 3. Consider the titration of 40.0 mL of 0.200 M HClO 4 with 0.100 M KOH. Calculate the pH of the resulting solutions after the following volumes of KOH has been added.
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Unformatted text preview: (a.) 0 mL (b.) 10.0 mL (c.) 40.0 mL (d.) 80.0 mL (e.) 100.0 mL 4. Calculate the molar solubility of each of the following compounds in moles per liter and grams per liter (Ignore any acid-base properties). a. Ag 3 PO 4 (Ksp = 1.8 x 10-18 ) b. CaCO 3 (Ksp = 8.7 x 10-9 ) 5. Calculate the solubility (in mol/L) of Fe(OH) 3 (Ksp = 4.0 x 10-38 ) in each of the following instances. a. Water (pH = 7) b. A buffered solution at pH = 5.0 c. A buffered solution at pH = 11.0 1. Calculate the pH for the titration of a 50-mL solution of 1.0 M pyridine C 5 H 5 N (K b = 1.7 x 10-9 ) with 0.25 M HCl. Individual Problems a. At the starting point with no HCl added. b. After 50 mL of HCl is added. c. After 100 mL of HCl is added. d. After 200 mL of HCl is added e. After 250 mL of HCl is added Sketch the titration curve. 2. The Ksp for silver sulfate (AgSO 4 ) is 1.2 x 10-5 . Calculate the solubility of silver sulfate in each of the following. a. Water b. 0.10 M AgNO 3 c. 0.20 M K 2 SO 4...
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This note was uploaded on 11/30/2009 for the course CHEM 1101 taught by Professor Bottomley during the Fall '08 term at Georgia Institute of Technology.

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2 Nov 2009 Recitation - (a.) 0 mL (b.) 10.0 mL (c.) 40.0 mL...

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