postlab7 - -11 . 5. Calculate the solubility of AgCl in...

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Chemistry 116 General Chemistry Lab I Section: 17 Date: 4/2/08 Score____________ Exp #7: Determination of the Solubility-Product Constant for a Sparingly Soluble Salt Name: James Anders TA: Ed Torres Room: 206 Post-Lab Questions 1. For the equilibrium equation: Ag 2 CO 3(s)  2 Ag + (aq) + CO 3 2- (aq) , write the K c and the K sp . (2 points) 2. Why are you required to construct a calibration curve for this experiment? (2 points) 3. If the K sp for PbI 2 is 3.1 x 10 -7 , will precipitation of PbI 2 occur when 10mL of 1.0 x 10 -5 M Pb(NO 3 ) 2 is mixed with 10mL of 1.0 x 10 -2 M KI? (2 points) 4. Calculate the solubility of Mg(OH) 2 in water. K sp = 1.2 x 10
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Unformatted text preview: -11 . 5. Calculate the solubility of AgCl in 0.20 M AgNO 3 solution. K sp of AgCl is 1 x 10-10 . 6. The solubility of PbSO 4 in water is 0.038 g/L. Calculate the solubility product constant of PbSO 4 . 7. What is the solubility of Pb(IO 3 ) 2 (a) in mol/L, and (b) in g/L ? K sp of Pb(IO 3 ) 2 = 2.5 x 10-13 . 8. Determine the solubility of AgCl in 0.10 M BaCl 2 . K sp of AgCl is 1.0 x 10-10 . 9. What mass of BaSO 4 will dissolve in 450 mL of aqueous solution. K sp for BaSO 4 is 1 x 10-10 . 10. How many mol CuI (K sp = 5 x 10-12 ) will dissolve in 1.0 L of 0.10 M NaI solution?...
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This note was uploaded on 04/08/2008 for the course CHEM 116 taught by Professor Torres during the Spring '08 term at Ole Miss.

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postlab7 - -11 . 5. Calculate the solubility of AgCl in...

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