CW15-Ksp - solid ions and the equilibrium constant is...

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CHM 2046/Myers Worksheet 15 February 12, 2010 1. Buffer Capacity. A buffer can be used to set the pH. Once the pH is “set,” a buffer will hold the pH reasonably constant against changes such as the addition of small amounts of acid or base. 2. Acid-Base Indicators. Indicators are highly colored, very low concentration weak acids: HIn + H 2 O H 3 O + + In - The pKa of an indicator is its crossover pH . See the separate table for a list of common pH Indicators and their pKa’s. Use 2 or more indicators to find the pH of a solution. In a titration pick an indicator that changes at the pH of the equivalence point: For H 3 O + + OH - 2 H 2 O, pH (at EP) = ______, so use _________ For HAc + OH - Ac - + H 2 O, pH (at EP) = ______, so use _________ For NH 4 + + OH - NH 3 + H 2 O, pH (at EP) = ______, so use _________ For H 3 O + + NH 3 NH 4 + + H 2 O, pH (at EP) = ______, so use _________
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3. Solubility Equilibria. The “standard form” way to write a solubility chemical equation is in the form
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Unformatted text preview: solid ions and the equilibrium constant is called a solubility product , Ksp. 4. Solubility Problems. A. Solubility in Water. (1)What are [Ag + ] and [Cl-] for AgCl saturated in water? AgCl(s) Ag + (aq) + Cl-(aq), Ksp 1.8 x 10-10 [Ag + ] = ____________ [Cl-] = _____________ (2)What are [Ag+] and [CrO 4-2 ] for Ag 2 CrO 4 saturated in water? Ag 2 CrO 4 (s) 2 Ag + (aq) + CrO 4-2 (aq), Ksp 1.1 x 10-12 [Ag + ] = ____________ [CrO 4-2 ] = _____________ B. Common Ion Effect. (3)What are [Ag + ] and [Cl-] for AgCl saturated in 0.10 M HCl? AgCl(s) Ag + (aq) + Cl-(aq), Ksp 1.8 x 10-10 [Ag + ] = ____________ [Cl-] = _____________ C. Working Backwards (4)Saturated Ca(OH) 2 is 0.025 M. What what is the value of Ksp for Ca(OH) 2 ? Ksp = _________________...
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This note was uploaded on 09/19/2011 for the course CHM 2051 taught by Professor Staff during the Spring '08 term at University of Florida.

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CW15-Ksp - solid ions and the equilibrium constant is...

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