›Determine the molar solubility (S) of Ag₂CO3 in a buffered solution with a pH of 5.619 using the systematic treatment of equilibrium. Ksp (Ag2CO3) = 8.46 × 10-¹²; Kai (H₂CO3) = 4.45 × 10−7; K₁2(H₂CO3) = 4.69 × 10-¹¹. S = 1.46 ×10-4 Incorrect M

›Determine the molar solubility (S) of Ag₂CO3 in a buffered solution with a pH of 5.619 using the systematic treatment of equilibrium. Ksp (Ag2CO3) = 8.46 × 10-¹²; Kai (H₂CO3) = 4.45 × 10−7; K₁2(H₂CO3) = 4.69 × 10-¹¹. S = 1.46 ×10-4 Incorrect M

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section: Chapter Questions

Problem 42PS

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The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
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