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show that the equilibrium constant fc 2 en defined in the earlier problems 1-3 e numerical values at 25° C that hav nine the concentration of Ca2+(aq) ane n solid CaCO3 and water that is expose -ic carbon dioxide, 0.000405 atm. pproximation with the values found fc

show that the equilibrium constant fc 2 en defined in the earlier problems 1-3 e numerical values at 25° C that hav nine the concentration of Ca2+(aq) ane n solid CaCO3 and water that is expose -ic carbon dioxide, 0.000405 atm. pproximation with the values found fc

Chemistry & Chemical Reactivity
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
Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability
Section: Chapter Questions
Problem 41PS
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24. When the acidity provided by the dissolved carbon dioxide and the basicity provided by the solid CaCO3 are both considered, the single reaction that best represents what happens when solid CaCO3 dissolves in water in contact with atmospheric carbon dioxide at a partial pressure Pis the following: CaCO3(s) + CO2 (g) + H2O = Ca2+(aq) + 2HCO3 (aq) a. Using the approach of adding reactions, show that the equilibrium constant for the above reaction is given by: K' = KspkHKai/Ka2 where the equilibrium constants have been defined in the earlier problems 1-3; calculate a numerical value for K' from the numerical values at 25° C that have been given. b. Use the value calculated for K' to determine the concentration of Ca2+(ag) and HCO3 (ag) in water that is in equilibrium with solid CaCO3 and water that is exposed to the nominal partial pressure of atmospheric carbon dioxide, 0.000405 atm. c. Compare the solubility calculated by this approximation with the values found for the water samples in Table 1. Table 1. Results for benchmark water samples (Brooklyn, Long Island, Bottled Spring Water). The values are mean ± standard deviation for 3-4 years of data. Poland Spring Analyte Brooklyn Long Island Water Ca2+ (mg/L) 33.0±20 38.0±10 120±80 pH 8.5±0.4 7.9+0.6 7.2±0.2
Transcribed Image Text:24. When the acidity provided by the dissolved carbon dioxide and the basicity provided by the solid CaCO3 are both considered, the single reaction that best represents what happens when solid CaCO3 dissolves in water in contact with atmospheric carbon dioxide at a partial pressure Pis the following: CaCO3(s) + CO2 (g) + H2O = Ca2+(aq) + 2HCO3 (aq) a. Using the approach of adding reactions, show that the equilibrium constant for the above reaction is given by: K' = KspkHKai/Ka2 where the equilibrium constants have been defined in the earlier problems 1-3; calculate a numerical value for K' from the numerical values at 25° C that have been given. b. Use the value calculated for K' to determine the concentration of Ca2+(ag) and HCO3 (ag) in water that is in equilibrium with solid CaCO3 and water that is exposed to the nominal partial pressure of atmospheric carbon dioxide, 0.000405 atm. c. Compare the solubility calculated by this approximation with the values found for the water samples in Table 1. Table 1. Results for benchmark water samples (Brooklyn, Long Island, Bottled Spring Water). The values are mean ± standard deviation for 3-4 years of data. Poland Spring Analyte Brooklyn Long Island Water Ca2+ (mg/L) 33.0±20 38.0±10 120±80 pH 8.5±0.4 7.9+0.6 7.2±0.2
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