4.2 4.24.3Calculate the activity coefficient and activity of each ion in a solution containing 75mg/L Na+, 25 mg/L Ca²+, 10 mg/L Mg2+, 125 mg/L CI, 50 mg/L HCO3, and 48mg/L SO².A solution is prepared by diluting 10-3 mol of propionic acid to 1 liter with distilledwater. Calculate the equilibrium concentration for each chemical species in the water.

The concept of ion activity is essential in understanding the behavior of ions in non-ideal solutions. Activity coefficients () account for deviations from ideal behavior in solutions. In this case, for simplicity, we are assuming ideal behavior, which means the activity coefficients are approximately equal to 1. However, in real-world scenarios, these coefficients can deviate from 1 based on factors such as ion concentration and ionic strength.To calculate the activity coefficient and activity of each ion in the given solution, we need to use the concentration of each ion and the ion activity coefficient. The ion activity coefficient () accounts for the non-ideality of the solution and allows us to relate the concentration of the ion to its activity. First, we need to convert the given concentration from mg/L to mol/L (or molarity). We'll use the molar masses of the ions to make this conversion:1 mg/L = 1 g/mL1 g = 1 10-6 g1 g = 1 mol = 6.022 1023 molecules (Avogadro's number)Molar mass:Na+ (sodium ion) = 22.99 g/molCa2+ (calcium ion) = 40.08 g/molMg2+ (magnesium ion) = 24.31 g/molCl- (chloride ion) = 35.45 g/molHCO3- (bicarbonate ion) = 61.02 g/molSO42- (sulfate ion) = 96.06 g/molNow, let's calculate the molar concentrations (molarity) for each ion:[Na+] = [Ca2+] = [Mg2+] = [Cl-] = [HCO3-] = [SO42-] = Now, we'll calculate the activity coefficients () for each ion. Activity coefficients are typically not provided directly but can be estimated using models like the Debye-Hückel equation or by referring to chemical databases.For the sake of this example, we'll assume ideal behavior for simplicity, which means that the activity coefficients are approximately equal to 1. In reality, these coefficients could deviate from 1 depending on the concentration and ionic strength of the solution.So, assuming ideal behavior:[Na+] = 1[Ca2+] = 1[Mg2+] = 1[Cl-] = 1[HCO3-] = 1[SO42-] = 1Now, we can calculate the activities (a) of each ion: These are the activities of each ion in the solution.Analyzing ion activity and activity coefficients is crucial in fields like chemistry and environmental science, providing insights into the behavior of ions in various solutions and their impact on chemical reactions and equilibrium. The solutions may exhibit deviations from ideal behavior, and these calculations help us understand the extent of those deviations.

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4.2 Calculate the activity coefficient and activity of each ion in a solution containing 75 mg/L Nat, 25 mg/L Ca²+, 10 mg/L Mg2+, 125 mg/L Cl, 50 mg/L HCO3, and 48 mg/L SO.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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