xamining the system of equations you wrote in part A, what changes t you expect if the source of chloride ions was hydrochloric acid O instead of sodium chloride? Would this make the silver oxalate more ple or less soluble? {Note that the answer to this question should use atlier's-principle-type arguments about shifting equilibria.}

xamining the system of equations you wrote in part A, what changes t you expect if the source of chloride ions was hydrochloric acid O instead of sodium chloride? Would this make the silver oxalate more ple or less soluble? {Note that the answer to this question should use atlier's-principle-type arguments about shifting equilibria.}

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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3. The sulfate ion concentration in natural water can be determined by measuring the turbidity that results when an excess of BaCl, is added to a measured quantity of the sample. A turbiditimeter, the instrument used for this analysis, was calibrated with a series of standard Na,SO, solutions. The following data were obtained for the calibration: Assume that a linear relationship exists C, mg So,2- Turbiditimeter between the instrument reading and 4. reading, R concentration. 0.00 0.06 Derive an equation of a line that tells us the relationship of C and а. 5.00 1.48 10.00 2.28 R. b. What is the concentration of 15.00 3.98 sulfate when the turbiditimeter 20.00 4.61 reading was 3.67?
4 Using what you know about equilibrium, explain why the molar solubility for the pure Ca(OH)2 solution differs from the spiked solution. Do your results match your expectations? Why or why not?
2. What are the characteristics of an ideal precipitate? Using the Von Weirman ratio, explain the different methods that you can perform to make the precipitate more ideal?
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Aluminum trifluoride (AIF3) is sparingly soluble with a Ksp value of 1.1 x 103. Calculate the molar solubility ("s") of this precipitate in pure water. 04.1 x 105 06.4 x 10-3 O0.080 O0.14
2. Consider a solution that is 0.100M in silver and 0.050 M in copper(I). Is it possible to selectively precipitate 99.9% of the silver by complexing with chloride without also precipitating the copper(I)?
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[4ab] a. Calculate the mass of calcium and magnesium in the original sample. b. Calculate for the mass of the mixed oxalate precipitate that was formed.
In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?
A solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration value
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