Calculate pCd²+ at each of the given points in the titration of 50.00 mL of 0.0070 M Cd²+ with 0.0070 M EDTA in the presence of the auxiliary complexing agent NH3. The solution is buffered at a pH of 11.00 and the NH3 concentration is fixed at 0.100 M. The fraction of EDTA in the form Y4 as a function of pH can be found in this table. The formation constant for the Cd²+ -EDTA complex can be found in this table. The cumulative formation constants for the Cd(NH₂)2+ complexes can be found in this table. 0 mL pCd²+ = 45.00 mL pCd²+ = 55.00 mL pCd²+ = 00 14.00 mL 50.00 mL pCd²+ pCd²+ =

Calculate pCd²+ at each of the given points in the titration of 50.00 mL of 0.0070 M Cd²+ with 0.0070 M EDTA in the presence of the auxiliary complexing agent NH3. The solution is buffered at a pH of 11.00 and the NH3 concentration is fixed at 0.100 M. The fraction of EDTA in the form Y4 as a function of pH can be found in this table. The formation constant for the Cd²+ -EDTA complex can be found in this table. The cumulative formation constants for the Cd(NH₂)2+ complexes can be found in this table. 0 mL pCd²+ = 45.00 mL pCd²+ = 55.00 mL pCd²+ = 00 14.00 mL 50.00 mL pCd²+ pCd²+ =

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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2. Construct a titration curve for the following complexometric titration by calculating the calcium ion concentration in terms of pCa during the titration of 50.00 mL of 0.0500 M CaCl with 0.1000 M EDTA in a solution buffered to constant pH = 10, after the addition of the following volumes of EDTA reagent: (a) In the pre-equivalence region at 10.00 mL, (b) At the equivalence point (include what the equivalence volume calculation), and (c) After the equivalence point at 30.00 mL. Given that Kf for CaY2-is 1010.65 and ay4- at pH 10.0=0.30.
3. Calculate the pZn of solutions prepared by adding 15.0, 25.0, and 35.0 mL of 0.100M EDTA to 50.0 mL of 0.00500M Zn²+ in 0.100M NH3 and 0.175M NH4Cl buffered to a pH of 9.0.
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Calculate PCa of the solution that results when 50.0 mL of 0.0050 M Ca2+ is titrated with 25.00 mL of 0.0100 M EDTA in a solution buffered to a conastant pH of 10.00.
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Write a balanced net ionic equation to show why the solubility of AgCN(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Be sure to specify states such as (aq) or (s). K= + + +
One of the buffers that can be used for running an agarose gel is 1x TBE (tris borate EDTA) buffer. The recipe for 1x TBE is: • 0.13 M tris • 45 mM boric acid • 2.5 mM EDTA How will you make 1 L of this buffer from 1M stock solutions of tris, boric acid, and EDTA? Put your answers in the blanks. To make 1 Lof this buffer, I would need: L of 1 M Tris ml of 1 M boric acid ml of 1 M EDTA Then, these will be topped up with distilled water in a volumetric flask up to the 1L mark.
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