What is the concentration of Ca²+ in solution that is prepared by mixing 50 ml 0.4 M Ca²+ with 100 ml 0.4M EDTA at pH 10?Table 12-1 Values of ays for EDTATABLE 17-4at 20°C and μ = 0.10 MFormation Constants for EDTA ComplexespH0aye1.3 x 10-231.4 x 10-18CationKMYlog KMYKMY1log KMY18.802.6 × 10-142.1 x 10-11Ag2.1 x 1077.326.3 × 10¹834.9 × 1088.693.0 × 10-9Mg²+Ca²+3.2 x 101616.505.0 × 10¹010.702.9 x 10-72.9 x 10¹616.461.8 x 10-53.8 x 10-44.2 x 10-30.0410.300.810.981.001.004910111213Lütfen birini seçin:a.7.7x10-11b.8.7x10-7C.8.7x10-11d.6.9x10-6e.9.2x10-10CationCu²+Zn²+Cd²+

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What is the concentration of Ca²+ in solution that is prepared by mixing 50 ml 0.4 M Ca²+ with 100 ml 0.4 M EDTA at pH 10? Table 12-1 Values of ays for EDTA TABLE 17-4 at 20°C and μ = 0.10 M Formation Constants for EDTA Complexes PH Cation 1.3 x 10-23 1.4 x 10-18 KMY log KMY KMY log KMY 2.6 × 10-14 2.1 x 107 7.32 6.3 × 10¹8 18.80 Ag Mg²+ 2.1 x 10-11 3.0 x 10-9 4.9 × 108 8.69 3.2 x 1016 16.50 Ca²+ 5.0 × 10¹0 10.70 2.9 x 10-7 2.9 x 10¹6 16.46 1.8 x 10-5 3.8 x 10-4 4.2 x 10-3 0.041 0.30 0.81 0.98 1.00 1.00 0 1 3 4 9 10 11 12 13 Lütfen birini seçin: a. 7.7x10-11 b. 8.7x10-7 C. 8.7x10-11 d. 6.9x10-6 e. 9.2x10-10 Cation Cu²+ Zn²+ Cd²+

What is the concentration of Ca²+ in solution that is prepared by mixing 50 ml 0.4 M Ca²+ with 100 ml 0.4 M EDTA at pH 10? Table 12-1 Values of ays for EDTA TABLE 17-4 at 20°C and μ = 0.10 M Formation Constants for EDTA Complexes PH Cation 1.3 x 10-23 1.4 x 10-18 KMY log KMY KMY log KMY 2.6 × 10-14 2.1 x 107 7.32 6.3 × 10¹8 18.80 Ag Mg²+ 2.1 x 10-11 3.0 x 10-9 4.9 × 108 8.69 3.2 x 1016 16.50 Ca²+ 5.0 × 10¹0 10.70 2.9 x 10-7 2.9 x 10¹6 16.46 1.8 x 10-5 3.8 x 10-4 4.2 x 10-3 0.041 0.30 0.81 0.98 1.00 1.00 0 1 3 4 9 10 11 12 13 Lütfen birini seçin: a. 7.7x10-11 b. 8.7x10-7 C. 8.7x10-11 d. 6.9x10-6 e. 9.2x10-10 Cation Cu²+ Zn²+ Cd²+

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter13: An Introduction To Ultraviolet-visible Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 13.11QAP: The equilibrium constant for the conjugate acid-base pair HIn+H2OH3O++In is 8.00 10-5. From the...

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0 The acid-base indicator HIn undergoes the following reaction in dilute aqueous solution:HIn color1 m H1 1 In2color2The following absorbance data were obtained for a 5.00 3 1024M solution of HIn in 0.1 M NaOH and0.1 M HCl. Measurements were made at wavelengths of 485 nm and 625 nm with 1.00-cm cells.0.1 M NaOH A485 5 0.075 A625 5 0.9040.1 M HCl A485 5 0.487 A625 5 0.181In the NaOH solution, essentially all of the indicator is present as In2; in the acidic solution, it is essentiallyall in the form of HIn.(a) Calculate molar absorptivities for In2 and HIn at 485 and 625 nm.(b) Calculate the acid dissociation constant for the indicator if a pH 5.00 buffer containing a small amountof the indicator exhibits an absorbance of 0.567 at 485 nm and 0.395 at 625 nm (1.00-cm cells).(c) What is the pH of a solution containing a small amount of the indicator that exhibits an absorbance of0.492 at 485 nm and 0.245 at 635 nm (1.00-cm cells)?(d) A 25.00-mL aliquot of a solution of purified weak…
Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. Identify the indicator and endpoint color.
A 15.00 mL urine specimen containing Ca2+ and Mg2+ was diluted to 2.000 L. A 10.00 mL sample was taken and buffered to a pH of 10 and required 27.32 mL of 0.003960 M EDTA to react with 'all' the Ca²+ and Mg2+. A second 10.00 mL sample was taken and all the Ca²+ was precipitated as Ca(C204)(s). The Ca(C2O4) (s) precipitate was then taken and dissolved in 18.00 mL of water, buffered to a pH of 10, and required 12.21 mL of 0.003960 M EDTA solution to react with all the Ca2+. Calculate the concentration of Ca²+ and Mg2+ in the original urine specimen.
A solution containing Mg2+ was buffered to pH 9.99 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)
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A solution containing Mg2+ was buffered to pH 9.75 and titrated with EDTA. Eriochrome black T, with pKa1 = 6.3 and pKa2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator's most prevalent species at this pH) Review text sections 10.4 and 10.5 for help with this!
Titration of Ca 2+ and Mg 2+ in a 50.00 ml sample required 25.50 mL Of 0.01115 M EDTA. A second 50 ml aliquot was made strongly basic with NaOH to precipitate the Mg 2+ as Mg(OH) 2(s). The supernatant liquid was titrated with 16.19 mL of the EDTA solution. Calculate the concetration in ppm of CaCO 3 in the sample О а. 100 O b.568.65 О с. 361.04 O d. 207.61
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