Calculate pBa 2* after 14.00 ml of 0.100 M EDTA is added to 89.00 mL of 0.100 M Ba2* in the presence of 0.100 M nitrilotriacetate (auxiliary complexing agent). The solutionis buffered at pH 10. a = 1.48 x 10 -4."t. = 0.300 at pH 10. K; = 7.59 x 107 forBay 2-.4.211Question 10Calculate pBa 2* after 93.00 mL of 0.100 M EDTA is added to 19.00 mL of 0.100 M Ba2* . The solution is buffered at pH 10. For the buffered pH of 10, “ = 0.30. K + = 7.59x 107 for Bay 2-.4.564

Mole is the amount of the substance that contains the same number of particles or atoms or…

Calculate pBa 2* after 14.00 ml of 0.100 M EDTA is added to 89.00 mL of 0.100 M Ba 2* in the presence of 0.100 M nitrilotriacetate (auxiliary complexing agent). The solution is buffered at pH 10. " - 1.48 x 10 -4."t. = 0.300 at pH 10. K,- 7.59 x 107 for Bay 2-. 4.211 Question 10 Calculate pBa 2* after 93.00 mL of 0.100 M EDTA is added to 19.00 mL of 0.100 M Ba 2* . The solution is buffered at pH 10. For the buffered pH of 10, "a- - 0.30. K , = 7.59 x 107 for Bay 2-. 4.564

Calculate pBa 2* after 14.00 ml of 0.100 M EDTA is added to 89.00 mL of 0.100 M Ba 2* in the presence of 0.100 M nitrilotriacetate (auxiliary complexing agent). The solution is buffered at pH 10. " - 1.48 x 10 -4."t. = 0.300 at pH 10. K,- 7.59 x 107 for Bay 2-. 4.211 Question 10 Calculate pBa 2* after 93.00 mL of 0.100 M EDTA is added to 19.00 mL of 0.100 M Ba 2* . The solution is buffered at pH 10. For the buffered pH of 10, "a- - 0.30. K , = 7.59 x 107 for Bay 2-. 4.564

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter9: Complexometric And Precipitation Titrations

Section: Chapter Questions

Problem 13P

See similar textbooks

Similar questions

The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1
The equilibrium constant for the conjugate acid-base pair HIn+H2OH3O++In is 8.00 10-5. From the additional information in the following table, (a) calculate the absorbance at 430 nmand 600 nm for the following indicator concentrations: 3.00 10-4M,2.00 10-4M, 1.00 10-4M, 0.500 10-4 M, and 0.250 10-4M. (b) plot absorbance as a function of indicator concentration.
A sample is analyzed for chloride by the Volhard method. Calculate the %KCl from the following data: Wt of sample = 0.5000g; Vol of AgNO3 added = 35.00ml; M of AgNO3 = 0.1157; Vol of SCN- used for back titration = 14.71ml; M of SCN- = 0.08598; Atomic wts: Ag = 107.87, N = 14.00, Cl = 35.5, O = 16.00
50 mL of a solution of 0.0200 M Zn2+ will be titrated with 0.0100 M EDTA in 0.0100 M NH3 at pH 6.0. Ethylenediaminetetraacetic acid (EDTA) can be considered as a tetraprotic acid (H4Y). The stepwise acid dissociation constants are: K1 = 1.02 x 10-2, K2= 2.14 x 10-3, K3 = 6.92 x 10-7 and K4 = 5.50 x 10-11. The alplia value of the un-deprotonated species in a solution buffered to a certain pH is given by the following equation: a0 = [H+]4/([H+]4 + K1[H+]3 + K1K2[H+]2 + K1 K2K3[H+] + K1 K2K3K4) Calculate the alpha value of the fully deprotonated species (Y4- ) in a solution buffered to a pH of 6.0.
To a 50.00-mL aqueous solution containing Pb2+ is added a total amount of 5.000 mmol EDTA. The pH is made alkaline, and the excess EDTA is back-titrated with 0.0100 M Mg2+, requiring 15.2 mL. Calculate the molar concentration of Pb in the sample. A.0.100 M B. 0.0970 M C. 0.0486 M D. 2.94 x 10-3 M
A foot powder sample containing Zn was dissolved on 50.00 mL water and was titrated to the end point color with 22.57 mL of 0.01639 M EDTA at pH=4. (α= 3.61x109, KKzny2 = 3.2 x 1016). The pZn in the sample is:
A solid containing tris was dissolved in water and brought to a total volume of 50.00 ml. A 10.00 ml aliquot of the solution was titrated with 0.09978 M HCl to a bromcresol green endpoint. The aliquot consumed 38.93 ml of titrant. Calculate the weight of tris in the original sample.
(a) Sketch a titration curve for a 50.0 mL of 0.01M Sr2+ solution, buffered at pH 11 when 0.0,10.0, 24.0, 25.0, 26.0, 30.0, and 40.0 mL of 0.02 M EDTA are added. Given the KSrY2- is 4.3X108 and α4 is 0.85.
For the following lab Complexometeric Determination of Magnesium... Mg^2+ + Y^4- -> MgY^2- Unknown MgO was titrated with roughly 0.03M of Na2EDTA and pH10 buffer solution (~5mL to MgO) using Nh4CL(s) and NH4OH, 8 drops of Calmigate Indictor and titrated to a blue endpoint with the EDTA (disappearance of the last tinge of red) 1. a. Why is it necessary to buffer the solution to a pH between 10 and 12? b. What is the structure and full name for EDTA? c. Although EDTA has, in its fully protonated form, 4 hydrogen atoms that can be lost, it is listed as a hexadentate ligand. Explain why this is the case
Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 by 0.040 0 M Cu+ to give Ce3+ and Cu2+, using Pt and Ag | AgCl electrodes (Eref = 0.197 V) to find the end point. Ce4+ + e- ↔ Ce3+ E⁰ = 1.70 Cu2+ + e- ↔ Cu+ E⁰ = 0.161 Calculate E at the following volumes of Cu+: 12.5, 25.0, and 30.0 mL.
Consider the titration of 25.00 mL of 0.03555 M Co2+ by 0.02784 M EDTA at pH 10.00. Kf is 1045. Calculate the pCo2+ when 35.00 mL of EDTA are added.
For the following lab Complexometeric Determination of Magnesium... Mg^2+ + Y^4- -> MgY^2- Unknown MgO was titrated with roughly 0.03M of Na2EDTA and pH10 buffer solution (~5mL to MgO) using Nh4CL(s) and NH4OH, 8 drops of Calmigate Indictor and titrated to a blue endpoint with the EDTA (disappearance of the last tinge of red) 1. Titration of Zn^2+ and EDTA is carried out in the same manner as Mg^2+ - EDTA titration (Zn can actually be used to standardize EDTA solution). In this case the ammonia from the pH 10 buffer serves an additional purpose. What is it? 2. If the unknown consisted of Co+2, Fe+2, Sr+2, and Ni+2, which cation would completely complex with the EDTA first? Second? Third? Fourth? (State your reasons!) Also what are the minimum pH values required for satisfactory titrations of the above metal cations? (How know?) 3. Briefly (but specifically) discuss how the Calmagite indicator works.