11. A solution of 0.0500M Ca²* and 0.00500M Mg* was titrated against EDTA at pH = 10 (K'r for CaY2 =1.75 x 1010 and K't for MgY2 1.72 x 10). Which statement is NOT TRUE? a. The reaction of formation of the calcium complex ion occurs with lower tendency. b. In the titration curve of Mg*, a smaller change of pM occurs around the equivalence point. c. Eriochrome black T indicator could be used for both titrations. d. The pCa is larger than pMg after the excess addition of the EDTA.

11. A solution of 0.0500M Ca²* and 0.00500M Mg* was titrated against EDTA at pH = 10 (K'r for CaY2 =1.75 x 1010 and K't for MgY2 1.72 x 10). Which statement is NOT TRUE? a. The reaction of formation of the calcium complex ion occurs with lower tendency. b. In the titration curve of Mg*, a smaller change of pM occurs around the equivalence point. c. Eriochrome black T indicator could be used for both titrations. d. The pCa is larger than pMg after the excess addition of the EDTA.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.20QAP

See similar textbooks

Similar questions

Cd²+ forms a stable complex with EDTA. Consider the titration of 30.00 ml of 0.0525 M Cd with 0.125 M EDTA at pH 9, using Eriochrome black T as the indicator. Constants you may need: log K, (Cd-EDTA) 16.5. a, @ph 9= 0.052 The pCd at equivalence point (12.6 mL) is [a]
3. A 50.00 mL solution containing Ni2+ and Fe2+ was treated EDTA to bind all the metal ions. After back-titration, the amount of EDTA used is 2.500 mmol. In another 50.00 mL solution was added pyrophosphate to mask the Fe2+ ions, and the solution required 25.00 mL of 0.04500 M EDTA. Calculate the ppm Fe (55.85 g/mol) in the solution.
25.00 mL 0.01000 M Ni2+ is titrated with 0.01000 M EDTA in a solution buffered topH 5.0. Given that the formation constant for the Ni-EDTA (NiY2–) chelate is4.2 x 1018 and the 4 value at pH 5.0 is 3.54 x 10–7. Calculate the pNi at the equivalence point.
b. EDTA cannot be used as a primary standard always. When can EDTA be used as a primarystandard ? Give reason why EDTA is used in complexometric titrations.
Calculate the PCa vs. EDTA titration curve for 50.0 mL of 0.0060 M Ca2+ being titrated with 0.0150 M EDTA in a solution buffered to a constant pH of 10.00. After the addition of 0.00 mL After the addition of 26.0 mL
What is the equivalence volume when 0.0500 M EDTA is titrated with 100.0 mL of 0.0500 M Mn+ buffered to a pH of 9.00?
Consider the titration of 25.0 mL of 0.020 0 M MnSO4 with 0.010 0 M EDTA in a solution buffered to pH 6.00. Calculate pMn21 at the following volumes of added EDTA and sketch the titration curve: 0, 20.0, 40.0, 49.0, 49.9, 50.0, 50.1, 55.0, and 60.0 mL.
The formation constant (Kf) for calcium reacting with EDTA is 6.2 x108. A calcium-EDTA titration was done at a pH = 10.00, where the fraction of species of Y4- is approximately 0.39, what would be the value for the conditional formation constant (Kf') for the reaction? Group of answer choices 6.2 x 108 2.4 x 108 4.5 x 1011 1.0 x 1010
25.00 mL 0.01000 M Ni2+ is titrated with 0.01000 M EDTA in a solution buffered to pH 5.0. Given that the formation constant for the Ni-EDTA (NiY2–) chelate is 4.2 x 1018 and the 4 value at pH 5.0 is 3.54 x 10–7 Calculate the approximate transition range of this indicator when used in the titration of Ni2+ with EDTA at pH 5.0.
A cyanide solution with a volume of 13.72 mL was treated with 25.00 mL of Ni2+ solution(which contained an excess of Ni(II) ions) to convert the cyanide to the complex ion tetracyanonickelate(II): 4CN- + Ni2+ → 6 Ni(CN)2- The excess Ni 2+ was then titrated with 10.15 mL of 0.01307 M EDTA. One mole of this reagent reacts with one mole of Ni(II) as follows: Ni(CN)42- does not react with EDTA. If 39.35 mL of EDTA was required to react with 30.10 mL of the original Ni 2+ solution, calculate the molarity of CN- in the 13.72 mL cyanide sample.
25.00 mL 0.01000 M Ni2+ is titrated with 0.01000 M EDTA in a solution buffered to pH 5.0. Given that the formation constant for the Ni-EDTA (NiY2–) chelate is 4.2 x 1018 and the 4 value at pH 5.0 is 3.54 x 10–7. What is EDTA?
Calculate the pSr value for 10 mL of EDTA in the titration of 50 mL of 0.02 M Sr2 + in an environment buffered at pH 11 with a titre of 0.02 M EDTA. A. 1.89B. 3.78C. 7.56D. 12.11