What is the value of pMg for 50.0 ml of a 0.0500 M Mg2 solution buffered at pH 10.00 and titrated with 0.0500 m EDTA when 50.0 mL of EDTA is added (Kf = 6.2x10)(ay4 = 0.30 )? 1. 05.77 2 02.88 3. 04.94 4. O1.39 5. 07.96
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- In order to titrate EDTA into a water sample of unknown water hardness, the EDTA of known concentration is first diluted. If 25.0 mL of a 0.0632 M EDTA solution is transferred into a 250.0 mL volumetric flask, what is the concentration of the diluted EDTA solution? 0.00632 M 0.006320 M 3.950e-4 M 0.01580 M 0.00158 M 3.95e-4 M 0.6320 M(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.Consider the titration of 25.0mL 0.020M of Co(NO3)2 with .0100M EDTA in a solution buffered to pH 10.00. Calculate pCo^2+ at the following volumes of added EDTA. a. 0.0 mL b. 20.0 mL c. 40.0 mL d. 49.0 mL e. 50.0 mL f. 50.1 mL g. 55.0 mL h. 60.0 mL
- 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.Is this for Average Molarity of EDTA Standard Solution? Then, would it be always the same with average Molarity of EDTA? How about the Ca Titer (mg Ca/mL of EDTA Solution? Show step by step solution.Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn of the solution after 30 mL of titrant have been added?
- 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.Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0 Zn(NH3)n2+: pKfn, = 2.21, 2.29, 2.36, 2.03ZnY2-: Kf = 3.0 x 1016EDTA: Ka1 = 1.02 x 10-2 , Ka2 = 2.14 x 10-3 , Ka3 = 6.92 x 10-7 , Ka4 = 5.50 x 10-11Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00 and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+ and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0
- The concentration of a solution of EDTA was determined by standardizing against a solution of Ca2+ prepared from the primary standard CaCO3. A 0.4025 g sample of CaCO3 was transferred into a 250 mL Erlenmeyer flask and the pH adjusted by adding 5 mL of a pH 10 NH3-NH4Cl buffer containing a small amount of Mg2+EDTA. After adding calmagite as a visual indicator, the solution was titrated with the EDTA requiring 42.36 mL to reach the end point. Report the molar concentration of the titrant.9. The Tl in a 9.57 g sample of rodenticide was oxidized to the trivalent state and treated with an unmeasured excess of Mg/EDTA solution. The reaction is:Tl3++ MgY2-→TlY-+ Mg2+Titration of the liberated Mg2+required 12.77 mL of 0.03560 M EDTA. Calculate the percentage of Tl2SO4(MM= 504.80 g/mol) in the sample.a. A 40.0 mL sample containing 0.0400 M Ni2+ was titrated with 0.0400 M EDTA at pH 11.0. Given pKNiY = 18.62 and α = 0.85. Calculate pNi at 0, 10, 100 and 110% of the titration.