What is the formula of EDTA-complex with La3+?
In complex formation
potentiometric titration with EDTA solution, the working electrode
is La and the reference electrode is saturated calomel.
This is the table of titration 25 ml ionic solution
La3+ with EDTA solution 3,95x10-3 M.
Determine the concentration of La3+.
Vol EDTA (mL) 0,00 0,02 0,04 0,06 0,08 0,10 131,5 129,0 124,0 113,5 103,5 101,0 100,0 99.0 0.14 0.16 0,18 0,20 98,0 98,0 97,0 96,0 95.5 95.0 0,30 0,35 0.40
1. The K for the complex ion formation between Pb2+ and EDTA is 1.4x1018 at 25°C. Pb2+ (aq) + EDTA (aq) → (Pb(EDTA)]2+ (aq) Calculate at equilibrium the concentration of Pb2+ in a solution that was made to initially contain 0.0010 M Pb2and 0.0020 M EDTA. [Pb (EDTA)32+ T24
Zinc(II) ions forms a strong complex in the presence of EDTA. Calculate the equilibrium concentrations of Zn2+ and Zn(EDTA)2- after 0.600 mol of Zn(NO3)2 has been dissolved in 1.00 L of 2.60 M EDTA solution. The Kf of Zn(EDTA)2- is 3.8 x 1016.
2 poin QUESTION 5 What is the value of conditional formation constant, Kr. for the EDTA-complex with Cu2+ at pH 10.07 Kr(Cuy) - 6.03x1018 Cu2+ + EDTA CuY2 (Use Table 11-1 in the textbook as a reference.) 1.2.01 x 1019 2.1.81 x 1018 3.3.21 x 1015 O4 7.66 x 10-20 5.6.03 x 1018 QUESTION 6 2 poir Consider titration of 24.00 ml of 0.0880 M Cuat solution with 0.110 M EDTA at pH 10.0. Find the concentration of free Cu2+...
Zinc (II) ions form a strong complex in the presence of EDTA. Calculate the equilibrium concentration of Zn2+ and Zn(EDTA)2- after 0.600 mol of Zn(NO3)2has been dissolved in 1.00L of 2.60 M EDTA solution. The Kf of Zn(EDTA)2- is 3.8*1016. Is there a way you can do it without using the quadratic equation?
Calculate the conditional formation constant of the EDTA complex of Al3+ in a solution buffered to pH = 3.0 Answer to 3 significant digits.
2+ EDTA is often used to preserve blood samples because it can complex with Ca which is necessary for clotting. The typical concentration of Ca2 in blood is 1.1 x 10° M and a typical concentration of 4 x 10 M Na2H2EDTA is added. The pH of blood is 7.2 and for this pH, the EDTA alpha fractions are 2 x 1010, 3 x 10, 0.12, 0.88 and 8.1 x 10-4 for α0, α1, α2, α3 and α4, respectively. The...
In a water Hardness complexometric micro-titration, EDTA was used as a standard. The formula is : Ca ^2+ Y^4- - CaY^2 where (Y is EDTA) Suppose the EDTA used was not as dry as it should have been a. Would [EDTA] in the EDTA solution be higher or lower than the actual value? b. Would the [Ca] determined in the unknown be higher or lower than the actual value?
i am insure what are the correct answers for this one
EDTA Titration 1. EDTA (cthylenediaminetetraacetic acid) is the most widely used metal chelator in analytical chemistry, which forms strong 1:1 complexes with most metal ions. Water hardness can be determined by titrating Ca, Mg and other metal ions with EDTA. During the titration, ammonium-ammonia chloride buffer is often used. Which of the following descriptions about the function of ammonium-ammonia chloride is/are correct? (a) To react with EDTA To form...
In a water Hardness complexometric micro-titration, EDTA was used as a standard. The formula is : Ca ^2+ Y^4- - CaY^2 where (Y is EDTA) Suppose the EDTA used was not as dry as it should have been a. Would [EDTA] in the EDTA solution be higher or lower than the actual value? b. Would the [Ca] determined in the unknown be higher or lower than the actual value? Answers: a) Due to presence of water, the actual mass of...