An EDTA solution is standardized against a solution of primary standard CaCO3 (0.5622 g dissolve in 1000 ml of solution) and titrating aliquots of it with the EDTA. If a 25.00 ml aliquot required 21.88 ml of the EDTA, what is the molar concentration of the EDTA? (CaCO3 - 100.0875 g/mo) O 0.0006418 0.005622 0.6420 0.0002933

An EDTA solution is standardized against a solution of primary standard CaCO3 (0.5622 g dissolve in 1000 ml of solution) and titrating aliquots of it with the EDTA. If a 25.00 ml aliquot required 21.88 ml of the EDTA, what is the molar concentration of the EDTA? (CaCO3 - 100.0875 g/mo) O 0.0006418 0.005622 0.6420 0.0002933

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

If you have a sample of 100 mg/L of calcium, and you have two standardized EDTA solutions of 0.005 M and 0.001 M, which one is more adequate to spend approximately 15.00 mL of the titrant if 25.00 mL of sample are added in the Erlenmeyer flask? How many mL of titrant will be used? Solution: The 0.005 M solution. 12.5 mL will be used.
1. Calcium is determined in serum by microtitration with EDTA. A 150 ml sample is treated with few drops of 2M KOH, calmagite indicator is added and the titration is performed with 0.00125M EDTA, using a microburet. A 0.205mL of EDTA is required for titration. What is the level of Ca in the serum in a. mg/dL b. mg/L
A solution containing 60 mL of a 0.025 mol / L metal ion (Mn +) buffer buffered to pH 7.0 was titrated with a 0.05 mol / L EDTA solution. Data: Conditional formation constant (Kf)=10^15. Determine: i) The concentration of the free metal when ½ of the equivalence volume is added. ii) the concentration of free metal in the equivalence volume. iii) the concentration of free metal with an excess of 2 mL of EDTA? (Data - EDTA constants: K1=0.01; K2=2.19.10^-3; K3=6.92.10^-7; K4=5.75.10^-11)
A 25.00 ml. solution of 0.03180 M Na, CO, is titrated with 0.02630 M Ba(NO, ), Calculate pBa+ following the addition of the given volumes of Ba(NO,). The K, for BaCO, is 5.0 x 10. 8.19 10.30 ml pBa+ Incorrect Ve pBa+ 4.18 %3D 2.69 35.80 mL pBa²* Incorrect
Standard oxylate solution used to standardize KMnO4 was prepared by dissolving 3.299g of Na2C2O4 in 1.000L of water containing H2SO4. add 25mL aliquot of the Na2C2O4 solution required 28.39 mL of KMnO4 for titration. A blank titration of 25mL of water containing H2SO4 required 0.03 mL of KMnO4. what is the molarity of the KMnO4 solution? 5C2O42-+2MnO4-+16H+ → 10CO2+2Mn2++8H2O
A sampie of water (200 mil) was titrated by 0.05 M HZS04. The bitrabion completed when the color changed from pink to color less at consuming 1.25 mL of the Pacid? Calculate the phenolphthalein alkalinity mg/L 625 O mg/ 6.25 mg/t 6250 mg/L 62.5
Titration of 46.00 mL of 0.04726 M Na2 C2 04 required 39.26 mL of a potassium permanganate solution. 2Mn O4 + 5H2 C2O4 + 6H+ → 2MN²+ + 10CO2 (g) + 8H20 Calculate the molar concentration of the KMNO4 solution. Concentration
3. A 100 mL sample of hard water is titrated with 22.4 mL of the EDTA solution from problem 2. The same amount of MgCl, is added as previously and the total volume of EDTA solution required is 22.44 mL. moles c) How many moles of Ca²* are in 100 mL of water?
What is the maximum concentration of iodide ions that will precipitate Agl but not Pbl2 from a solution that is 1.8 x 10-3 M each in Ag and Pb²+? For Agl, Ksp=1.5 x 10-16 a and for Pbl2. Ksp = 1.4 x 4 × 10-8. 02.8 x 10 M 83 x 10-14 M 7.8 x 10- M 12x 10- M None of these, Pbly will always precipitate before Agl. .
50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, which of the following is the amount of magnesium in the sample in ppm? (Mg:24 B/mol)
The water hardness of tap water has been determined to be 120 (= 120 mg CaCO3 per 1 L of water). After the tap water has run through the ion exchange column, titration of a 20.00 mL sample used only 0.70 mL of 0.0100 M EDTA, to reach the endpoint. Calculate the effectiveness of the ion exchange column: what is the % of the calcium, removed by the ion exchange column? Provide your answer in % and without decimal. ( Please type answer note write by hend)
A titration of 50.00 mL of 0.1100 M Fe3+ with 0.07750 M Sn2+ is carried out. The analytical reaction is 2Fe3+ + Sn2+ ⇋ 2Fe2+ + Sn4+ and Fe3+ + e− ⇋ Fe2+ E° = +0.732 V Sn4+ + 2e− ⇋ Sn2+ E° = +0.139 V What is the volume of Sn2+ is added at the equivalence point?