How much free lead (II) ion is present in a 95.4 mL of a solution that contains 136.8 microgram of Pb2* per deciliter of solution upon addition of 95.4 mL 0.0100 M EDTA? Give just the numerical portion of the answer: X 10 22 M Pb2+ Kr for [Pb(EDTA)2 is 2.0 X 1018 As a side note: For adults, blood lead concentrations > 89 ug/dL require treatment for lead poisoning even if the patient is asymptomatic.

How much free lead (II) ion is present in a 95.4 mL of a solution that contains 136.8 microgram of Pb2* per deciliter of solution upon addition of 95.4 mL 0.0100 M EDTA? Give just the numerical portion of the answer: X 10 22 M Pb2+ Kr for [Pb(EDTA)2 is 2.0 X 1018 As a side note: For adults, blood lead concentrations > 89 ug/dL require treatment for lead poisoning even if the patient is asymptomatic.

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 129CP: A few drops of each of the indicators shown in the accompanying table were placed in separate...

See similar textbooks

Similar questions

A 47.00 ml aliquot from a 0.490 L solution that contains 0.410 g of MnSO, (MW = 151.00 g/mol) required 40.7 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO, ( MW = 100.09 g/mol) will react with 1.61 ml. of the EDTA solution? mass: mg
A 47.90 mL aliquot from a 0.500 L solution that contains 0.480 g of MnSO4 (MW = 151.00 g/mol) required 40.9 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 (MW = 100.09 g/mol) will react with 1.68 mL of the EDTA solution? mass: mg
A 25.00 mL solution was prepared by dissolving CaCO3 solid. It required 24.25 mL of a standard 0.02 M EDTA (ethylenediaminetetraacetic acid) solution to titrate the Ca2+ ions to the end point. (moles= 4.85 * 10^-4) (I need help with D) a. How many moles of EDTA are contained in the 24.25 mL used for tritration. 4.85* 10^-4 moles b. How many moles of CaCO3 were used? 4.85* 10^-4 moles c. What is the concentration (molarity) of Ca2+ in the 25.00 mL of solution? .0194 M d. How many grams of CaCO3 were used in the preparation of the 25.00 ml of .0194 M CaCO3 solution.
The Zn in a 0.6803-g sample of foot powder was titrated with 27.3 mL of 0.04246 M EDTA. Calculate the percentage of Zn (65.39g/mol) in this sample.
A 0.1504-g sample of impure Na₂CO₃ (106.00g/mol) was analyzed via Volhard method. After adding 50.0 mL of 0.07106 M AgNO₃, the sample was back-titrated with 0.06485 M KSCN requiring 11.69 mL to reach the end point. What is the purity of the Na₂CO₃ sample? CHOICES: 98.5% 95.7% 89.0% None of these
Titration of 30.00 mL of 0.02502 M Na2C2O4 required 34.75 mL of a potassiumpermanganate solution.2MnO -+ 5H C O + 6H+  2Mn2- + 10CO + 8H O4 2 2 4 2(g) 2Calculate the molar concentration of the KMnO4 solution
A cobalt (ii) solution wants to be examined by titration with 0.0415 M EDTA solution at ph 6.0. What will be the concentrations of cobalt(ii) ions in a titration of 30.0 ml and 0.0193 M cobalt (II) solution if a)12ml b)equivalent volume ,c) 16 ml EDTA are used in these titrations (K f =2.82*10^ 16 )
Titration of 0.2121 g of primary standard Na,C,0, (133.999 g/mol) required 21.66 mL of KIMnO, (158.034 g/mol) to reach the end point. Calculate the molar concentration of KMNO,? 2 MnO, +5 C20,2 + 16 H+ 2 Mn2+ 10 CO2 +8 H20 1. 000146 2. O0.0292 3. 00.00731 4. 00.1462
Titration of 0.2342 g of pure Na,C,0, (134.0 g/mol) required 33.45 ml of KMNO4 solution according to the chemical reaction: 2MNO, + 5C,0, +16 H* 2MN2* + 10CO, +8H,0 The Molarity of KMNO, solution would be: a. 0.01609 M b. 0.04020 M c. 0.02090 M d. 0.20140 M e. 0.12450 M Please fill in the space with one of the following characters (a or b or c or d or e)
0.0322 M EDTA solution is used as the titrant in the titration of a 50.00 mL solution that is 0.0129 M in Cu2+. The solution is held at pH = 10.00 by a buffer that is 0.050 in ammonia (NH3). At what volume (in mL) of EDTA added will the equivalence point be reached?
Plot the titration curve for titration of 50mL of 0.0150M Fe2+ solution buffered to pH's 7.0 with 0.03M EDTA. A-) OmL, B-) 10mL, C-) 25 mL, D-) Calculate the pFe after 26 mL of titrant additions. (Kr.Y= 2.1x10^14, a4=4.8x10^-4)
What volume of 0.370 M KMnO4 would be required to titrate 0.41 g of K2[Cu(C2O4)2]⋅2H2O = ?mL