50.00 mL of a solution containing both Ni2* and Pb²+ ions requires 46.32 ml of a 0.02041 M EDTA solution for titration of both metals. A second 50.00 mL aliquot is treated with KCN to mask the nickel and then titrated with 30.28 mL of the same EDTA solution. Calculate the molarities of the Ni2+ and Pb2+ ions. acid anc

50.00 mL of a solution containing both Ni2* and Pb²+ ions requires 46.32 ml of a 0.02041 M EDTA solution for titration of both metals. A second 50.00 mL aliquot is treated with KCN to mask the nickel and then titrated with 30.28 mL of the same EDTA solution. Calculate the molarities of the Ni2+ and Pb2+ ions. acid anc

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 101QRT

See similar textbooks

Similar questions

A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?
Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?
What must the ratio of H2PO4 to HPO42 be to have a buffer with a pH value of 7.00?
A few drops of each of the indicators shown in the accompanying table were placed in separate portions of a 1.0-M solution of a weak acid, HX. The results are shown in the last column of the table. What is the approximate pH of the solution containing HX? Calculate the approximate value of Ka for HX. Indicator Color of Hln Color of ln pKa of Hln Color of 1.0 M HX Bromphenol blue Yellow Blue 4.0 Blue Bromcresol purple Yellow Purple 6.0 Yellow Bromcresol green Yellow Blue 4.8 Green Alizarin Yellow Red 6.5 Yellow
Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
Chloride in a brine solution is determined by the Volhard method. A 10.00 mL aliquot of the solution is treated with 15.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KCNS solution, requiring 2.38 mL to reach the endpoint. Calculate the concentration of chloride in g NaCl/liter.
Chloride in a brine solution is determined using Volhard method. A 10.00 mL aliquot of the solution is treated with 25.00 mL standard 0.1182 M AgNO3 solution. The excess silver is titrated with standard 0.1010 M KSCN solution, requiring 12.38 mL to reach the red Fe(SCN)2+ end point. Identify the (a) indicator (b) end point color (c) molarity of the Cl- in sample.
A student wanted to determine the amount of NaOCI in a commercial bleaching solution. He diluted 2 g of bleach in a 100 ml volumetric flask. A 50 ml sample of the diluted bleach was mixed with excess acidified potassium iodide KI and a few drops of an indicator. The resulting solution was titrated with Na-S.O, solution. The titration required 17 mL of 0.05M Na,S,O, solution. The series of reactions that take place during this experiment: 21+OCI+ 2H1₂ + Cl + H₂O 1₂+28,0,³ →21+S,0,² a) Calculate the number of moles of OCI- in 50 mL diluted bleach and in 100 mL.
Chloride in a brine solution is determined by precipitation titration. A 10.00 mL aliquot of the solution is treated with 25.00 mL standard 0.1182 M AgNO3 The excess silver is titrated with standard 0.1010 M KSCN solution, requiring 12.38 mL to reach the red Fe(SCN)2+ end point. Identify the molarity of the chloride ion in the brine solution.
The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN for titration to the FeSCN2+ end point. Calculate the percentage of phosphate in the detergent.
0.28g 0f MBr is dissolved in distilled water and made up to 250mL mark in a volumetric flask. 25 mL of this solution is titrated against 0.019 M silver nitrate solution using eosin as indicator. The end point was obtained at 12.4 mL of AgNO3 solution . Calculate the molar mass of the metal bromide.
A 10.00 mL sample containing 8.00 g/L of a mixture of KCI and NaCl was titrated with 0.10 M standard solution of AgNO3; where 5.6 mL was needed to reach the end-point. Calculate the mass of sample (in grams). 1. O0.0033 2. O0.0800 3. O0.0083 4. O0.0337