A 30.00-mL solution containing 0.1553 M Na2C2O4 was titrated with 0.1250 M Ca(NO3)2 to precipitate calcium oxalate: Ca+ C,0, CaC,O4(s) Ksp 1.3 x 108 What is the pCa at the equivalence point? O A. 4.56 O B. 2.52 O C. 4.50 OD. 1.75 O E. 3.94

A 30.00-mL solution containing 0.1553 M Na2C2O4 was titrated with 0.1250 M Ca(NO3)2 to precipitate calcium oxalate: Ca+ C,0, CaC,O4(s) Ksp 1.3 x 108 What is the pCa at the equivalence point? O A. 4.56 O B. 2.52 O C. 4.50 OD. 1.75 O E. 3.94

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 50E: A solution contains 1.0 105 M Ag+ and 2.0 106 M CN. Will AgCN(s) precipitate? (Ksp for AgCN(s) is...

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Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

A 30.00-mL solution containing 0.1553 M Na2C204 was titrated with 0.1250 M Ca(NO3)2 to
precipitate calcium oxalate:
Ca + C,0,
CaC,O4(s) Ksp 1.3 x 108
What is the pCa at the equivalence point?
O A 4.56
O B. 2.52
OC. 4.50
OD. 1.75
O E. 3.94

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In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?
A 65.0-mL sample of 0.010 M Pb(NO3)2 was added to a beaker containing 40.0 mL of 0.035 M KCl. Will a precipitate form?
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A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3.
Copper(l) chloride, CuCl, is the starting material for the fungicide copper oxychloride. At 25C, a saturated solution of CuCl is prepared by dissolving 10.1 mg of CuCl in 0.250 L of water. What is the Ksp, for copper(I) chloride?
A mixture contains 1.0 103 M Cu2+ and 1.0 103 M Mn2+ and is saturated with 0.10 M H2S. Determine a pH where CuS precipitates but MnS does not precipitate. Ksp for CuS = 8.5 1045 and Ksp for MnS = 2.3 1013.
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Cadmium(ll) chloride is added to a solution of potassium hydroxide with a pH of 9.62. (KspCd(OH)2=2.51014) (a) At what concentration of Cd2+ does a precipitate first start to form? (b) Enough cadmium(II) chloride is added to make [ Ca2+ ]=0.0013 M. What is the pH of the resulting solution? (c) What percentage of the original hydroxide ion is left in solution?
What mass of Ca(NO3)2 must be added to 1.0 L of a 1.0-M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 1011 and Ka for HF = 7.2 104. Assume no volume change on addition of Ca(NO3)2(s).
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