Indicate whether it is present or not a.) Concentrated HCl is added to the original solution. A solid precipitate forms.Ag*| Select)Pb2+ I Select ]Hgz2 I Select]b.) Hot water is added to the precipitate in (a). Some precipitate remains.Ag* I Select ]Pb2+ Select ]2+ I Select]c.) The supernatant from (b) is removed to a new test tube and then treated with K2CrO4. No precipitate forms.Ag* TSelect ]Pb2+ I Select ]Hg,2 I Select]d.) NH3 is added to the original test tube in (b) containing the precipitate. Some white and black precipitate remains.Ag* I Select ]Pb2+ I Select ]2+ [ Select ]e.) The supernatant from the test tube in (d) is removed and treated with HNO3. No precipitate forms.Ag* TSelect ]Pb2+ Select ]Hg22+ I Select]>>>>

Answered: Image /qna-images/answer/6d31e4ed-e249-4de9-91eb-bb1269678b2c.jpg

a.) Concentrated HCl is added to the original solution. A solid precipitate forms. Ag*| Select) Pb2+ I Select ] Hgz2 I Select] b.) Hot water is added to the precipitate in (a). Some precipitate remains. Ag* I Select ] Pb2+ Select ] 2+ I Select] c.) The supernatant from (b) is removed to a new test tube and then treated with K2CrO4. No precipitate fo Ag* TSelect ] Pb2+ I Select ] Hg,2 I Select] d.) NH3 is added to the original test tube in (b) containing the precipitate. Some white and black precipitate Ag* I Select ] Pb2+ I Select ] HP,2+ I Select] > >

a.) Concentrated HCl is added to the original solution. A solid precipitate forms. Ag| Select) Pb2+ I Select ] Hgz2 I Select] b.) Hot water is added to the precipitate in (a). Some precipitate remains. Ag I Select ] Pb2+ Select ] 2+ I Select] c.) The supernatant from (b) is removed to a new test tube and then treated with K2CrO4. No precipitate fo Ag* TSelect ] Pb2+ I Select ] Hg,2 I Select] d.) NH3 is added to the original test tube in (b) containing the precipitate. Some white and black precipitate Ag* I Select ] Pb2+ I Select ] HP,2+ I Select] > >

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.26QAP

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(c) 1.0cm^3 0.25 moldm^-3 potassium chromate(VI), K2CrO4, is added as an indicator. At the end-point, all the silver chloride has been precipitated in the 52.5cm^3 solution. A slight excess of silver ions causes a red-brown precipitate of silver chromate(VI) to form. 2Ag + (aq) + CrO4 2- (aq) - - > Ag2CrO4 (s) (i) The solubility product of silver chloride is: Ksp = 2.0 ×10^-10 mol^2 dm^-6 Use this value to explain why [Ag+] = 1.41 × 10^-5 moldm^-3 at the end point.
An aqueous solution contains Cu+, Tl+, Hg+, and Ti+ with each ion at a concentration of 0.15M. Chloride ion is slowly added to the solution. Using the Ksp information below, determine the order in which the ions would precipitate. AgCl = 1.8 x 10−10TiCl = 1.8 x 10−4PbCl2 = 1.7 x 10−5CuCl = 6.73 x 10−7TlCl = 3.7 x 10−4HgCl2 = 17.91 x 10−18
The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M silver nitrate is combined with 25mL of 0.1M sodium chromate, what is the mass of the silver chromate precipitate in grams?
The solubility of Ag2CrO4 (Ksp = 1.2 x 10^-12) is several times greater than that of AgCl (Ksp = 1.82 x 10^-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 as an indicator for 100 mL of sample solution, what is the concentration (M) of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?
The solubility of lead (II) chloride is 1.00 g in 100 mL. 165.6 g of nitrate of Lead (II) in 900 mL and 100 mL of 1M HCl added. Will lead chloride precipitate?
mixing 17.5 mL of 4.700 M aluminum chloride with 24.0 mL of 2.00M silver (I) nitrate solution results in a precipitate. the resulting mixture contains a total free chloride ion concentration of
An aqueous solution contains Ag+, Pb2+, Cu+, and Tl+ with each ion at a concentration of 0.15M. The chloride ion is slowly added to the solution. Using the Ksp information below, determine the order in which the ions would precipitate. AgCl = 1.8 x 10−10TiCl = 1.8 x 10−4PbCl2 = 1.7 x 10−5CuCl = 6.73 x 10−7TlCl = 3.7 x 10−4HgCl2 = 17.91 x 10−18
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Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq) and 0.0260 M Ag+(aq). What will be the concentration of Ca2+(aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, ?sp, can be found in the chempendix. [Ca2+]= M What percentage of the Ca2+(aq) can be precipitated from the Ag+(aq) by selective precipitation? percentage:
A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final precipitate (assumed to be Fe,03) contains 20.0 mg of Al,O3 by mistake, what percentage of Fe does the analyst find?
25 mL of a saturated solution of K2Cr2O7 was cooled from 90oC to 50oC, how many moles solid will precipitate from solution?
Based in the principles of Precipitimetry. Precipitates form when the ions concentrations exceed the solubility product of a solution. If a solution of Silver Nitrate mixed titrated against Sodium Chloride at a ratio of 1:1, are precipitates formed? Yes or No? Rationalize using Ksp and ion product principles.