Place the steps in order from first to last for confirming the presence of mercury(I) ions in a sample. First Step Last Step Answer Bank Decant the liquid and add NH3 to the white precipitate. The formation of a white and black precipitate confirms the presence of mercury(I). The formation of a white solid confirms the presence of mercury(I). The formation of a yellow precipitate confirms the presence of mercury(I). Decant the liquid and add K₂ CrO to the liquid. Decant the liquid and add HNO3 to the liquid. Decant the liquid above the white precipitate and add hot water to the white precipitate. Add HCl to the sample.

Place the steps in order from first to last for confirming the presence of mercury(I) ions in a sample. First Step Last Step Answer Bank Decant the liquid and add NH3 to the white precipitate. The formation of a white and black precipitate confirms the presence of mercury(I). The formation of a white solid confirms the presence of mercury(I). The formation of a yellow precipitate confirms the presence of mercury(I). Decant the liquid and add K₂ CrO to the liquid. Decant the liquid and add HNO3 to the liquid. Decant the liquid above the white precipitate and add hot water to the white precipitate. Add HCl to the sample.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.97QE: According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as...

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Ammonium sulfate is added to an unknown mixture of ions. A precipitate forms. The solution is centrifuged, and the remaining solutions is decanted. Ammonium oxalate is then added to the solution and no precipitate forms. Sodium monohydrogen phosphate and sodium hydroxide are added to the decanted solution, and no precipitate forms. Sodium hydroxide is added to a fresh sample of the unknown. A damp piece of litmus paper over the opening of the test tube turns blue. Select the ions present. Question 4 options: Ba2+ Ca2+ Mg2+ NH41+
Ammonium sulfate is added to an unknown mixture of ions. A precipitate forms. The solution is centrifuged, and the remaining solutions is decanted. Ammonium oxalate is then added to the solution and no precipitate forms. Sodium monohydrogen phosphate and sodium hydroxide are added to the decanted solution, and no precipitate forms. Sodium hydroxide is added to a fresh sample of the unknown. A damp piece of litmus paper over the opening of the test tube remains red. Select the ions present. Question 5 options: Ba2+ Ca2+ Mg2+ NH41+
Ksp for PbCl2(s) is 1.6 x 10-³. If you mix 200.0 mL of 0.010 M Pb(NO3)2(aq) with 400.0 mL of 0.010 M NaCI(aq), then sodium nitrate will precipitate. the concentration of CI will be 0.0033 M. no precipitate will form. PbCl2(s) will precipitate.
Suppose you mistakenly used tap water instead of distilled water to dissolve your consumer product. When you did the test for chloride, you observe formation of a white precipitate after addition of silver nitrate. Can you rightly conclude that the product being tested contains chloride? Explain your reasoning.
12b.
12b.
A 1.000g sample of a mixture which contains only NaCl and KCl gave a precipitate of AgCl which weighed 2.000g. What are the percentages of Na and K in the mixture? Molar masses: AgCl = 143.3; KCl = 74.55; NaCl = 58.45; Na = 23.0; K = 39.0 * 3/3
The Kgp of Ca3 (PO4), is 1.3 x 10-26. Estimate the solubility of this salt in units of g. L-1. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Ca3 (PO4)2 is stirred into exactly one litre of a 0.550M solution of NazPO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
19. What will be the result if 100 mL of 0.06 M Ca(NO3)2 is added to 50 mL of 0.06 M K₂C2O4? Assume the reaction takes place at 25°C and Ksp of CaC₂O4(s) is 1.7 x 10⁹. a. No precipitate will form b. A precipitate will form and an excess of Ca2+ ions will remain in solution A precipitate will form and an excess of C₂O42- ions will remain in solution A precipitate will form and both Ca²+ and C₂O4²- ions are present in excess c. d.
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