The substance to be analyzed is white, highly soluble in water salt. A barium chloride or silver nitrate (in presence of nitric acid) doesn't precipitation. Reaction with zinc uranyl acetate leads to formation crystals, which have tetrahedral geometry. Addition of antipyrin in aci changes color to red. What kind of substance is this? NaNO3

The substance to be analyzed is white, highly soluble in water salt. A barium chloride or silver nitrate (in presence of nitric acid) doesn't precipitation. Reaction with zinc uranyl acetate leads to formation crystals, which have tetrahedral geometry. Addition of antipyrin in aci changes color to red. What kind of substance is this? NaNO3

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter27: Relative Stabilities Of Complex Ions And Precipitates Prepared From Solutions Of Copper(ii)

Section: Chapter Questions

Problem 1ASA

See similar textbooks

Similar questions

You are assigned an unknown solution that contains Group III cations. To -1 mL of this solution was added 6 M NH3 the solution was agitated to mix well, and a reddish-brown precipitate with a gelatinous solid clinging to the inner walls of the test tube was observed. The solution was centrifuged and the supernatant was tested for completeness of precipitation by adding an additional drop of 6 M NH3. No cloudiness was observed as the drop of reagent diffused through the solution. The supernatant was then carefully decanted into a clean test tube, labeled (1st solution), and saved for further testing later. The precipitate remaining in the test tube was washed with a small amount of water, centrifuged, and the wash decanted and discarded. To the precipitate was added about 10 drops of 6 M NAOH plus ~1 mL H20 and the test tube was vigorously agitated. The resulting suspension was centrifuged and the supernatant liquid was transferred to another clean test tube and clearly labeled (2nd…
In gravimetric analysis, volatile solvents are used _______. to rinse the precipitate and remove adsorbed surface impurities because they can be obtained in a purer form than aqueous solvents because they are easily removed from the precipitate by ignition A) 1 only B) 3 only C) 1 and 3 D) 1 and 2 E) 2 only
To determine the percent purity of a sample containing iron(II) ammonium sulfate; Suggest , 2 different methods for iron(II) ion. Explain in detail what errors may occur in the methods. (volhard method, gravimetric analysis, kjeldahl, etc.) Percentage content: 1-100% ; the solution concentrations to be used are 0.01-0.1M; Take the volumes of solution to be used between 1-50 mL
6. The solubilities of the sulfate and chromate of Barium in this reagent is used to distinguish the 2 compounds. (Provide only the chemical formula) 7. How should you write the chemical formula of zinc ammonia complex ion? 8. Identify the chemical formula of Grp 3 cation/s that form a pink precipitate when treated with thioacetamide. 9. What reagent acts as buffer to prevent precipitation of Magnesium Hydroxide during the analysis of Grp 3 cations? (chemical formula) 10. What ion is reduced when a precipitate which may contain Barium Chromate is added with HCl and concentrated? (chemical formula of the resulting reduced ion)
An unknown salt X reacts with hot conc. H2SO4 to produce a brown coloured gas which intensifies on addition on copper turnings. On adding dilute ferrous sulphate solution to an aqueous solution of X and then carefully adding conc. H2SO4along the sides of the test tube, a brown complex Y is formed at the interface between the solution and H2SO4. Identify X andY and write the chemical equation involved in the reaction.
Give a list of laboratory apparatus and equipment that are to be utilized for the preparation of 500 mL of 0.2 M K4 Fe (CN) 6. Also give the procedure of preparation.
Calculate the equilibrium concentration of N2O4 in 1.00 L of a solution prepared from 0.129 mol of N2O4 with chloroform as the solvent. (Assume that the change in concentration of N2O4 is small enough to be neglected).
why does this happen? After the sodium oxalate was added to the lead nitrate, a white precipitate formed immediately. After letting this solution sit for a few minutes, the precipitate fell to the bottom of the test tube. There was about 2.4 cm of white precipitate at the bottom of the test tube. After the nitric acid was added, there was only 0.3 cm of precipitate at the bottom of the test tube.
Regarding the stability of the permanganate solution: describe the reactions that occur when it decomposes. Indicate which factors catalyze its decomposition and indicate how they can be controlled.
1. The substance to be analyzed – is white, highly soluble in water salt. When interacting with concentrated sulfuric acid – evolving of some odorless and colorless gas is observed. Reaction with diluted acids or NaOH solution doesn’t lead to any precipitation. Interaction with Nessler's reagent leads to formation of reddish-brown precipitate. Addition of barium chloride solution leads to appearance of white precipitate, which soluble in acetic acid. What kind of salt is this? Explain you answer, provide chemical equations
Bleach (sodium hypochlorite, NaOCl, a strong oxidizing agent) neutralizes and inactivates mustard gas. Bleach is also effective on organic stains because it oxidizes coloredcompounds to colorless compounds. Propose products that might be formed by thereaction of mustard gas with bleach
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 SiF6 2− ions)(b) Ce(IO3)4, 1.5 × 10–2 g/100 mL(c) Gd2(SO4)3, 3.98 g/100 mL(d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr6 2− ions)