6. (2 pts) Aqueous solutions of a compound did not form precipitates with Cl, Br, I, SO,2", CO;²,, PO4³-, OH", or S2. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified with HCl (aq). This compound is A) Pb(NO3)2 B) (NH4)2S C) KBr D) Li2CO3 E) AgNO3

6. (2 pts) Aqueous solutions of a compound did not form precipitates with Cl, Br, I, SO,2", CO;²,, PO4³-, OH", or S2. This highly water-soluble compound produced the foul-smelling gas H2S when the solution was acidified with HCl (aq). This compound is A) Pb(NO3)2 B) (NH4)2S C) KBr D) Li2CO3 E) AgNO3

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

See similar textbooks

Similar questions

In the standardization of HCl using pure anhydrous sodium carbonate as the primarystandard for methyl orange as an indicator, 1.0 mL HCl was found to be equivalent to 0.05gof sodium carbonate (MW =106). The normality of HCl is:
The aluminum in a 1.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al2O3.xH2O. The precipitate was filtered and ignited at to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysis in terms of %NH4Al(So4)2 %Al2O3 %Al
Calculate the weight of pure sodium carbonate that is necessary to prepare 2.806 L of 0.223 N Na2CO3 (105.99 g/mol) from the primary-standard solid. Assume the solution is to be used for titrations in which the reaction is: CO32- + 2H+ ----> H2O + CO2 Express you answers in 3 decimal places
A 0.2500-g of dry CaCO3 was completely dissolved into a solution of 5-mL conc. HCl and 50-mL distilled water in an erlemeyer flask. The resulting solution was boiled for 5 minutes to expel CO2 from the reaction, and then it was cooled to room temperature and the solution was transferred in a 500-mL volumetric flask filled to volume by rinsing the erlenmeyer flask and combining all the washings to fill the mark. A 5.0-mL aliquot of the CaCl2 solution was taken from the orignal solution and was transferred into an erlenmeyer flask with 10-mL NH3 buffer, 20-mL distilled water, and 5 gtts of EBT. The solution consumed 4.96 mL of an EDTA solution. MW: CaCO3 = 100.1 Compute for the N EDTA solution.   0.0053 N   0.0531 N   0.5313 N   None of the choices
25.0mL of a 0.515 M K2S solution is mixed with 30.0 mL of 0.833 M HNO3 acid solution to give the following reaction:                               K2S(aq) + 2HNO3(aq)   →  2KNO3(aq) + H2S(g) H2S is an unwanted by-product in a pulp and paper industry. To capture H2S gas, it is bubbled through a NaOH solution to produce Na2S with a yield of 94%. H2S(g) + 2NaOH (aq)   →  Na2S (aq) +  2H2O(l) The mass of H2S(g) that was processed (in kg) if 10.76 kg of Na2S was collected is
Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol ?    What is the molar concentration of the prepared KOH solution?…
Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol What is the molar concentration of the prepared KOH solution?…
1. Calculate the equivalent weight of KMnO₄ in the following reaction: MnO₄⁻ + CN⁻ + H₂O ⟶ MnO₂ (s) + CNO⁻ + OH⁻) 2. Calculate the normality and molarity of a 15.0% (by weight) H₂SO₄ solution with a specific gravity of 1.090. * 3. To what volume should 100 mL of the above solution be diluted to prepare 1.50 N solution?
A sample containing chlorophenol, C6H4ClOH, was analysed by gravimetric analysis. A 0.783-g of this sample goes through a chemical process allowing the chlorine in the chlorophenol to precipitate as silver chloride, weighing 0.271 g. Calculate the % (wt/wt) of the chlorophenol in the sample, assuming that chlorophenol is the only source of chlorine in the sample. Provide your answer to two decimal places and without units. Avoid using scientific notation.
One litre of a saturated aqueous solution of Ag2SO4 (MW = 311.79 g mol- 1) at 25 °C is evaporated to dryness. 4.844 g of Ag2SO4 residue was produced. What is the solubility product (Ksp)?
What is the concentration of ions in the soil solution after fertilizer application? Suppose that 122 pounds of K+ were applied per acre, then a gentle rain soaked the top 10 inches of soil to field capacity, which for the given soil was about 16% water by volume. If the K+ was applied as KCl, it is plausible that it all dissolved and distributed relatively uniformly with the infiltrating water. If so, then what was the K+ concentration in the soil solution in mol K+/L solution? Note that the volume can be computed like we do for an acre-furrow-slice (AFS), as area times depth. This is going to be a relatively small number, so please report your answer in mol K+/L solution to at least 5 decimal places.
Consider Palmitic acid C16H32O2, a common fatty acid used in the manufacture of soap. A solution of palmitic acid is prepared by mixing 112 g palmitic acid with 725 mL of benzene C6H6. The density of the resulting solution is 0.902 g/mL. Palmitic acid (molar mass = 256 g/mol and density = 0.852 g/mL); Benzene (molar mass = 78 g/mol and density = 0.879 g/mL) What is the %m/m of the solution? Final answer must be rounded off to 1 decimal place, and shall NOT have any unit.