Reagents A. Cu(SO4)2, NaHCO3, Na-citrate B. concentrated HCI, orcinol, FeCl3 C. Alkyl chloride, AlCl3 D. NH₂OH, alcoholic HCI, alcoholic KOH, FeCl 3 E. Dilute KMnO4 F. NaOH, KI, I₂ G. FeCl3 Observation H. blue-green solution 1. Formation of purple-colored solution J. Decolorization of purple solution and formation of brown precipitate K. Formation of yellow precipitate L. Formation of a colored complex M. Appearance of a brick red precipitate N. Change in color of the crystal; warm test tube Given the following reagents and tests above, what could best differentiate the two compounds below? Provide also the letter of the expected experimental observation and state which of the two would give that result. OH OH OH

Reagents A. Cu(SO4)2, NaHCO3, Na-citrate B. concentrated HCI, orcinol, FeCl3 C. Alkyl chloride, AlCl3 D. NH₂OH, alcoholic HCI, alcoholic KOH, FeCl 3 E. Dilute KMnO4 F. NaOH, KI, I₂ G. FeCl3 Observation H. blue-green solution 1. Formation of purple-colored solution J. Decolorization of purple solution and formation of brown precipitate K. Formation of yellow precipitate L. Formation of a colored complex M. Appearance of a brick red precipitate N. Change in color of the crystal; warm test tube Given the following reagents and tests above, what could best differentiate the two compounds below? Provide also the letter of the expected experimental observation and state which of the two would give that result. OH OH OH

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter7: The Structure Of Atoms And Periodic Trends

Section: Chapter Questions

Problem 65IL: Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel....

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Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel. It can be prepared in the general chemistry laboratory by treating nickel(II) acetate with formic acid (HCO2H). Ni(CH3CO2)2(aq) + 2 HCO2H(aq) Ni(HCO2)2(aq) + 2 CH3CO2H(aq) Green crystalline Ni(HCO2)2 is precipitated after adding ethanol to the solution. (a) What is the theoretical yield of nickel(II) formate from 0.500 g of nickel(II) acetate and excess formic acid? (b) Is nickel(II) formate paramagnetic or diamagnetic? If it is paramagnetic, how many unpaired electrons would you expect? (c) If nickel(II) formate is heated to 300 C in the absence of air for 30 minutes, the salt decomposes to form pure nickel powder. What mass of nickel powder should be produced by heating 253 mg of nickel(II) formate? Are nickel atoms paramagnetic?
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)
In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)
23. Silver (1) ions form a precipitate with chromate ions. Ksp = 9.0 x 10-¹2. a. Write the balanced chemical equation of the reaction. Indicate physical states of all reaction components. 4 Agcag) + Croucags + Ay₂ CrO4(s) t b. Calculate the solubility of the precipitate in pure water. C. Calculate the solubility of the precipitate in a solution containing 0.100 M potassium nitrate.
Which of the following compounds is the most soluble in water based on its Ksp value? A. CuS, Ksp = 1.27 x 10^-36B. PbS, Ksp = 9.04 x 10^-29C. AgCl, Ksp = 1.77 x 10^-10D. AgI, Ksp = 8.51 x 10^-17E. There is not enough information in the prompt to answer this question.
Chemistry 3. (6%) Ca(HCO3 ) 2 is called calcium bicarbonate. It is one of the most abundant compounds in water, the hardness of this water sample is measured at 162 mg/L as CaCO 3 . Determine 3a. Molar concentration of HCO 3- ions (2%) 3b. Normal concentration of Ca 2+ ions. (2%) 3c. Mass fraction of calcium bicarbonate (Ca(HCO 3 ) 2) (2%) 4. (2%) Percentage of each gas in dry air is listed in the table below. Currently, the percentage of nitrogen gas (N2 ) is 77%. Determine the percentage of O2 gas, CO2 gas, Ar gas and H2 O in the moist air. Gas Percentage N2 78.08% O2 20.95% Ar 0.93% CO2 0.035%
Solubility of CrF3 in water is 0.120 g/L at 25 oC. What is the molar concentration of F- ion in the solution at the same temperature? A.) 3.30 x 10-3 B.) 3.97 x 10-11 C.) 1.10 x 10-2 D.) 2.80 x 10-3 E.) 3.10 x 10-4
a. A 1.00 liter solution contains 0.45 moles nitrous acid and 0.35 moles potassium nitrite .If 0.17 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HNO2 will decrease. B. The number of moles of NO2- will decrease. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase. b. A 1.00 liter solution contains 0.38 M ammonia and 0.49 M ammonium bromide. If 0.120 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) A. The number of moles of NH3 will decrease. B. The number of moles of NH4+ will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will increase. E. The ratio of [NH3] /…
SOLUBILITY PRODUCT PRINCIPLE (? Calcium citrate (Ca3(C6H507)2; MM = 498.46 g/mol), a common food preservative, has a Ksp of 1.12 × 10-15 at 25 °C. A. Write the reaction equation for the dissolution of Ca3(C6H5O7)2 solid (in your solution sheet). B. Calculate the solubility in mg/L at 25 °C in pure water. Neglect other competing equilibria. C. Calculate the solubility in mg/L at 25 °C in the presence of 0.010 M CaCl2. Neglect other competing equilibria. Assume that 3s << 0.010 M. D. Is the assumption that s << 0.010 M valid? (Yes or No)
a. Solid sodium hydroxide is slowly added to 125 mL of a 0.0475 M iron(II) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is M. b. Solid sodium carbonate is slowly added to 150 mL of a 0.0396 M silver nitrate solution. The concentration of carbonate ion required to just initiate precipitation is M. c. Solid magnesium nitrate is slowly added to 75.0 mL of a 0.0635 M sodium carbonate solution. The concentration of magnesium ion required to just initiate precipitation is M.
1. Mg metal + 6M HCl No reaction Readily dissolved with H2 gases evolved Partially dissolved with the evolution of H2 gases 2. When potassium chlorate (KClO3) was heated, it produces a ________. luminol gypsum sugary gummy bear
Solid aluminum hydroxide (Ksp = 1.3 x 10-33) is added to 3.50 mM Al(NO3)3 solution until the solid no longer dissolves. What is the molar solubility of Al(OH)3 in the given solution? a. 2.40 x 10-11 M b. 3.46 x 10-11 M c. 1.24 x 10-31 M d. 2.63 x 10-9 M