The following reaction scheme is given: Aluminum metal added to a strong base aqueous solution provides a colorless solution (A), releasing a colorless gas (B). Introduction of carbon dioxide gas into (A) precipitates a white gelatinous precipitate (C). (C) is divided into two equal parts. To one portion, excess sodium hydroxide solution is added, dissolving the precipitate to a colorless solution (D). By annealing the other part of (C) at high temperature, an anhydrous white oxide (E) is formed. Write the corresponding equilibrium chemical equations for the described reactions and name the chemical forms (A) to (E).

The following reaction scheme is given: Aluminum metal added to a strong base aqueous solution provides a colorless solution (A), releasing a colorless gas (B). Introduction of carbon dioxide gas into (A) precipitates a white gelatinous precipitate (C). (C) is divided into two equal parts. To one portion, excess sodium hydroxide solution is added, dissolving the precipitate to a colorless solution (D). By annealing the other part of (C) at high temperature, an anhydrous white oxide (E) is formed. Write the corresponding equilibrium chemical equations for the described reactions and name the chemical forms (A) to (E).

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 113QRT: A 0.250-M sodium sulfate solution is added to a 0.200-M barium nitrate solution and 0.700 g barium...

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A 0.250-M sodium sulfate solution is added to a 0.200-M barium nitrate solution and 0.700 g barium sulfate precipitates. Write the balanced equation for this reaction. Calculate the minimum volume of barium nitrate solution that was used. Calculate the minimum volume of sodium sulfate needed to precipitate 0.700 g barium sulfate. Assume 100% yield.
When you mix solutions of lead (II) nitrate and potassium iodide,(i) What is the colour of the precipitate formed? Name the compound evolved?
(a) Halogen, V reacts with hydrogen gas to form HV only when heated to 200 °C in the presence of a platinum catalyst. An aqueous solution of HV is formed when HV is dissolved in water. When aqueous silver nitrate solution is added to the HV solution, precipitate W is formed. With the aid of a balanced chemical equation, explain the reaction between precipitate W and concentrated ammonia solution. () (i) The melting point of hydrogen fluoride, HF is higher than HV. Explain this phenomenon in terms of structure and bonding.
A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the molar concentration of the hydroxide ion in the saturated solution?
I need the net ionic equation for the reactions below: -Dissolution of silver oxalate with nitric acid -Dissolution of silver chloride with aqueous ammonia -Oxidation of the iodide ion by hypochlorite solution -Precipitation of the sulfate ion with barium ion -Dissolution of barium phosphate solution with hydrochloric acid -Reaction of sodium phosphate solution with hydrochloric acid -Reaction of phosphoric acid with ammonium molybdate solution -Precipitation of the oxalate ion with calcium ion -Reaction of calcium axalate with sulfuric acid -Reaction of oxalic acid with acidic permanganate solution -Production of carbon dioxide from solid sodium carbonate and hydrochloric acid -Production of acetetic acid or ethyl acetate in sulfuric acid Thank you
(a) Write chemical equations to show what happens when each of the following substances is mixed with water: (1) Hydride ion (ii) Glucose, C6H12O6(s) (iii) Copper(II) bromide (iv) Formic acid (b) Write chemical equations for the following processes: 1. Chemical reaction for ΔHf for mercury(I) phosphate 2. Thermal dissociation of gaseous bromine 3. Sublimation of carbon dioxide 4. Reduction of VO2+ to produce VO2+ 5. Neutralization of sulfuric acid by barium hydroxide 6. Themal decomposition of I mol of sodium bicarbonate to produce soditum carbonate, carbon dioxide and water
Precipitation of the sulfate ion with barium ion -Dissolution of barium phosphate solution with hydrochloric acid -Reaction of sodium phosphate solution with hydrochloric acid -Reaction of phosphoric acid with ammonium molybdate solution I need the net ionic equation and state of the reactions bellow: -Precipitation of the oxalate ion with calcium ion -Reaction of calcium axalate with sulfuric acid -Reaction of oxalic acid with acidic permanganate solution -Production of carbon dioxide from solid sodium carbonate and hydrochloric acid -Production of acetetic acid or ethyl acetate in sulfuric acid Thank you
Accounts for the following(i) Rusting of iron is quicker in saline water than in ordinary water.(ii) Blocks of magnesium are straped to the steel hubs of ocean going ships.
what mass of solid lanthanum oxalate nonahydrate can be obtained from 650 ml of 0.0170 m aqueous solution of LaCl3 by adding a stoichiometric amount of sodium oxalate
A sample of 70.5 mg of potassium phosphate is added to 15.0 mL of 0.050 M silver nitrate, resulting in the formation of aprecipitate. (a) Write the molecular equation for the reaction. (b) What is the limiting reactant in the reaction? (c) Calculatethe theoretical yield, in grams, of the precipitate that forms.
Which methods are usually employed for purifying the following metals :(i) Nickel (ii) GermaniumMention the principle behind each one of them.
Potassium Ferrioxalate is mixed with in 50 mL of 1 M H2SO4 In a beaker , it is then placed one-half of this solution in another beaker in the sun and the other half in a cabinet in the dark. the color of both solutions after 0, 5, 15, and 30 minutes are : In the sun it stayed clear the whole 30 min and the sample in the darkness of the cabinet turned light green, Briefly explain your observations in terms of the photochemical properties of ferrioxalate.