Part A What is the net ionic equation of the reaction of FeCl2 with NaOH? Express you answer as a chemical equation including phases. , View Available Hint(s) emplates Symbols uado redo resat keyboard shortcuts help A chemical reaction does not occur for this question. Submit Part B What is the net ionic equation of the reaction of M9SO4 with Pb(NO3)2? Express you answer as a chemical equation including phases. , View Available Hint(s) V. Templates Symbols uado redo resat keyboard shortcuts help A chemical reaction does not occur for this question. Submit Provide Feedback

Part A What is the net ionic equation of the reaction of FeCl2 with NaOH? Express you answer as a chemical equation including phases. , View Available Hint(s) emplates Symbols uado redo resat keyboard shortcuts help A chemical reaction does not occur for this question. Submit Part B What is the net ionic equation of the reaction of M9SO4 with Pb(NO3)2? Express you answer as a chemical equation including phases. , View Available Hint(s) V. Templates Symbols uado redo resat keyboard shortcuts help A chemical reaction does not occur for this question. Submit Provide Feedback

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 51E: Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production...

See similar textbooks

Similar questions

Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production of uranium, titanium, and other active metals) is isolated from sea water by the following sequence of reactions: Mg2+(aq)+Ca(OH)2(aq)Mg(OH)2(s)+Ca2+(aq)Mg(OH)2(s)+2HCl(aq)MgCl2(s)+2H2O(l)MgCl2(l)electrolysisMg(s)+Cl2+Cl2(g) Sea water has a density of 1.026 g/cm3 and contains 1272 parts per million of magnesium a5 Mg2+(aq) by mass. What mass, in kilograms, of Ca(OH)2; is required to precipitate 99.9% of the magnesium in 1.00103 L of sea water?
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 C), filtering to remove insoluble impurities, cooling to 0 C to precipitate solid NaHCO3, and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 C is 164 g/L. Its solubility in cold water of 0 C is 69 g/L. What is the percent yield of NaHCO3 when ills purified by this method?
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
A. CaSO4 B. Ba3(PO4)2 C. PbS D. Pb3(PO4)2 Complete the following statements by entering the letter(s) corresponding to the correct compound(s). (If more than one compound fits the description, include all the relevant compounds by writing your answer as a string of characters without punctuation, e.g, ABC.) Without doing any calculations it is possible to determine thatcobalt(II) carbonate is more soluble than _______, and cobalt(II) carbonate is less soluble than _______ It is not possible to determine whether cobalt(II) carbonate is more or less soluble than _________ by simply comparing Kspvalues.
Write the balanced neutralization reaction that occurs between H2SO4H2SO4 and KOHKOH in aqueous solution. Phases are optional. Suppose 0.650 L0.650 L of 0.440 M H2SO40.440 M H2SO4 is mixed with 0.600 L0.600 L of 0.240 M KOH0.240 M KOH. What concentration of sulfuric acid remains after neutralization?
A 1.00 g sample of a magnesium-aluminum alloy yields 0.107 g H2 when treated with an excess of HCl(aq). What is the percentage by mass of Al in the alloy? [Hint: This is the inverse of Example 4-16. To solve this problem, let m and 1.00 - m be the masses of Al and Mg, respectively, and then use these masses in the setup above to develop an equation that relates m to the total mass of H2 obtained. Then solve for m.]
5. A 0.5664 g ore sample is dissolved in nitric acid and then filtered. The aluminum is present in solution as Al3+. The solution is made basic with ammonium hydroxide, NH4OH, and the aluminum hydroxide, Al(OH)3 (FW 78.004), precipitates. This gel is filtered in a porous glass crucible, rinsed with dilute ammonium hydroxide, ignited, cooled in a desiccator, and weighed. The resulting alumina, Al2O3 (FW 101.94), weighed 0.1605 g. Why is the solution filtered after acid dissolution? To remove insoluble matrix material (like sand, etc.) 6. In #5, why rinse with ammonium hydroxide solution? To avoid peptization or loss of precipitate. Ammonium hydroxide is a volatile electrolyte. 7. In #5, what chemical transformation takes place during ignition? (Show the balanced chemical equation) 2Al(OH)3 -> Al2O3 + 3H2O 8. In #5, why use a desiccator during cooling? To avoid weight gain by adsorption of atmospheric water. 9. In #5, calculate the weight percent Al (AW 26.9815) in the sample.
Write the balanced COMPLETE ionic equation for the reaction when KCl and Na₃PO₄ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
Write the balanced COMPLETE ionic equation for the reaction when CaCl₂ and Na₃PO₄ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
Sodium metal (Na(s)) reacts exothermically with water to produce a basic solution of sodium hydroxide (NaOH(aq)) and hydrogen gas (H2(g)). The hear released is sufficient to ignite the hydrogen gas produced, which burns in oxygen (O2(g)) to produce water vapor (H2O(g)). Write balanced equations for these two chemical reactions.
Sample: Saline 0.900% (m/v), in sodium chloride (NaCl). Data: M.A. (g/mol): Na = 22.9898; K = 39.0983; Cr=51.9961; Ag = 107.8682; Cl = 35.453; N=14.0067; O = 15.9994. Material available in the laboratory's warehouse: Reagents: distilled water; standardized solution of silver nitrate (AgNO₃), at a concentration of 0.09980 mols/L; Potassium chromate solution (K₂CrO₄) 1%; ammoniacal ferric alum solution [Fe(NH₄)(SO₄)₂] and; nitrobenzene (or cooking oil, alternatively); 0.1000 mols/L potassium thiocyanate (KSCN) standard solution. Glassware: beakers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyers; 10.00 and 25.00 mL volumetric pipettes; 15.00 mL burette; 30.00, 50.00 and 100.00 mL volumetric flasks Calculate the molarity of saline, in terms of the NaCl concentration (concentration in mols/L). (a) 0.900 mols/L (b) 5.84 mols/L (c) 0.154 mols/L (d) 0.0154 mols/L