X bAnswered: Chemistry Question |X (74) How to Write Complete lonic X 101 Chem 101 app.101edu.co Submit Question 37 of 43 Write the balanced COMPLETE ionic equation for the reaction when KOH and Cu(NO3)2 are mixed in aqueous solution. If no reaction occurs, write only NR. 4- |2- |2+ 3+ 4+ + 83 1 2 3 4 5 6 7 0 4 3 17 1 5 (g) (aq) (s) (1) NR Cu Н N K Reset Delete x H20 8:12 PM е OTYPE here to search 11/7/2019 S LO

X bAnswered: Chemistry Question |X (74) How to Write Complete lonic X 101 Chem 101 app.101edu.co Submit Question 37 of 43 Write the balanced COMPLETE ionic equation for the reaction when KOH and Cu(NO3)2 are mixed in aqueous solution. If no reaction occurs, write only NR. 4- |2- |2+ 3+ 4+ + 83 1 2 3 4 5 6 7 0 4 3 17 1 5 (g) (aq) (s) (1) NR Cu Н N K Reset Delete x H20 8:12 PM е OTYPE here to search 11/7/2019 S LO

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 158IP: The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with...

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Iron (II) can be oxidized to iron (III) by dichromate ion, which is reduced to chromium (III) in acid solution. A 2.5000-g sample of iron ore is dissolved and the iron converted into iron(II). Exactly 19.17? ml. of 0.0100 M Na2Cr2O7 is required in the titration. What percentage of the ore sample was iron?
The vanadium in a sample of ore is converted to VO2+. The VO2+ ion is subsequently titrated with MnO4 in acidic solution to form V(OH)4+ and manganese(II) ion. The unbalanced titration reaction is MnO4(aq)+VO2++(aq)+H2O(l)V(OH)4+(aq)+Mn2+(aq)+H+(aq) To titrate the solution, 26.45 mL of 0.02250 M MnO4 was required. If the mass percent of vanadium in the ore was 58.1 %, what was the mass of the ore sample? Hint: Balance the titration reaction by the oxidation states method.
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?
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?
68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
A sample containing NaCl, NaBr, & inert material weighs 1.000 g. Excess of AgNO3 gave a whiteprecipitate consisting of only AgCl and AgBr which weighs 0.5260 g. By heating the precipitate in a currentof Cl2 gas, the AgBr (187.78 g/mol) is converted to AgCl (143.32 g/mol) and the precipitate weighs 0.4260g. Find the % NaCl (58.44 g/mol) and % NaBr (102.909 mol) in the original sample.
Write the balanced neutralization reaction that occurs between H2SO4H2⁢SO4 and KOHKOH in aqueous solution. Phases are optional. Suppose 0.950 L0.950 L of 0.400 M H2SO40.400 M H2⁢SO4 is mixed with 0.900 L0.900 L of 0.300 M KOH0.300 M KOH. What concentration of sulfuric acid remains after neutralization?
Sodium formate reacts with permanganate in neutral solution according to the equation CHO2 + MnO4 + H2O → MnO2(s) + CO2 + OH" (a) A 0.500 g sample containing sodium formate is treated with 50.00 mL of 0.0600 M MnO4 (an excess) in neutral solution, and the reaction given above is allowed to proceed to completion. The solution is filtered to remove the MnO2, acidified with H2SO4, and titrated with 30.00 mL of 0.1000 M H2C2O4. The MnO4- is reduced to Mn2+ and the oxalate oxidized to CO2. Calculate the percentage of NaCHO2 in the sample.
e. In one experiment, 0.2480 g sample of CaCO3 was dissolved in an acidic solution. The calcium was precipitated as CaC2O4.H2O and the dry precipitate was weighed at 0.3084 g. Calculate the percentage of CaO in the sample (Molecular weight CaCO3 = 100 g mol-1, CaC2O4.H2O = 146 g mol-1, CaO = 56 g mol-1).
A sample of solid Eu(OH)3 was stirred in water at a certain temperature until the solution contained as much dissolved Eu(OH)3 as it could hold. A 650-mL sample of this solution was withdrawn and titrated with 1.33e-05 M HBr. It required 21 mL of the acid solution for neutralization.What is the solubility of Eu(OH)3 in water, at the experimental temperature, in grams of Eu(OH)3 per liter of solution? a) The solubility is 7.06e-10 g/L. b) The solubility is 8.72e-05 g/L. c) The solubility is 0.000262 g/L. d) The solubility is 2.91e-05 g/L. e) The solubility is 6.08e-06 g/L.
A 280.5 mg sample containing only Pb3O4and inert matter gives a precipitate of PbSO4 weighing 381.5 mg. What is the purity of the sample?
The concentration of KClO3 in the explosive sample can be determined by reaction with Fe(II):ClO3- + 6Fe2+ + 6H+ Cl- + 3H2O + 6Fe3+. 50.00 ml of 0.08930 M Fe2+ solution was added to 0.1279 grams of explosive sample, and after the reaction, the excess Fe2+ was titrated with 0.08361 M Ce4+ solution, which consumed 14.93 ml. Calculate the KClO3 concentration of the explosive sample in percent by weight.