first question o uoL0.44 MreasTon occurse inr.A chemist wishes to precipitate yttrium cations out of a 1.00L solution. If the concentration of [Y"] insolution is 0.428 M and the Ksp of yttrium iodate is 1.12 x 1010, what mass of potassium iodate (KIO3) must beadded so that precipitation may begin? The molar mass of potassium iodate is 214.00 g/mol.(27)thisakes.くて。のuo(v)99'1664.0 Hg(6.4 x 10° g)(8)411 mg(5.6 x 10* g)(a)(E) 137 mgSu 0'95The standard Gibbs free energy associated with the following reaction is -91.2 kJ:HCI (g) + NH3 (g) → NH,CI (s)(28)What will be the value of AGxn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atmand the partial pressure of NH3 (g) is 0.284 atm?-95.1 kJ(v)(B) -90.7 kJ())3.93 kJ-79.5 kJ(a)-87.3 kJ(E)

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e in kes. A chemist wishes to precipitate yttrium cations out of a 1.00 L solution. If the concentration of [Y"] in solution is 0.428 M and the Kp of yttrium iodate is 1.12 x 1010, what mass of potassium iodate (KIO,) must be added so that precipitation may begin? The molar mass of potassium iodate is 214.00 g/mol. (27) (6.4 x 10° g) (v) (8) 3 9'16 arl O'v9 411 mg (5.6 x 10 g) (a) 137 mg 3u 0'9s (3)

e in kes. A chemist wishes to precipitate yttrium cations out of a 1.00 L solution. If the concentration of [Y"] in solution is 0.428 M and the Kp of yttrium iodate is 1.12 x 1010, what mass of potassium iodate (KIO,) must be added so that precipitation may begin? The molar mass of potassium iodate is 214.00 g/mol. (27) (6.4 x 10° g) (v) (8) 3 9'16 arl O'v9 411 mg (5.6 x 10 g) (a) 137 mg 3u 0'9s (3)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 68QAP: 68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming...

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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?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
When 85.0 mL of 0.250 M Ba(OH)2 solution is added to 85.00 mL of 0.250 M Al (NO3)3 solution, a white gelatinous precipitate of Al(OH)3; is formed. Assuming 100% yield, (a) what mass (in grams) of Al(OH)3 is formed? (b) what is the molarity of each of the ions Ba2+, OH-, Al3+, NO3- in the resulting solution?
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?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion. :math>PbSe. BaCO3 :math>Mg(OH)2f. AlPO4 :math>Na2SO4g. PbCl2 :math>(NH4)2Sh. CaSO4
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)
Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
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?