Use the References to access important values if needed for this question. A sample of a substance with the empirical formula XCI₂ weighs 0.5351 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.2478 g. The chemical reaction is XCl₂ + 2 AgNO3-2AgCl + X(NO3)2 (a) Calculate the formula mass of XCI₂. Formula mass XCl₂ = (b) Calculate the atomic mass of X. Atomic mass X= g mol-¹ g mol-1

Use the References to access important values if needed for this question. A sample of a substance with the empirical formula XCI₂ weighs 0.5351 g. When it is dissolved in water and all its chlorine is converted to insoluble AgCl by addition of an excess of silver nitrate, the mass of the resulting AgCl is found to be 1.2478 g. The chemical reaction is XCl₂ + 2 AgNO3-2AgCl + X(NO3)2 (a) Calculate the formula mass of XCI₂. Formula mass XCl₂ = (b) Calculate the atomic mass of X. Atomic mass X= g mol-¹ g mol-1

World of Chemistry

7th Edition

ISBN:9780618562763

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 50A

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39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.
Twenty-five mL of a 0.388 M solution of Na2SO4 is mixed with 35.3 mL of 0.229 M Na2SO4. What is the molarity of the resulting solution? Assume that the volumes are additive.
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 mixture consisting of only sodium chloride (NaCl) andpotassium chloride (KCl) weighs 1.0000 g. When the mixtureis dissolved in water and an excess of silver nitrate isadded, all the chloride ions associated with the originalmixture are precipitated as insoluble silver chloride (AgCl).The mass of the silver chloride is found to be 2.1476 g.Calculate the mass percentages of sodium chloride andpotassium chloride in the original mixture.
Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride, CaCL2. To precipitate the calcium ion from the resulting solution, an excess of potassium oxalate was added. The precipitate of calcium oxalate, CaC2O4, weighed 1.437 g. What was the molarity of CaCl2 in the solution?
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