Be sure to answer all parts. What is the maximum mass (in grams) of each of the following soluble salts that can be added to 260 mL of 0.050 M BaCl₂ without causing a precipitate to form? (Assume that the addition of solid causes no change in volume.) (a) (NH4)2SO4 1.029x105 g (Enter your answer in scientific notation.) (b) Pb(NO3)2 (c) NaF

Be sure to answer all parts. What is the maximum mass (in grams) of each of the following soluble salts that can be added to 260 mL of 0.050 M BaCl₂ without causing a precipitate to form? (Assume that the addition of solid causes no change in volume.) (a) (NH4)2SO4 1.029x105 g (Enter your answer in scientific notation.) (b) Pb(NO3)2 (c) NaF

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter4: Chemical Reactions In Solution

Section: Chapter Questions

Problem 4.83QE: A solid forms when excess barium chloride is added to 21 mL of 3.5 M ammonium sulfate. Write the...

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Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.
An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
A solid forms when excess barium chloride is added to 21 mL of 3.5 M ammonium sulfate. Write the overall equation, and calculate the mass of the precipitate.
For a product to be called vinegar, it must contain at least 5.0% acetic acid, HC2H3O2, by mass. A 10.00-g sample of a raspberry vinegar is titrated with 0.1250 M Ba(OH)2 and required 37.50 mL for complete neutralization. Can the product be called a vinegar?
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?
The molarity of iodine in solution can be determined by titration with arsenious acid, H3AsO4. The unbalanced equation for the reaction is H3AsO3(aq)+I2(aq)+H2O2 I(aq)+H3AsO4(aq)+2 H+(aq)A 243-mL solution of aqueous iodine is prepared by dissolving iodine crystals in water. A fifty-mL portion of the solution requires 15.42 mL of 0.134 M H3AsO3 for complete reaction. What is the molarity of the solution? How many grams of iodine were added to the solution?
In order to determine the purity of ammonium sulfate, a sample with a mass of 0.850 g is dissolved in KOH. The equation for the reaction that takes place is NH4+(aq)+OH(aq)NH3(aq)+H2OThe ammonia liberated is distilled into a flask that contains 50.00 mL of 0.250 M HCI. Not all the HCI is consumed. The excess HCI reacts with 17.3 mL of 0.120 M NaOH. What is the mass percent of (NH4)2SO4 in the sample?
What mass of NaOHNaOH is needed to precipitate the Cd2+ ions from 30.0mL of 0.500 M Cd(NO3)2 solution?
An aqueous solution of silver acetate, AgC2H3O2, 50.0 mL and 0.300 M, is mixed with 25.00 mL of 0.300 M iron (III) chloride, FeCl3. Calculate the mass of any precipitate formed and the concentration of each ion remaining in solution.
what mass of Na2CrO4 is required to precipitate all of the silver ions from 55.0 mL of a 0.300 M solution of AgNO3?
Make a complete schematic diagram for the precipitation, separation, and identification of Group V Cations.

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