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 250 mL of 0.050 M BaCl, without causing a precipitate to form? (Assume that the addition of solid causes no change in volume.) "os"HN) (E) x 10 (Enter your answer in scientific notation.) (b) Pb(NO,)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 250 mL of 0.050 M BaCl, without causing a precipitate to form? (Assume that the addition of solid causes no change in volume.) "os"HN) (E) x 10 (Enter your answer in scientific notation.) (b) Pb(NO,)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

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.74QE: Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman...

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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?
Calcium oxalate, CaCO4, is very insoluble in water. What mass of sodium oxalate,Na2C2O4, is required to precipitate the calcium ion from 37.5 mL of 0.104 M CaCl2solution?
You have a solution of 1M BaCl2 and another of 1M Hg2(NO3)2. If you poured them together, what precipitate, if any, would you expect to form?
3) When excess sliver nitrate was added to 25.00 ml of barium chloride, a precipitate of sliver chloride formed at the bottom of the beaker. If the mass of the precipitate was 4.30g, calculate the initial concentration of barium chloride.
Moly Cule is also mixing a solution of calcium fluoride (CaF2). If she adds some Aqueous Calcium Oxide (CaO) to the solution, can she eventually get some solid CaF2 to form? What dictates how much Ca2+ and F- are in solution, and how much are in solid CaF2. Since Ca(OH)2 is a strong base and HF is a weak acid, would adding some strong NaOH (another strong base) to the solution cause a precipitate to form? Why or why not?
Solid ammonium carbonate is slowly added to 175 mL of a 0.0585 M lead nitrate solution. What is the concentration (in M) of carbonate ion required to just initiate precipitation?
You are asked to weigh 2 g of lithium and add it to 1500 ml of distilled water +2 drops of indicator, knowing that the density of water is 1 at room temperature while conducting this experiment. After determining the molarity of the LIOH, you need to know how many volume should be taken to reach the final concentration. Therefore, use the one underneath, so the molarity after dilution will be 0.025 M instead of 0.25 MAfter knowing the amount of LiOH, you need to dilute to prepare 0.025 M of LiOH in a 3000 ml solution. Show your calculation and units. dont forget to use Use this equation to calculate ( CLiOH x VLiOH) before dilution = (CLiOH x VLiOH) after dilution
You are asked to weigh 2 g of lithium and add it to 1500 ml of distilled water +2 drops of indicator, knowing that the density of water is 1 at room temperature while conducting this experiment. After determining the molarity of the LIOH, you need to know how many volume should be taken to reach the final concentration. Therefore, use the one underneath, so the molarity after dilution will be 0.025 M instead of 0.25 MAfter knowing the amount of LiOH, you need to dilute to prepare 0.025 M of LiOH in a 3000 ml solution. Show your calculation and units.
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.
A titration experiment between barium oxalate and HCl was done, with HCl as the titrant. The barium oxalate was prepared by dissolving the solid in 100 mL water, once it was saturated, a 10.0 mL aliqout was drawn. The amount of HCl used to reach the endpoint was 10.70 mL of 0.000560 M HCl. Considering their stoichiometry (2 moles of HCl react for every mole of dissolved oxalate), determine the amount of dissolved oxalate in the flask (in mol/L).
three solutions are mixed together to form a single solution ; in the final solution, there are 0.2 mol Pb(CH3COO)2, 0.1 mol NA2S and 0.1 mol CACL2 present. which solid(s) will precipitate?
3. how would the following errors affect the concentration of Cl- obtained in question 2b? give your reasoning in each case. a. the student read the molarity of AgNo3 as 0.02104M instead of 0.02014M b. the student was past the endpoint of titration when he took the final buret reading.