6. In hard water, [Ca2+] is about 2.0×103 M. Water is fluoridated with 1.0 g F per 1.0×103 L of water. Will CaF2(s) precipitate from hard water upon fluoridation? Show clear work to support your answer. (no)

What additional information do we need to answer the following question: How is the equilibrium of solid silver bromide with a saturated solution of its ions affected when the temperature is raised?

Suppose that the solubility of calcium iodate are 2.5 g/L at 20oC and 5.5 g/L at 60oC. What are the solubility in mol/L at 20oC and at 60oC? How many milliliters (mL) of 0.045 M Na2S2O3 will be required to titrate a 10.0-mL sample of saturated Ca(IO3)2 solution collected at 20oC and 60oC, respectively?

(a)  Will Mn(OH)2 precipitate from solution if the pH of a 0.050 M solution of MnCl2 is adjusted to 8.0?  (b) Will Ag2SO4 precipitate when 100 mL of 0.010 M AgNO3 is mixed with 20 mL of 5.0 x 10-2 M Na2SO4 solution?

As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl. A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely.     B(C6H5)4-+K+⟶KB(C6H5)4(s)     B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s) The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate. Find the mass percentages of NH4Cl and…

How many grams of precipitate will form when Na2SO4 reacts with 25 mL of 0.50 M Ba(NO3)2?

Iron (55.845 g/mol) can be determined gravimetrically by precipitation as Fe(OH)3 (106.867 g/mol) and subsequent inflammation of the precipitate to convert it to Fe2O3 (159.69 g/mol). A 0.7873 g sample to be analyzed was weighed and transferred to a 400 mL beaker, where it was dissolved in 50 mL of H2O and 10 mL of 6M HCl. Then 2 mL of concentrated HNO3 was added to the solution. After boiling to remove excess HNO3 and nitrogen oxides, the solution was diluted to 200 mL, brought to boiling, and Fe(OH)3 was precipitated by the slow addition of 1:1 NH4OH solution until an odor of NH3 was detected (indicating the presence of excess NH3 in the medium). The solution was left in a water bath at 80 ºC for 30 min at rest. The precipitate was then filtered and washed with several portions of hot 1% m/v NH4NO3 until no Cl– was detected in the wash water. Finally, the precipitate was ignited at 500-550 °C, then left in a desiccator to cool and weighed as Fe2O3, resulting in a mass of 0.4512 g.…

What pH is needed to precipitate Ni(OH)2 so completely that the nickel concentration is less than 1.1 x 10-5 M (Ksp = 1.6 x 10-14)? The answer is 9.58.

(i) Silver tarnishes in the presence of hydrogen sulfide (produced by rotten eggs) and oxygen because of the reaction below: 4Ag + 2H2S + O2 → 2Ag2S + 2H2O How many grams of Ag2S could be obtained from a mixture of 0.95 g Ag, 0.140 g H2S and 0.08 g O2 ? (ii) At 20°C the solubility limit of silver(I)sulfate (Ag2SO4) is 0.800 g/100 mL. What is the molarity of such a solution? (iii) What volume in mL of concentrated H2SO4 (18.0 M) must be used to prepare 400 mL of 3.0 M H2SO4 solution?

A solution contains 0.04500.0450 M Ca2+ and 0.09500.0950 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? -Ca3(PO4)2 -Ag3PO4 -Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution?