In the gravimetric analysis of iron, 12 tablets of iron supplement were completely dissolved and the iron was precipitated out as Fe203. If 0.25 g of Fe203 was obtained, how much Fe in milligrams is present in each tablet?

A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide to calcium oxide by heating. How many grams of calcium oxide should the student obtain if his solution contains 48.0 mL of 0.479 M calcium nitrate? g

A student determines the nickel content of a solution by first precipitating it as nickel hydroxide, and then decomposing the hydroxide to nickel oxide by heating. How many grams of nickel oxide should the student obtain if his solution contains 44.0 mL of 0.525 M nickel nitrate?

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200.mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl3 (aq) + 3AgNO3 (aq) →3AgCl (s) + (FeNO3)3 (aq) The chemist adds 48.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 7.5mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.

A sample of 8.51 g of solid calcium hydroxide is added to 35.0 mL of 0.480 M aqueous hydrochloric acid. Write the balanced chemical equation for the reaction. Physical states are optional. chemical equation: What is the limiting reactant? hydrochloric acid calcium hydroxide How many grams of salt are formed after the reaction is complete? mass of salt: How many grams of the excess reactant remain after the reaction is complete? excess reactant remaining: g

One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate, Suppose an EPA chemist tests a 200 mL sample of groundwater known to be contaminated with iron(III) chloride, which would react with silver nitrate solution like this: FeCl,(aq) + 3 AgNO,(aq) 3 AgCl(s) + Fe(NO₂),(ag) The chemist adds 21.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 3.3 mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. e -12 D.P C P

It is known that when mixed in solution aqueous, silver ions will react with chloride ions to form insoluble silver chloride. Upon dissolving a 5.000 g solid mixture of AgNO3 and KNO3 in a concentrated KCl solution, 1.582 grams of a white precipitate, AgCl(s), formed. Determine the percent, by weight, of AgNO3 in the original mixture.

You work as an intern at a drug testing facility. The head scientist asks you to prepare 50.0 milliliters (ml) of a 0.625 M (molar) solution of FeCl3 he needs for a Trinder spot test, used to detect salicylates. How many grams of solid FeCl3 will you need to make the solution?

Hydrobromic acid dissolves solid iron according to the following reaction: Fe(s)+2HBr(aq)→FeBr2(aq)+H2(g) A.) What mass of HBr (in g) would you need to dissolve a 2.6−g pure iron bar on a padlock? Express your answer using two significant figures.   B.)What mass of H2 would be produced by the complete reaction of the iron bar? Express your answer using two significant figures.