3. FeCl3 reacts with AgNO3 in aqueous solutions to produce a precipitate of AgCl that can be filtered and weighed. The balanced equation for the reaction is: FeCl3 (aq) +3 AgNO3 (aq) → 3 AgCl (s) + Fe(NO3)3 (aq) Suppose you have a mixture that contains FeCl3, plus other compounds that do not react with AgNO3. If 0.3291 g of the mixture yields 0.5571 g of AgCl, what is the percentage of FeCl3 in the mixture? Molar masses: FeCl3 162.21 g/mol AgCl 143.32 g/mol

A quality control technician needs to determine the percentage Arsenic (As) in particular pesticide.The pesticide is dissolved and all of the arsenic present is converted to arsenate ions (AsO43-). Then the amount of AsO43- is determined by titrating with a solution containing silver ions (Ag+). The silver reacts with the arsenate according to the net ionic equations: 3 Ag+ + AsO43- → Ag3AsO4 When a 1.22 g sample of pesticide was analyzed this way, it required 25.0 mL of 0.102 M Ag+ solution to precipitate all of the AsO43-. What was the mass percentage of arsenic in the pesticide?

Using the balanced equation: FeCl3(aq) + 3 NaOH (aq) ------> FeOH3 (s) + 3 NaCl (aq), determine the mass of solid product that can be made by starting with 14.0 grams of iron (III) chloride and 9.0 grams of sodium hydroxide.

What is the molarity of a hydrchloric acid, HCl, solution if it takes 26.90 mL of acid to neutralize 7.77 g of Fe(OH)3? The molar mass of Fe(OH)3 is 106.87 g/mol and the molar mass of HCl is 36.46 g/mol. The balanced chemical reaction is: 3 HCl (aq)   +   Fe(OH)3 (aq)   →   FeCl3 (aq)   +   3 H2O (l)

Balance the molecular equations for the following reactions between aqueous solutions. You will need to decide on the formulas and states of the products in each of the cases. CaCl2 (aq) + Pb(OH)2 (aq) → H2SO4 (aq) + Ba(OH)2 (aq) - AGNO3 (aq) + KCI (aq) – HCIO4 (aq) + Ca(OH)2 (aq) -

Which of the following chemical reactions will produce a precipitate?

Choose balanced molecular, ionic, and net ionic equations for the reaction of hydrochloric acid with strontium and gallium. (Both are oxidized by hydrogen ions.)   1. Molecular equation for the reaction of hydrochloric acid with strontium a. Sr (s) + 2HCl(aq) →  Sr Cl2(aq) + H2(g) b. Sr (s) + 2HCl(aq) →  Sr Cl2(aq) + H2(g) + H2O c. Sr (s) + 2H+(aq) →  Sr 2+(aq) + H2(g) d. Sr (s) + 2H+(aq) + 2Cl–(aq) →  Sr 2+(aq) + 2Cl–(aq) + H2(g) 2. Ionic equation for the reaction of hydrochloric acid with strontium a. Sr (s) + 2HCl(aq) →  Sr Cl2(aq) + H2(g) b. Sr (s) + 2H+(aq) →  Sr 2+(aq) + H2(g) c. Sr (s) + 2H+(aq) + 2Cl–(aq) →  Sr 2+(aq) + 2Cl–(aq) + H2(g) d. Sr (s) + 2HCl(aq) →  Sr Cl2(aq) + H2(g) + H2O   3. Net ionic equations for the reaction of hydrochloric acid with strontium a. Sr (s) + 2H+(aq) →  Sr 2+(aq) + H2(g) b. Sr (s) + 2HCl(aq) →  Sr Cl2(aq) + H2(g) c. Sr (s) + 2H+(aq) + 2Cl–(aq) →  Sr 2+(aq) + 2Cl–(aq) + H2(g) d. Sr (s) + 2HCl(aq) →  Sr Cl2(aq) + H2(g) + H2O 4.…

Sodium bicarbonate reacts with hydrochloric acid in a gas-forming reaction to produce aqueous sodium chloride, water, and carbon dioxide gas NaHCO3(s) + HCl(aq)→NaCl(aq) + H2O(l) + CO2(g) Determine the mass of CO2 gas produced when 8.89 g of NaHCO3 is added to a solution that contains 5.15 g of HCl.

1. A student was asked to react silver nitrate with sodium during a stoichiometry lab. The student react 12.3 g of silver nitrate with 7.83 g of sodium sulfate to produce the following products.  Na2SO4(aq) + 2 AgNO3 (aq) -> Ag2SO4(s) + 2 NaNO3(aq) a) predict the mass of percipitate that the student should obtain.

What mass of precipitate (in g) is formed when 69.0 mL of 0.500 M FeCl3 reacts with excess AgNO3 in the following chemical reaction? FeCl3(aq)+ 3 AgNO3(ag) ———> 3 AgCl(s) + Fe(NO3)3(aq)