Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' a. HCl(aq) + Hg₂(NO₃)₂(aq) →

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' d. aqueous ammonium chloride and aqueous calcium hydroxide

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' b. Cr(NO₃)₃(aq) + LiOH(aq) →

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' c. liquid pentanol (C₅H₁₂O) and gaseous oxygen

Hard water often contains dissolved Ca²⁺ and Mg²⁺ ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. A solution is 0.050 M in calcium chloride and 0.085 M in magnesium nitrate. What mass of sodium phosphate would you add to 1.5 L of this solution to completely eliminate the hard water ions? Assume complete reaction.

An acid solution is 0.100 M in HCl and 0.200 M in H₂SO₄. What volume of a 0.150 M KOH solution would completely neutralize all the acid in 500.0 mL of this solution?

Find the mass of barium metal (in grams) that must react with O₂ to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH^-.

A solution contains Cr³⁺ ions and Mg²⁺ ions. The addition of 1.00 L of 1.51 M NaF solution causes the complete precipitation of these ions as CrF₃(s) and MgF₂(s). The total mass of the precipitate is 49.6 g. Find the mass of Cr³⁺ in the original solution.

The nitrogen in sodium nitrate and in ammonium sulfate is available to plants as fertilizer. Which is the more economical source of nitrogen, a fertilizer containing 30.0% sodium nitrate by weight and costing $9.00 per 100 lb or one containing 20.0% ammonium sulfate by weight and costing $8.10 per 100 lb?

Find the volume of 0.110 M hydrochloric acid necessary to react completely with 1.52 g Al(OH)₃.

Treatment of gold metal with BrF₃ and KF produces Br₂ and KAuF₄, a salt of gold. Identify the oxidizing agent and the reducing agent in this reaction.

Treatment of gold metal with BrF₃ and KF produces Br₂ and KAuF₄, a salt of gold. Find the mass of the gold salt that forms when a 73.5-g mixture of equal masses of all three reactants is prepared.

A solution contains one or more of the following ions: Ag⁺ , Ca²⁺ , and Cu²⁺ . When you add sodium chloride to the solution, no precipitate forms. When you add sodium sulfate to the solution, a white precipitate forms. You filter off the precipitate and add sodium carbonate to the remaining solution, producing another precipitate. Write net ionic equations for the formation of each of the precipitates observed.

A solution contains one or more of the following ions: Hg₂²⁺ , Ba²⁺ , and Fe²⁺ . When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Which ions were present in the original solution?

A solution contains one or more of the following ions: Hg₂²⁺, Ba²⁺, and Fe²⁺. When you add potassium chloride to the solution, a precipitate forms. The precipitate is filtered off, and you add potassium sulfate to the remaining solution, producing no precipitate. When you add potassium carbonate to the remaining solution, a precipitate forms. Write net ionic equations for the formation of each of the precipitates observed.

The reaction of NH₃ and O2 forms NO and water. The NO can be used to convert P₄ to P₄O₆, forming N₂ in the process. The P₄O₆ can be treated with water to form H₃PO₃, which forms PH₃ and H₃PO₄ when heated. Find the mass of PH₃ that forms from the reaction of 1.00 g of NH₃.

An important reaction that takes place in a blast furnace during the production of iron is the formation of iron metal and CO₂ from Fe₂O₃ and CO. Determine the mass of Fe₂O₃ required to form 910 kg of iron. Determine the amount of CO₂ that forms in this process.

A liquid fuel mixture contains 30.35% hexane (C₆H₁₄), 15.85% heptane (C₇H₁₆), and the rest octane (C₈H₁₈). What maximum mass of carbon dioxide is produced by the complete combustion of 10.0 kg of this fuel mixture?

Titanium occurs in the magnetic mineral ilmenite (FeTiO₃), which is often found mixed with sand. The ilmenite can be separated from the sand with magnets. The titanium can then be extracted from the ilmenite by the following set of reactions: FeTiO₃(s) + 3 Cl₂(g) + 3 C(s) → 3 CO(g) + FeCl₂(s) + TiCl₄(g) TiCl₄(g) + 2 Mg(s) → 2 MgCl₂(l) + Ti(s) Suppose that an ilmenite–sand mixture contains 22.8% ilmenite by mass and that the first reaction is carried out with a 90.8% yield. If the second reaction is carried out with an 85.9% yield, what mass of titanium can be obtained from 1.00 kg of the ilmenite– sand mixture?