For each of the following balanced equations, write the oxidation number above the symbol of each atom that changes oxidation state in the course of the reaction. (a) N,O4(g) + KCI(s) → NOCI(g) + KNO3(s) (b) H,S(g) + 4 O̟F2(s) – (c) 2 POB13(s) + 3 Mg(s) → 2 PO(s) + 3 MgBr2(s) (d) 4 BCI3(g) + 3 SF4(g) · → SF,(g) + 2 HF(g) + 4 O2(g) 4 BF3(g) + 3 SCI2(t) + 3 Cl2(g)

3. Give the net ionic equation for the reaction (if any). that occurs when aqueous solutions of K2S and Fe(NO;)2 are mixed. A) K*(aq) + NO;(aq) – KNO;(s) B) No reaction occurs. C) Fe"(aq) + S³(aq) + 2 K^(aq) + 2 NO;(aq) → FeS(s) + 2 K“(aq) +2 NO;(aq) D) Fe"(aq) + S²(aq) + 2 K*(aq) + 2 NO;(aq) → Fe²"(aq) + s²(aq) + 2 KNO3(s) E) Fe2(aq) + S²-(aq) FeS(s)

Apply the concepts of stoichiometry and solution concentration in this section.  Potassium iodide reacts with lead (II) nitrate in the following precipitation reaction 2 KI (aq)  + Pb(NO3)2 (aq)       KNO3 (aq)    +  PbI2 (s). What volume of 0.200 M KI solution is required to completely precipitate all of the lead in 255mL of a 0.312 M Pb(NO3)2 solution?           An solution is made by dissolving 28.4 g of glucose (C6H12O6) in 355 g of water. The final volume of the solution is 378 mL. Calculate the molarity, molality, mole fraction, mole percent and mass percent of the solution,                          Hydrochloric acid is usually purchased in a concentrated form that is 37.0 % HCl by mass and has a density of 1.20 g/mL. Describe exactly how to prepare 2.85 L of a 0.500 M HCl to be used in Dr. Henary’s CHEM1211K lab from the concentrated solution. Hint (Find molarity of concentrated solution and use dilution equation. This is how your solution are prepared)

Which of the following reactions will produce a precipitate? Na₂SO4 (aq) + CuCl₂ (aq) → KF (aq) + AgNO3(aq) → Li₂CO3 (aq) + Mg(C₂H3O2)2 (aq) → Fe₂(SO4)3 (aq) + NH4ClO3 (aq) → AlCl3 (aq) + K3PO4 (aq) → Ba(ClO4)2 (aq) + (NH4)2S (aq) →

Calculate the molarity of the following solutions: (a) 0.14 mol of solute in 79.2 mL of solution (b) 2.99 mol of KBr in 0.46 L of solution (c) 27.5 g of NaC2H3O2 in 1.67 L of solution (d) 80 . g of CuSO4 · 5H2O in 8.5 L of solution

A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with 1.00 L of 4.00M NaCl (ag) in an Erlenmeyer flask. Both the AgNO3 (aq) solution and the NaCl(aq) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. What is the expected mass of AgCl (s), in grams, assuming that the yield is 100%? In the box, enter the mass to the nearest gram.

Calculate the molarity of the following solutions: (a) 0.85 mol of solute in 135 mL of solution (c) 260. g of C6H12O6 in 632 mL of solution (d) 128. g of MgSO4 · 7 H2O in 4.75 L of solution

2. The solubility of KClO, at several temperatures is shown in the accompanying diagram. Solubility, g per 100 g H₂O 50 40 30 20 10 10 20 30 40 50 60 70 80 90 Temperature, °C If a student mixes 10.0 g of KCIO, with 45.0 g of H₂O at 70 ° C. Which statement about the final solution is correct? (A) It is a saturated solution. (B) It is a supersaturated solution. (C) It is an unsaturated solution. (D) It is impossible to determine.

For each of the following reactions, suggest two soluble ionic compounds that, when mixed together in water, result in the net ionic equation given: (a) 2 Ag+ (aq) + CO3²¯ (aq) → Ag₂CO3(s) (b) Mg²+ (aq) + 2 OH¯(aq) → Mg(OH)₂(s), the suspension present in milk of magnesia 3+ (c) 3 Ca³+ (aq) + 2 PO2 (aq) → Ca3(PO4)2(s), gypsum, a component of concrete

The following equation represents the reaction that occurs when aqueous solutions of sodium hydroxide and magnesium acetate are combined. Mg(CH3COO)2(aq) + 2NaOH(aq) Mg(OH)2(s) + 2NaCH3COO(aq) Write a balanced net ionic equation for the reaction. Assume that all ionic compounds that are in aqueous solution are dissociated. Use the pull-down choices to specify states such as (aq) or (s). If a box is not needed leave it blank. ______ + ______ + ______ + ______ >>> ______ + ______