Sodium hypochlorite is the active ingredient in most household bleach products. One method of preparing this compound is as follows: Cl2(g) + 2N2OH(aq) → NaOCI (aq) + NaCl(aq) + H2O(1) In a certain experiment, 50.0 g chlorine was reacted with 50.0 g sodium hydroxide to yield 37.8 g sodium hypochlorite. (a) Calculate the theoretical yield (b) Calculate the percent yield.

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 cadmium chloride, which would react with silver nitrate solution like this: CdCl₂(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Cd(NO3)₂(aq) The chemist adds 75.0 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 7.0 mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. mg L

For each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced. CH4(9)+H₂O(g) → CO(g) + 3 H₂(g) Na₂CO3(s) + H₂PO4(aq) → Na₂HPO4(aq) + CO₂(g) + H₂O(1) 2H,S(aq)+O,(g) →2S(s)+2H,O) FeO(s)+CO(g) → Fe(s)+CO₂(g) Explanation reaction Check highlighted atom is being... oxidized O O O O reduced οιοιοιο O X neither oxidized nor reduced MacBook Air O O S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of U=

Classify each chemical reaction: Reaction Zn(s) + FeSO₂ (aq) → ZnSO₂ (aq) + Fe(s) CuSO₂ (aq) + ZnCrO₂ (aq) → ZnSO₂ (aq) + CuCrO₂ (s) - 2 Na(s) + Cl₂(g) → 2NaCl(s) 2H₂O₂(1)→ 2H₂O() + 0₂ (8) Type ✓ choose one combination decomposition single substitution double displacement none of the above choose one

Sodium carbonate, Na2CO3, is commonly used to neutralize acid spills in the laboratory. The neutralization of nitric acid is described by the UNBALANCED chemical equation HNO3 + Na2CO3 ➜ CO­2 (g) + H2O + NaNO3 How much Na2CO3 (molar mass: 105.99 g/mol) is required to neutralize 1.50 × 102 g of spilled nitric acid (molar mass: 63.01 g/mol)?   a.252 g Na2CO3 b.126 g Na2CO3 c.505 g Na2CO3 d.150 g Na2CO3

3 NaHCO3(aq) + H3C6H5O7(aq) → 3 CO2(g) + 3 H2O(l) + Na3C6H5O7(aq)   In a certain experiment 5.05 g of sodium bicarbonate and 4.50 g of citric acid are allowed to react. How many grams of carbon dioxide form?

Iodine is prepared both in the laboratory and commercially by adding Cl, (g) to an aqueous solution containing sodium iodide. 2 Nal(aq) + Cl,(g) I,(s) + 2 NaCI(aq) How many grams of sodium iodide, Nal, must be used to produce 89.9 g of iodine, I,? mass: g Nal

4. A student does a reaction that forms Pb(NO3)2 (ag). The student boils off some of the water in a beaker until Pb(NO3)2 (s) crystals form. The student vacuum filters this solution to collect the crystals. Since some of the crystals remain in the beaker, the student squirts water from their wash bottle in the beaker and pours this over the filter paper in the vacuum apparatus. When the student goes to collect the crystals from the paper they find that there is none there. Explair what happened and how it can be corrected.

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(II) chloride, which would react with silver nitrate solution like this:FeCl2(aq)+2AgNO3(aq)→2AgCl(s)+Fe(NO3)2(aq) The chemist adds 78.0mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 3.4mg of silver chloride.Calculate the concentration of iron(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. _________________mg/L

Honors Chemistry Chapter 9 Name/Date 3. Gold is very valuable because it does not oxidize easily. It can be oxidized by reacting it with nitric acid as shown below: Au(s) + 4H'(aq) + NO: (aq) → NO(g) + 2H:0(g) + Au³ (aq) 3a. If 30 grams of gold react with 3.4 grams of nitrate ion, which reactant is limiting?. 3b. What is the theoretical yield?. 4. Lead (II) nitrate reacts with sodium chloride according to the equation below: Pb(NO.): + NaCl → PbCla + NANO. 4a. If 8.3 grams of lead (II) nitrate react with 5 grams of sodium chloride, which material would be the limiting reactant? 4b. What is the theoretical yield?