Lead ions can be precipitated from solution with KCl according to the reaction: Pb²+ (aq) + 2KCl(aq) → PbCl₂ (s) + 2K+ (aq) When 34.3 g KCl is added to a solution containing 25.8 g Pb2+, PbCl2 (s) forms. The solid is filtered and dried and found to have a mass of 30.9 g. theoretical yield of PbCl2 = 25.8 g Ph Part C % yield = X Determine the percent yield for the reaction. Express your answer in percent to three significant figures. ΠΫΠΙ ΑΣΦ 1 mol Pb2+ 1 mol 1 met X 207.2 g Pb²+ 2 ? %

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

Consider the following reaction H2S (g) + FeS(s) + CO2(g) →FeS2(s) + HCO2H(aq) If 2.00 g of each reactant is each dissolved in 250.0 mL of water and all the solutions are mixed together. The final volume was measured to be 750.0 mL.  a)How many grams of CO2 left unreacted?  b) What is the concentration of HCO2H in this solution?

Classify each chemical reaction: KOH(aq) + HBrO (aq) reaction K BrO (aq) + H₂O (1) Na Cl (aq) + AgNO3(aq) → NaNO3(aq) + Ag Cl (s) 16K (s) + S₂ (s)→ 8K₂S (s) 2CH₂CH₂CO₂H (1) + 70₂(g) → 6CO₂(g) + 6H₂O(g) ✓ 6 ✓ 7 type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition ✓8 X precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base 9 10

How many grams of Cu(OH)2 will precipitate when excess KOH solution is added to 41.0 mL of 0.618 M CuBr2 solution? CuBr2(aq) + 2KOH(aq) Cu(OH)2(s) + 2KBr(aq)g?

How many grams of Ag₂CO3 will precipitate when excess Na₂CO3 solution is added to 49.0 mL of 0.590 M AgNO3 solution? 2AgNO3(aq) + Na2CO3(aq) → Ag2 CO3(s) + 2NaNO3(aq) g

A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)₂(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.67 g PbCl₂ (s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)₂(aq) solution. concentration: M

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 89.0 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 5.4 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. E d OL E

250 mL of a 1.9 M Mg(OH)2 solution is added to a beaker.  How many moles of Mg(OH)2 were added?  How many grams of Mg(OH)2 were added?

The balanced chemical equation for the reaction between calcium hydroxide and hydrochloric acid is: Ca(OH)2 ( aq) + 2 HC1 ( aq )→ CaCl2 ( aq ) + 2 H,0 (1) We can interpret this to mean: 1 mole of calcium hydroxide and |mole(s) of hydrochloric acid React to produce: | mole(s) of calcium chloride and |mole(s) of water