A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction occurs:                  K2SO4(aq) + Pb(NO3)2 (aq)    ⟶ 2 KNO3(aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 2.62 g.  Determine the percent yield.   1 mole PbSO4 = 303.26 g Group of answer choices A.) 69.5% B.) 120% C.) 91.1% D.) 80.1%

What is the molarity of ZnCl2 that forms when 25.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL . Zn(s)+CuCl2(aq)→ZnCl2(aq)+Cu(s) Part B: 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 0.055 M in calcium chloride and 0.095 M in magnesium nitrate. What mass of sodium phosphate would you add to 1.0 L of this solution to completely eliminate the hard water ions? Assume complete reaction. Express your answer using two significant figures   Part C: Enter an equation for the precipitation reaction that occurs (if any) when solutions of ammonium chloride and silver nitrate are mixed. Express your answer as a chemical equation. Identify all of the phases in your answer. Enter noreaction if no precipitate is formed.

In the laboratory you are given the task of separating Ca2+ and Fe2+ ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the lons, give the formula of the precipitate. If it cannot, type "No" Y or N 1. 12. 3 Reagent Formula of Precipitate if YES ка K₂SO4 Na CO

The balanced equation for the reaction of aqueous Pb(ClO3)2 with aqueous Nal is Pb(CIO,),(aq) +2Nal(aq) — Pbl,(s)+2NaClO,(aq) What mass of precipitate will form if 1.50 L of concentrated Pb(CIO3)2 is mixed with 0.500 L of 0.280 M Nal? Assume the reaction goes to completion. mass of precipitate: g

It is known that when mixed in solution aqueous, silver ions will react with chloride ions to form insoluble silver chloride. Upon dissolving a 5.000 g solid mixture of AgNO3 and KNO3 in a concentrated KCl solution, 1.582 grams of a white precipitate, AgCl(s), formed. Determine the percent, by weight, of AgNO3 in the original mixture.

2. Given that 0.0643 mol Mg(OH)2 (58.32 g/mol) are theoretically formed in the reaction: 2 NaOH (aq) + MgCl2 (aq)  2 NaCl (aq) + Mg(OH)2 (s) calculate the percent yield of Mg(OH)2 (s) if you weighted the product at the end of the experiment and your actual yield is 3.18g.

A 65.0 mL sample of a 0.110 M potassium sulfate solution is mixed with 36.5 mL of a 0.114 M lead(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 1.01 g . Determine the limiting reactant, the theoretical yield, and the percent yield.

9. What is the molarity (M) of a solution if 500 mL of the solution contains 40.85 g of NaHCO₁? 10. If 42.50 mL of a 1.100 M MgCl solution is needed to completely react with 45.0 mL of AgNO, solution, what is the molarity of the AgNO, solution? Hint: use example in Section 9.5 MgCl +2AgNO 2(aq) 3(aq) 2AgCl + Mg(NO3)2(aq) (s) 4

A 20.0 mL sample of 0.500 M Calcium nitrate solution, Ca(NO3)2(aq), is reacted with 80.0 mL of 0.200 M potassium iodate, KIO3(aq), and calcium iodate precipitate, Ca(IO3)2(s), is produced according to the following equation. Ca(NO3)2(aq) + 2KIO3(aq) -> Ca(IO3)2(s) + 2KNO3(aq) (a) Determine the limiting reactant.(b) How many grams of Ca(IO3)2 is expected to be produced? (c) If 2.90 g of Ca(IO3)2 was obtained, what is the percent yield?

Write a balanced equation to describe any precipitation reaction that should occur when the following substances are mixed. If no reaction occurs, then answer 1 for the coefficients and write NR for the products.  (a)   MgSO4(aq) +   BaCl2(aq) →     (b)   K2SO4(aq) +   MgCl2(aq) →     (c)   MgCl2(aq) +   Pb(NO3)2(aq) →