A solution of NaCl(aq)NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq)Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.05 g PbCl2(s)10.05 g PbCl2(s) is obtained from 200.0 mL200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq)Pb(NO3)2(aq) solution

A 57.0 mL sample of a 0.118 M potassium sulfate solution is mixed with 38.0 mL of a 0.122 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.

A 26.6 mLmL sample of a 1.48 M potassium chloride solution is mixed with 15.0 mL of a 0.860 M lead(II) nitrate solution and this precipitation reaction occurs: 2KCl(aq)+Pb(NO3)2(aq)→PbCl2(s)+2KNO3(aq) The solid PbCl2 is collected, dried, and found to have a mass of 2.62 g. Determine the limiting reactant, the theoretical yield, and the percent yield.

A 30.00 mL sample of an aqueous solution of CaI2 reacts with excess NaOH according to the following reaction: 2NaOH(aq) + CaI2(aq) ---> Ca(OH)2(s) + 2NaI(aq) If the mass of the precipitate is 0.489g, what is the concentration of the CaI2 solution?

9 mL of a 1.25 M solution of CaCl2(aq) is reacted with 125.0 mL of 0.17M  solution of Na3PO4(aq) Given the reaction : 2Na3PO4(aq) + 3CaCl2(aq) → Ca3(PO4)2 (s)+6NaCl(aq) Determine the mass of the precipitate Ca3(PO4)2 formed Determine the concentration in mol/L of NaCl in the solution after the reaction has occurred Determine the concentration in mol/L of Na3PO4 in the solution after the reaction has occurred Determine the concentration in mol/L of CaCl2 in the solution after the reaction has occurred

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg .   Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5

A solution of NaCl(aq)NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq)Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.41 g PbCl2(s)10.41 g PbCl2(s) is obtained from 200.0 mL200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq)Pb(NO3)2(aq) solution.

copper (II) ion is precipitated from solution by adding 3.00 M NaOH(aq) resulting in a blue precipitate. What volume in milliliters would be necessary to fully precipitate the copper (II) ion from 100.0 mL of a 0.288 M solution of copper (II) nitrate.

A 25.00 mL sample of boric acid requires 32.57 mL of 0.2514 M NaOH to reach the endpoint of titration. H3BO3 (aq) + 3 NaOH (aq) → Na3BO3 (aq)   + 3 H2O (l) Determine the concentration of boric acid in the sample. Write the full and net ionic equation for the reaction.