In an aqueous medium, 2.92 g of NaCl (molar mass 58.44 g/mol) reacted with 10.49 g of AgNO3 (molar mass 169.87 g/mol) to produce 6.16 g AgCl (molar mass 143.32 g/mol) which is insoluble in the medium along with 4.25 g of NaNO3 (molar mass 84.99 g/mol). What are the theoretical yield and % w/w yield AgCl, respectively?

40.00 mL of a solution of MgCl2 with a molar volume concentration of 0.933 mol/L is mixed with 100.0 mL of a solution of AlCl3 with a molar volume concentration of 0.211 mol/L.  What is the final molar volume concentration of chloride ions (Cl-) in the mixture in mol/L? Note: The density of pure water is 1.000 g/mL.

Mining companies use this reaction to obtain iron from iron ore: Fe₂O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) The reaction of 167 g Fe₂O3 with 85.8 g CO produces 72.3 g Fe. Determine the limiting reactant, theoretical yield, and percent yield. What volume (in mL) of 0.200 M NaOH do we need to titrate 35.00 mL of 0.140 M HBr to the equivalence point?

You are given a solid that is a mixture of Na2SO4 and K₂SO4. A 0.205g sample of the mixture is dissolved in water. An excess of an aqueous solution of BaCl₂ is added. The BaSO4 that is formed is filtered, dried, and weighed. Its mass is 0.298g. What are the percent compositions by mass of Na₂SO4 and K₂SO4 in the sample?

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.

You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First  you  extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2 and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After  decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2.   Calculate the percent Mg(OH)2 in the original sample mixture.

You are asked to determine the percentage of the components of a mixture containing sodium iodide, NaI, magnesium hydroxide, Mg(OH)2, and barium sulfate, BaSO4. The total mass of your mixture sample is 4.82g. First  you  extracted the NaI from the mixture with water and filtered insoluble Mg(OH)2 and BaSO4 from the solution, containing the NaI. After evaporating and drying the filtrate, you find that you have recovered 0.95g of NaI. When you react the insoluble residue of Mg(OH)2 and BaSO4 with 3M HCl, the Mg(OH)2 dissolves. After  decanting the supernatant liquid containing aqueous MgCl2 from the insoluble BaSO4 and drying the solid, you recover 2.04g of BaSO4. Finally you add 3M KOH solution to the aqueous solution to precipitate the Mg(OH)2. After filtering thesolution and drying the precipitate, you recovered 1.21g of Mg(OH)2.

50.0 mL of a 0.4230 M solution of Na3PO, was mixed with 100.0 mL of 0.5151 M HgNO3 and allowed to react: Na3PO4 (aq) + HgNO3(aq) → 3 NaNO3(aq) + Hg3PO4 (s) - Answer the following questions: What mass of precipitate was formed? What is the molarity of the unreacted reactant after the reaction is complete? Check 9 M

8. Sodium thiosulfate, Na2S₂O3, is an important reagent for titrations. Its solutions can be standardized by titrating the iodine released when a weighed amount of potassium hydrogen iodate, KH(IO3)2 (389.912 g/mol), is allowed to react with excess potassium iodide in acidic solutions. The net ionic equations are: production of iodine from KH(IO3)2: IO3¯¯ +5 I¯¯+ 6H* → 3 1₂ + 3 H₂O 1₂+2 S₂03² → 2 I¯+S406²- 2- titration of iodine: What is the molarity of a sodium thiosulfate solution if 39.66 mL are required to titrate the iodine released from 0.1022 g of KH(IO3)2?

F12 F11 ID: A Date: Class: ID: A 24. 6. The amount of calcium present in milk can be determined by adding oxalate to a sample and measuring the mass of calcium oxalate precipitated. What is the mass percent of calcium if 0.429 g of calcium oxalate forms in a 125-g sample of milk when excess aqueous sodium oxalate is added? Na,C2O4(aq) + Ca²*(aq) → CaC2O4(s) + 2Na*(aq) a. 0.107% b. 0.202% с. 0.343% d. 1.10% е. 1.37% 25. Identify all the spectator ions in the following reaction. KSO4(aq) + 2MNSO4(aq) + 5FE2(SO4)3(aq)