Consider the following reaction. MgCl2 (aq) +2 NaOH(aq) - Mg(OH)2 (s) + 2 NaCl (aq) A 140.0 mL solution of 0.149 M MgCl, reacts with a 42.50 mL solution of 0.594 M NaOH to produce Mg(OH), and NaCl. Identify the limiting reactant. O NAOH O MgCl2 O NaCl O Mg(OH)2 Caclulate the mass of Mg(OH), that can be produced. mass of Mg(OH)2 : The actual mass of Mg(OH), isolated was 0.600 g. Calculate the percent yield of Mg(OH), percent yield:

Consider the following reaction. MgCl2 (aq) +2 NaOH(aq) - Mg(OH)2 (s) + 2 NaCl (aq) A 140.0 mL solution of 0.149 M MgCl, reacts with a 42.50 mL solution of 0.594 M NaOH to produce Mg(OH), and NaCl. Identify the limiting reactant. O NAOH O MgCl2 O NaCl O Mg(OH)2 Caclulate the mass of Mg(OH), that can be produced. mass of Mg(OH)2 : The actual mass of Mg(OH), isolated was 0.600 g. Calculate the percent yield of Mg(OH), percent yield:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M Na₃PO₄ reacts with 58.5 mL of 0.200 M CrCl₃ in the following chemical reaction? Na₃PO₄(aq) + CrCl₃(aq) → CrPO₄(s) + 3 NaCl(aq)
If 365 mL of 0.285 M MgCl₂ is added to 235 mL of 0.215 M (NH₄)₃PO₄, how many moles of Mg₃(PO₄)₂ precipitate will be formed? The balanced equation is 3 MgCl₂(aq) + 2 (NH₄)₃PO₄(aq) → Mg₃(PO₄)₂(s) + 6 NH₄Cl((aq)
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.
Two beakers sit on a balance; the total mass is 167.170 g. One beaker contains a solution ofKI; the other contains a solution of Pb(NO3)2. When the solution in one beaker is poured completely.into the other, the following reaction occurs:What is the total mass of the beakers and solutions after reaction? Explain completely?
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
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
Which of the following chemical reactions will produce a precipitate?
Consider the following reaction. MgCl2(aq) + 2 NaOH(aq) → Mg(OH)2(s) + 2 NaCl(aq) A 185.0 mL solution of 0.395 M MgCl2 reacts with a 37.62 mL solution of 0.811 M NaOH to produce Mg(OH)2 and NaCl. Identify the limiting reactant. ○ Mg(OH)2 NaOH MgCl2 NaCl Caclulate the mass of Mg(OH)2 that can be produced. mass of Mg(OH)2: The actual mass of Mg(OH)2 isolated was 0.742 g. Calculate the percent yield of Mg(OH)2. percent yield: 6.0 g %
Lead ions can be precipitated from solution with KC1 according to the following reaction: Pb²+ (aq) + 2 KCl(aq) → PbCl₂(s) + 2 K+ (aq) When 28.8 g KCl is added to a solution containing 25.5 g Pb²+, a PbCl₂ precipitate forms. The precipitate is filtered and dried and found to have a mass of 29.6 g. Part A Determine the limiting reactant. KCI Pb²+ Submit Part B m = Determine the theoretical yield of PbCl₂. Submit Part C Request Answer ΨΕ ΑΣΦ Submit Request Answer Determine the percent yield for the reaction. ΨΕ ΑΣΦ Request Answer BE ? ? % g
Imagine you are preparing a solution of NaCl and a solution of CaCl2. After you prepare them you go out to lunch with your colleagues. When you come back you cannot remember which solution is in which container because you forgot to label the containers before going to lunch. What experiments can you perform to identify each solution?
You have 6.79 mL of a 0.415 M aqueous solution of Sodium Bicarbonate (NaHCO3). You add all of this solution to a 50.00 mL volumetric flask and dilute with water. How many mL of the resulting solution should be used to make 71.3 mL of a 0.026 M solution?
What mass, in g, of AgCl is formed from the reaction of 50.0 mL of a 0.100 M AgC2H3O2 solution with 25.0 mL of 0.100 M MgCl2 solution? 2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq)