After the experiment, a student decides to dispose of their excess Mg safely by reacting it with acetic acid. If the student had 0.52 g of excess Mg metal, how many mL of 0.83 M acetic acid (HC₂H3O2)are required to fully react with the metal? Assume the reaction proceeds as below, and give your answer to 2 decimal places. Mg(s) + 2 HC2H3O2 (aq) → H₂ (9) + Mg(C₂H3O2)2 (aq)

After the experiment, a student decides to dispose of their excess Mg safely by reacting it with acetic acid. If the student had 0.52 g of excess Mg metal, how many mL of 0.83 M acetic acid (HC₂H3O2)are required to fully react with the metal? Assume the reaction proceeds as below, and give your answer to 2 decimal places. Mg(s) + 2 HC2H3O2 (aq) → H₂ (9) + Mg(C₂H3O2)2 (aq)

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

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+ (aq) + 2I- (aq) → PbI2 (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 45.0 g of Pb(NO3)2 (aq) to completely precipitate the lead?
Lead(II) ions can be precipitated out of solution through the following reaction: Pb(NO3)2 (aq) +2 NaOH (aq)→Pb(OH)2 (s) +2 NaNO3 (aq) What volume of a 3.50 M NaOH solution is required to completely react with 750. mL of 1.20 M Pb(NO3)2
Potassium iodide reacts with lead(II)(II) nitrate in the following precipitation reaction: 2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s)2KI(aq)+Pb(NO3)2(aq)→2KNO3(aq)+PbI2(s) What minimum volume of 0.218 MM potassium iodide solution is required to completely precipitate all of the lead in 145.0 mLmL of a 0.150 MM lead(II)(II) nitrate 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
Students in a chemistry lab are making the compound cobalt (II) carbonate. It can be made byreacting sodium carbonate solution with cobalt (II) chloride solution.Calculate the volume of 1.0 mol/L cobalt (II) chloride solution required to completely reactwith 250 mL of 1.5 mol/L sodium carbonate.Na2CO3 (aq) + CoCl2 (aq) → CoCO3 (s) + 2 NaCl (aq)
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 %
Consider the following precipitation reaction: 2 K3PO4 (aq) + 3 Co(NO3)2 (aq) → Co3(PO4)2 (s) + 6 KNO3 (aq) What volume of 0.222 M K3PO4 (aq) in milliliters is needed to react with 36.28 mL of 0.250 M Co(NO3)2 (aq)?
According to the following reaction, what volume (in mL ) of 1.24 M KCl solution is required to react exactly with 50.0 mL of 1.39 M Pb(NO3)2 solution?2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) Write your numerical answer without unit inside the box. The answer should be in three Significant figures and in standard not scientific notation.
A total of 10.0 g of potassium permanganate, an ionic compound with chemical formula KMnO4, is dissolved in water such that the final volume of the solution is 850 mL. What is [KMNO4] in that solution?
After the experiment, a student decides to dispose of their excess Mg safely by reacting it with acetic acid. If the student had 1.22 g of excess Mg metal, how many mL of 0.83 M acetic acid (HC₂H3O₂)are required to fully react with the metal? Assume the reaction proceeds as below, and give your answer to 2 decimal places. Mg(s) + 2 HC₂H3O₂ (aq) → H₂ (9) + Mg(C2H3O2)2 (aq)
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g) How much MnO2(s) should be added to excess HCl(aq) to obtain 225 mL Cl2(g) at 25 °C and 755 Torr?
Given the reactant side of the total ionic equation for the neutralization reaction of sodium hydroxide (NaOHNaOH) with hydrochloric acid (HClHCl), write the total ionic equation (also known as the complete ionic equation) by entering both the reactant and the product species, separated by the reaction arrow. Na+(aq)+OH−(aq)+H+(aq)+Cl−(aq)→ ?Na+(aq)+OH−(aq)+H+(aq)+Cl−(aq)→ ? Be sure to include the charges on the ionic species and the physical state of all the reactant and product species. Express your answer as a chemical equation.