To summarize Antoine Lavoisier’s contributions to modern chemistry in one sentence could most probably be “Lavoisier revolutionized chemistry with the balance”. It was him who, by systematic and intelligent usage….
Sodium Thiosulfate Reaction
Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid Rate Laws Introduction The purpose of this demonstration is to investigate the effect of sodium thiosulfate concentration on the rate of reaction of sodium thiosulfate with hydrochloric acid. The reaction, which produces solid sulfur, will be followed by measuring the time needed for the reaction mixture to become opaque. The results will be analyzed graphically to determine the order of reaction— the mathematical relationship between the reactant concentration and the rate. The reaction of sodium thiosulfate and hydrochloric acid generates sulfur dioxide gas, which is a skin and eye irritant. Perform this demonstration in a well-ventilated lab only. Avoid contact with all chemicals with eyes and skin. Wear chemical splash goggles, temperature-resistant gloves, and a chemical-resistant apron. Please review the current Material Safety Data Sheets for additional safety, handling, and disposal information.
Label five 100-mL beakers 1–5 and clean the bottom of each beaker.
Draw a large “X” across the bottom on the outside of each beaker. Place the beakers on an overhead projector stage or a lightbox so that students can view the “X. ”
Using separate graduated cylinders for the solution and water, measure and add the required amounts of 0. 15 M sodium thiosulfate and distilled water to each beaker. Be as precise as possible. Beaker 0. 15 M Na2S2O3 Distilled Water 1 50. 0 mL 0 mL 2 40. 0 mL 10. 0 mL 3 30. 0 mL 20. 0 mL 4 20. 0 mL 30. 0 mL 5 10. 0 mL 40. 0 mL
Have students calculate the final concentration of sodium thiosulfate in each beaker 1–5. 91860 011509 Flinn Scientific—Teaching Chemistry eLearning Video Series
Record the following information in a data table: Beaker, the volume of Na2S2O3 solution, the volume of distilled water, the concentration of Na2S2O3, reaction time (sec), and 1/reaction time (reaction rate). See the Sample Data and Results table in the Discussion section.
Measure 5. 0 mL of 2 M hydrochloric acid into each of five 10-mL graduated cylinders.
Starting with beaker #1, carefully add the HCl all in one pour to the sodium thiosulfate solution. Stir the solution once with a stirring rod and immediately start timing.
Stop timing when the black “X” is no longer visible. Record the reaction time in seconds in the data table. Repeat steps 7 and 8 with beakers 2–5. 10. Calculate 1/reaction time for each trial. Plot concentration vs. time and concentration vs. 1/time on separate graphs. Disposal Please consult your current Flinn Scientific Catalog/Reference Manual for general guidelines and specific procedures governing the disposal of laboratory waste. Collect the leftover reaction mixtures and filter to separate the solid sulfur product. The sulfur may be disposed of in a landfill according to Flinn Suggested Disposal Method #26a. The filtrate may be neutralized and disposed of down the drain with excess water according to
This activity may be performed as a chemical demonstration with classroom participation or as a student activity. The contents of the beakers project well on an overhead projector and the time to the disappearance of the black “X” is easily seen and measured. The reaction may be downsized for a student lab activity. Carry out individual trials in separate wells in a 6-well reaction plate or in small medicine cups. If students will be doing the experiment in the lab, it is a good idea for them to start with beaker #5, because it takes the longest time. The activity may also be performed as a cooperative class exercise with different groups investigating different variables, including the effect of HCl concentration and the effect of temperature. The reaction rate is zero-order with respect to HCl. Empty the beakers and clean them thoroughly using paper towels to remove the sulfur. If the colloidal sulfur is allowed to sit in the beakers for an extended time, it will be much more difficult to remove the deposits from the glass. To achieve better mixing of the reactants, add the hydrochloric acid using a 10-mL Luer-lock plastic syringe (without needle). Squirt the acid using a fair amount of force. When lower concentrations of sodium thiosulfate are used, the rate law does not appear to be as simple as predicted in this experiment. At lower concentrations, the reaction appears to be closer to 3/2-order in sodium thiosulfate and 1/2-order in hydrochloric acid. The reaction time is more difficult to measure at lower concentrations because the onset of turbidity is more gradual. • Both the overall chemical equation and the mechanism for the decomposition of sodium thiosulfate are more complex than suggested by Equation 1.
The reaction is acid-catalyzed, which means that the acid concentration must have some bearing on the rate in terms of producing an equilibrium concentration of HS2O3– ions, The HS2O3– ion is a reactive intermediate, reacting further with additional S2O32– ions to produce polymeric ions containing multiple S atoms. When the chain of S atoms in a polymeric ion becomes long enough, it “closes” in on itself to form a ring of elemental sulfur (S8). – — S2O32– + H+ < — > HS2O3 —— – H—S—SO3– + nS2O32– > H—S—(S)n—SO3 + nSO32– – — – – H—S—Sn—SO3 < — > H+ + S—Sn—SO3 —— – S—S7—SO3 > S8 + SO32– –2– © 2009 Flinn Scientific, Inc. All Rights Reserved. 91860 Discussion Sodium thiosulfate reacts with hydrochloric acid to form sulfur and sulfur dioxide (Equation 1). Na2S2O3(aq) + 2HCl(aq) > S(s) + SO2(g) + 2NaCl(aq) Equation 1 The kinetics of the reaction can be analyzed by graphing the concentration of Na2S2O3 as a function of both reaction time and 1/time. A plot of concentration versus time gives a curved line, which levels off as it approaches the x-axis—the reaction slows down as the reactant concentration decreases. The rate of a reaction is inversely proportional to reaction time. Flinn Scientific—Teaching Chemistry™ eLearning Video Series A video of the Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid activity, presented by Annis Hapkiewicz, is available in Rate Laws, part of the Flinn Scientific—Teaching Chemistry eLearning Video Series. Materials for Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid are available from Flinn Scientific, Inc. Materials required to perform this activity are available in the Reaction Order and Rate Laws—Student Laboratory Kit available from Flinn Scientific.