Where does a reaction occur between hydrochloric acid and sodium thiosulfate occur within real life?
Answers
What is the reaction that occurs between sodium thiosulphate and hydrochloric acid?
What is the reaction that occurs between sodium thiosulphate and hydrochloric acid?Hydrochloric acid solution is corrosive to eyes and skin. It is moderately toxic by ingestion and inhalation. Sodium thiosulfate solution is a body tissue irritant. The reaction of sodium thiosulfate and hydrochloric acid generates sulfur dioxide gas, which is a skin and eye irritant.
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Answer:
Explanation:
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.
Concepts
• Kinetics • Rate law
• Order of reaction • Concentration
Materials
Hydrochloric acid solution, HCl, 2 M, 25 mL Graduated cylinders, 10-mL, 5
Sodium thiosulfate solution, Na2S2O3, 0.15 M, 150 mL Overhead projector or light box
Distilled or deionized water Permanent marker
Beakers, 100-mL, 5 Stirring rods
Graduated cylinders, 50- or 100-mL, 2 Stopwatch or timer
Safety Precautions
Hydrochloric acid solution is corrosive to eyes and skin. It is moderately toxic by ingestion and inhalation. Sodium thiosulfate solution is
a body tissue irritant. 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 of all chemicals with eyes and skin. Wear chemical
splash goggles, temperature-resistant gloves, and chemical-resistant apron. Please review current Material Safety Data Sheets for
additional safety, handling, and disposal information.
Procedure
1. Label five 100-mL beakers 1–5 and clean the bottom of each beaker.
2. Draw a large “X” across the bottom on the outside of each beaker. Place the beakers on an overhead projector stage or
a light box so that students can view the “X.”
3. 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 1 2 3 4 5
0.15 M
Na2S2O3
50.0 mL 40.0 mL 30.0 mL 20.0 mL 10.0 mL
Distilled Water 0 mL 10.0 mL 20.0 mL 30.0 mL 40.0 mL
4. Have students calculate the final concentration of sodium thiosulfate in each beaker 1–5.
5. Record the following information in a data table: Beaker, volume of Na2S2O3 solution, volume of distilled water,
concentration of Na2S2O3, reaction time (sec), and 1/reaction time (reaction rate). See the Sample Data and Results
table in the Discussion section.
6. Measure 5.0 mL of 2 M hydrochloric acid into each of five 10-mL graduated cylinders.
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Rate of Reaction of Sodium Thiosulfate and Hydrochloric Acid continued