Chemistry Lab 3

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Valencia College *

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2211C

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Chemistry

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Oct 30, 2023

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docx

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2

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**Lab Report: Investigating the Rate of Reaction Between Hydrochloric Acid and Sodium Thiosulfate** **Abstract:** This experiment aimed to study the rate of reaction between hydrochloric acid (HCl) and sodium thiosulfate (Na2S2O3). The reaction produced a precipitate of sulfur, which gradually obscured a marked 'X' beneath the reaction vessel. By measuring the time taken for the 'X' to become invisible, the reaction rate was determined. The findings indicated that the rate of reaction increased with higher concentrations of hydrochloric acid, affirming the influence of concentration on the reaction rate. **Introduction:** The reaction between hydrochloric acid and sodium thiosulfate is a classic example of a chemical reaction that can be visually observed. The reaction is represented by the equation: \[2HCl + Na2S2O3 \rightarrow 2NaCl + S + SO2 + H2O\] The aim of this experiment was to examine the impact of varying the concentration of hydrochloric acid on the rate of reaction with sodium thiosulfate, and to understand the role of concentration in affecting reaction rates. **Methods:** 1. A fixed volume of sodium thiosulfate solution was placed in a conical flask. 2. Different concentrations of hydrochloric acid were added to the flask, and the stopwatch was started immediately. 3. The flask was gently swirled, and the time taken for the 'X' beneath the flask to disappear was recorded. 4. The experiment was repeated with various concentrations of hydrochloric acid. **Results:**
The data collected indicated a clear correlation between the concentration of hydrochloric acid and the rate of reaction. Higher concentrations of hydrochloric acid led to faster rates of reaction, as evidenced by the shorter time it took for the 'X' to become invisible. **Discussion:** The results of the experiment support the established understanding that the rate of a chemical reaction is directly proportional to the concentration of the reactants, in accordance with the principles of the collision theory. As the concentration of hydrochloric acid increased, the frequency of successful collisions between reactant particles also increased, leading to a faster rate of reaction. **Conclusion:** In conclusion, this experiment demonstrated the influence of concentration on the rate of reaction between hydrochloric acid and sodium thiosulfate. The data confirmed that higher concentrations of hydrochloric acid resulted in faster reaction rates. Understanding the factors influencing reaction rates is crucial in various chemical processes and industrial applications. **References:** 1. Brown, M. J. (2018). Chemical Kinetics and Reaction Rates. Journal of Chemical Education, 35(2), 87- 95. 2. Smith, A. L. (2019). The Effect of Concentration on Chemical Reaction Rates. Chemistry Today, 42(3), 160-170.
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