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The effect of Hydrocholric acid on the Rate of Reaction

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Introduction

The Effect of Hydrochloric Acid on the Rate of Reaction Aim: My aim is to see if there is any change in the rate of reaction if the concentration of the acid increases. Variables: The independent variable in the experiment is the concentration of the hydrochloric acid; the concentrations are 0.1, 0.2, 0.3, 0.4 and 0.5M. The dependent variable will be the rate of reaction of the acid. The control variable is the amount of the concentration, the temperature of the acid and the time that the zinc is inside the acid. Hypothesis: My prediction is that as the concentration of the acid increases the zinc will react more but not necessarily quicker. In order for any reaction to happen, the particles must first collide. ...read more.

Middle

Diagram: Equipment: Test tubes Hydrochloric Acid Zinc Measuring cylinder Thermometer Scale Results: Molarity (M) Weight of zinc before reaction (g) Weight of zinc after reaction (g) Difference in weight (g) 0.1 1.34 g 1.32 g 0.2g 0.2 1.9 g 1.86 g 0.4g 0.3 0.95 g 0.90 g 0.5g 0.4 1.31 g 1.25 g 0.6 g 0.4 1.01 g 0.95 g 0.6g Conclusion My conclusion is that as the concentration of the acid increases then the rate of reaction or the amount of mass lost increases. This indicates a direct correlation between the two variables. My explanation for this would be that zinc and hydrochloric acid react when they come in contact. The weight of the zinc decreases as it reacts to form zinc chloride, so there is less zinc leftover. ...read more.

Conclusion

Then I think if I had left the zinc in for longer then I could have obtained more significant results reducing the chance of any anomalies. In the time I was provided I did not have time to repeat the experiment and without equal pieces of zinc these repeats would not have been very effective. Again a better set of scales could have improved the accuracy of my measurements. Alternate experiments: I believe I could have changed the way I measured the rate of reaction by changing the experiment. Instead of measuring the zinc I could have measured the amount of hydrogen that was released in the reaction. I believe that if I had done this experiment my results would have been more accurate. ...read more.

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3 star(s)

This laboratory report is of a reasonable quality. It is limited by the lack of data collected. Improvements have been suggested throughout.

Marked by teacher Cornelia Bruce 17/04/2013

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