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Law of conservation of matter lab report.The chemical reaction used to research is: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

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Introduction

Law of Conservation of matter Aim: To design and perform a quick experiment to prove the Law of Conservation of matter. Research question: Does the mass of the reactants before the experiment is same as the mass of the product formed? Does the mass of the matter stays conserved during a chemical reaction as stated by the Law of Conservation of Mass? Background theory: Law of Conservation of matter states that matter can neither be created nor be destroyed. According to this, there must be no loss in mass and particle of reactants after any physical or chemical reaction. The chemical reaction used to research is: AgNO3(aq) + NaCl(aq) � AgCl(s) + NaNO3(aq) Hypothesis: We hypothesis that the total mass of the reactants would be equal to the mass of products formed. This is because according to the Law of conservations of mass, there must be no loss in the mass of reactants in any reaction. Therefore, no loss in the total mass of reactants would prove the Law of Conservation of matter. Variables: The independent variable is the mass of the reactants. The dependent variable is the product produced and it's mass. The controlled variables are the same reactants, same volumes and types of the containers (beakers or graduated funnel, etc), same analytical balance to weigh and the same concentration of the reactants. ...read more.

Middle

5. Weigh a beaker of 50 ml(wash properly and dry it) using a Analytical Balance, but don not remove it from the balance after weighing and tare the balance(set it to zero). 6. With a of pipette of 10mL (which is cleaned before with distilled water) measure out 5mL of Silver nitrate by looking at top of the line horizontally, at eye level and slowly to ensure that the bottom of the meniscus is on the line of the pipette. 7. Pour the measured out 10mL of Silver nitrate into the weighed beaker of 50mL (wash properly and dry it) 8. Pour the 5 ml of Sodium chloride solution into the beaker containing 5 ml of Silver nitrate. 9. Now weigh the product formed using Analytical Balance. Diagram: Observations: When two solutions are mixed together, the color changes to white and afterwards it changes to pink and the mixture become cloudy which shows that there are some solid particles in it. The color of the mixture gradually changes to pinkish purple. Data table: Table showing the mass of the Sodium Chloride solution in grams, mass of the Silver nitrate in grams, mass of the product formed in grams and the actual calculated mass of the product formed in grams during five trails of the reaction. ...read more.

Conclusion

The temperature and pressure was not controlled as it was assumed that the experiment is conducted at room temperature but there might be some changes in temperature and pressure which might have influenced. Realistic modification to the experiment that explicitly addresses the error(s)/weakness(s) that I identified: The beakers, graduated cylinders and pipettes used must be cleaned properly. The proper caution should be taken while weighing the product and insure that there is no loss of product while weighing it and insure that reading on measuring balance is zero before you weigh it. Practice dropping water with dropper while preparing solution and ensure that the bottom of the meniscus is on the line and look horizontally, at the eye level. While it is necessary to transfer the content into another flask with filter paper in order to filter it, and therefore some loss of product is unavoidable, I do not think that the procedure made it clear just what impact this could have on the results. Therefore, in the future I think that this error could be minimized by placing an explicit warning in the procedure and by using the only solution to this problem would be to ensure that the lid is on the crucible and to carry it as carefully as possible to prevent the loss of the product. ?? ?? ?? ?? Chemistry Lab Report Sukhjant Kaur ...read more.

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