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AIM: To verify that mass-mass relationships hold by measuring the amount of NaCl produced.

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Introduction

Ilyas Shaikh IBDP -1 MASS-MASS RELATIONASHIPS AIM: To verify that mass-mass relationships hold by measuring the amount of NaCl produced. HYPOTHESIS: The fundamental law of chemical reactions is the Law of Mass Conservation (or Conservation of Mass). The law states that the total mass of reactants must equal the total mass of products for a chemical reaction. EXPERIMENTAL SETUP AND BACKGROUND: 1. To perform a reaction using measured samples of reactants 2. To measure the mass of the products; 3. To note the mass - mass relationships for this reaction. APPARATUS REQUIRED: 250 cm3 beaker Bunsen burner Graduated cylinder Safety glasses Spatula MATERIALS REQUIRED: Solid Na2CO3 1. M HCl solution PROCEDURE: 1. ...read more.

Middle

9. Finally, I computed the expected mass of NaCl produced using a mass-mass problem calculation. 10. I repeated the same process respectively with 4g and 5g of the carbonate. CALCULATIONS AND DATA PRESENTATION: Mass of the empty beaker/g Trial1 Trial2 Trial3 109.10 110.50 111.40 Mass of the beaker with Na2CO3 /g 112.10 114.50 116.40 Mass of Na2CO3 /g 3.00 4.00 5.00 Molar mass of Na2CO3 /g mol-1 0.03 0.04 0.05 Moles of HCl required to consume the Na2CO3 0.06 0.08 0.10 Volume of HCl required /cm3 560.00 750.00 940.00 Mass of the dry beaker and product NaCl /g 112.49 114.50g 117.12 Mass of NaCl recovered /g 3.39 4.50g 5.72 Expected mass of NaCl /g 3.50 4.68 5.85 Percent error /% 3.24 4.00 2.27 Molar mass (Na2CO3) = (23x2+12+16x3) =106 g mol-1 No. ...read more.

Conclusion

After placing the heated saturated solution in the hot air oven for 2 hours, white crystals of sodium chloride were visible in the beaker. CONCLUSION: I compared my results with expected amount and calculated the percent error for all three experiments Trial 1 Percentage error =3.24% Trial 2 = 4.00% Trial 3 = 2.27% EVALUATION: The resulting percentage errors would be due to the following experimental errors: 1. Inaccurate measurements of reactants- this could have been prevented by taking an average of the number of readings taken and using the most appropriate apparatus for measuring the reactants. 2. Splashing of the salt solution while heating- this case too can be prevented by using a lid to cover the beaker. ...read more.

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