• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2
3. 3
3
4. 4
4
5. 5
5
6. 6
6

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

Extracts from this document...

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.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

## Found what you're looking for?

• Start learning 29% faster today
• 150,000+ documents available
• Just £6.99 a month

Not the one? Search for your essay title...
• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month

# Related International Baccalaureate Chemistry essays

1. ## Our aim in this experiment to measure the heats of reaction for three related ...

for trial3. CALCULATIONS FOR REACTION 1 H2O used: 50ml(±0,1) mass of average NaOH used: 0,6(±0,01) Mass of solution : 50,0g(±?0,2)HCL+0,6(±?1,6)NaOH=50,6g(±?1,8) Initial temperature of HCL solution:23C(r)(±0,1) Final temperature of solution:26(r)(±0,1) ?t=26(r)(±?0,04) - 23 C(r)(±?0,04)=3(±?0,1) Final temperature of solution:27,5C(r)(±0,1) ?t=27,5C(r)(±?0,04) - 23 C(r)(±?0,04)=4,5(±?0,1) Final temperature of solution:23,5(r)(±0,1)

2. ## Can one determine the coefficients of a balanced chemical equation by having the mass ...

Ensure that step 3 is repeated so that precision of the experiment is being up-kept. Record all this data in "Data Table 2 - Quantitative Data Table" under "Mass of Filter Paper(�0.01g)" . All these materials are required to filter the copper metal out of the aluminum chloride solution. 15.

1. ## Stoichiometry Lab Report. Aim: To determine what solid product is produced in the ...

Using the more precise scale will also help. * You have to keep the crucible controlled because they often have impurities left behind in the crucible. If you have that for one trial, you have to keep it the same for the second trial.

2. ## Our aim in this experiment to measure the heats of reaction for three related ...

for trial3. CALCULATIONS FOR REACTION 1 H2O used: 50ml(�0,1) mass of average NaOH used: 0,6(�0,01) Mass of solution : 50,0g(�?0,2)HCL+0,6(�?1,6)NaOH=50,6g(�?1,8) Initial temperature of HCL solution:23C(r)(�0,1) Final temperature of solution:26(r)(�0,1) ?t=26(r)(�?0,04) - 23 C(r)(�?0,04)=3(�?0,1) Final temperature of solution:27,5C(r)(�0,1) ?t=27,5C(r)(�?0,04) - 23 C(r)(�?0,04)=4,5(�?0,1) Final temperature of solution:23,5(r)(�0,1)

1. ## Determining the Molar Mass of Volatile Liquid

The Erlenmeyer flask was dried completely 9) The mass of the Erlenmeyer flask with the boiling stone, aluminum foil cap and condensed vapor was weighed and recorded accurately on the electronic balance to the nearest 0.001g 10)

2. ## Mass-Mass Relationships

Since the HCl contains 1.0 mole per liter. 4. Then, add 10% to the calculated amount in order for the HCl to be in excess 5. Measure out the final amount of HCl in a graduated cylinder 6. Pour the acid slowly into the beaker containing the solid sodium carbonate and record any observations 7.

1. ## Investigation of reversible reactions at equilibrium - CuCl2 (s) was added to HCl , ...

Hence according to Le chatelier?s principle i.e. when a system under equilibrium is stressed the system moves in order to minimize the stress . The position of the equilibrium in the equation above shifts to the left in order to counter the increase in the concentration of the Cl- .

2. ## Research question: how to convert NaOH to NaCl by two different routes , and ...

From graph (1) highest temperature could be determined to be 35.0ËC Calculations : uncertainties Percentage uncertainty Mass of water 50.0g 1.0% Temperature 1. º C ( for original temperature) 0.1 º C ( for final temperature) 0.36 % Number of moles (NaOH)

• Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to
improve your own work