• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

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

See related essaysSee related essays

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

    I have come to the conclusion that this is because the procedure was not followed 100 percent correctly. First of all, a different crucible was used the second trial because it was done on a different day. Because we were in a hurry we did not clean the crucible as properly as in the first trial.

  1. Aim: To find the molar mass of butane, by finding the number of moles ...

    each trial the pressure inside the burrrete can be estimated to be equal to the atmospheric pressure. From the graph, it has been calculated that the RMM of butane is 53.946�60.2% using the formulae 'RMM = mass/n' and 'pV= nRT'.

  2. hess's law

    sulphate obtained from the internet (source included in the bibliography at the end) was -134 KJ mol-1. Hence, the difference between the literature value and the calculated value = -3 KJ mol-1. Percentage difference between the two values = 2%.

  1. Determining the Molar Mass of Volatile Liquid

    89.9 x 100= 0.1 % Total uncertainty: 0.30% + 0.10% +0.1% = 0.50% Amount of volatile liquid = 1.14 x 10-2 � 0.50 % moles Calculation of the mass of the condensed gas: Mass of condensed gas= mass of flask with condensed vapor- mass of empty flask Mass of condensed

  2. Chemistry Internal Assesment - Stoichiometry (measuring 'x' in salt)

    masses in g a) salt 1,2+0,1g b) water 0,8+0,1g 2) masses in g * mol-1: a) salt 2 * Na + C + 3 * 0 = 46 + 12 + 48 = 106 b) water 2 * H + O = 2 + 16 = 18 3)

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

    Ready a Fisher Scientific Hot Plate by setting the knob to 10. This setting signifies approximately 250�C. This high temperature will increase the speed at which the reaction takes place, ensuring that this otherwise slow reaction is completed quickly.

  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)

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