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

Determining the Percent Yield of Calcium Carbonate

Extracts from this document...

Introduction

Determining the Percent Yield of Calcium Carbonate Purpose: To compare the theoretical amount to the actual amount of calcium carbonate and calculate its percent yield in the reaction between solutions of sodium carbonate and calcium chloride. Materials: stirring rods fine filter paper 2 small beakers 0.8 - 1.2 g of sodium carbonate Erlenmeyer flask electronic balance graduated cylinder safety glasses 2 g of calcium chloride deionized water funnel retort stand ring clamp Safety Procedures: Sodium carbonate and calcium chloride are both harmful if swallowed or inhaled and may cause irritation to skin, eyes and respiratory tract. Safety goggles, and proper attire are to be worn at all times during this experiment. In particular, no loose clothing should be worn and long hair should be tied back. Procedure: 1. ...read more.

Middle

The filter paper was measured for mass. Results: Table 1: Masses of the Materials Material Mass (g) Filter Paper 1.77 Beaker 1 50.53 Beaker 1 with sodium carbonate 51.71 Beaker 2 101.46 Beaker 2 with calcium chloride 103.44 Filter paper with product 2.93 Table 2: Qualitative observations of the reagents before and after the reaction Course of time in the experiment Observations Before * sodium carbonate : white, powdery, odorless anhydrous salt that had a slower rate of dissolving in water and required extra water to completely dissolve; the solution was clear and transparent * calcium chloride: odouless white granules that dissolved easily in water; the solution was translucent During * as soon as the calcium chloride solution was poured into the sodium carbonate solution, a white, powdery precipitate was formed After * the residue in the filter paper was a white solid, powdery Calculations: Sample Calculation for determining ...read more.

Conclusion

Similarly, there are 1.11 � 10-2 moles of sodium carbonate in the experiment. NNa2CO3 < N CaCl2 Therefore, Na2CO3 is the limiting reactant. Number of moles of CaCO3 produced= Number of moles of Na2CO3 = 1.11 � 10-2 mol Mass of CaCO3= number of moles of CaCO3� molar mass of CaCO3 1 mol = 1.11 � 10-2 mol � 100.09 g 1 mol = 1.11 g Therefore, the theoretical mass of is CaCO3 1.11 g. Percent yield = experimental yield � 100% Theoretical yield = 1.16 � 0.02 g � 100% 1.11 g = 104.50 % Therefore, the percent yield is 104.50 %. Percent Error = | theoretical yield - experimental yield| � 100% theoretical yield = |1.11 g - 1.16 g| � 100% 1.11 g = 4.50% Therefore, the percent error in this experiment is 4.50%. ?? ?? ?? ?? - 1 - ...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. Lab 1 - Determining Hydrate Formulas

    Sulfate (ZnSO4) salt. Then by taking away the mass of water lost from the mass of the hydrated Zinc(II) Sulfate (ZnSO4) salt, I will be left with the dehydrated Zinc(II) Sulfate (ZnSO4) salt (which means just the salt without any water).

  2. Determining the mass of calcium carbonate obtained

    g mol ^-1 - 110.98 : 105.99 n = mass - 0.03604 : 0.056609 .

  1. The aim of the experiment is determining the percentage yield of the product (copper), ...

    HYPOTHESIS The assumed mass of copper is grams (theoretical yield), hence anything other than this explains that an error occurred during the experiment. If the actual mass of copper is within the range of grams, then the percentage yield is as close to 100% as possible and that the level of experimental errors is acceptable.

  2. Calculate % of caco3 in white egg shell

    Sometimes during the titration a bit extra phenolphthalein was added. This increased the error in the experiment even further. There were six reading taken and an individual count of all the samples was not taken but instead an average was taken.

  1. Aim: To estimate volumetrically the amount of Calcium carbonate present in the eggshell

    Systematic errors like parallax, random errors like taking readings and adding excess NaOH. On overall conclusion, the lab was set perfectly well with just a little bit of error, and nothing else, just there was a little bit mistake made by me when I was calculating the weight of watch

  2. FInding the percentage purity of CACO3 in egg shell

    Add two drops of phenolphthalein into the solution 28. Hold the tap with your left hand and the conical flask with your 29. Slowly open the tap of the burette and let the alkali flow into the conical flask.

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