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

Calcium Lab

Extracts from this document...


Jennifer Liu Block 2-1 Monday, December 13, 2010 Evelyn Korompai The Preparation of Calcium Carbonate from Calcium Carbonate It was found that when 2 g of calcium carbonate is reacted with hydrochloric acid, and then the aqueous product of that reacts with sodium carbonate, the same amount of calcium carbonate (2 g) should be produced. In other words, two chemical reactions, the first reaction containing calcium carbonate as the reactant, were conducted to produce a product of calcium carbonate in an aqueous solution. \ Purpose To use 2 g of calcium carbonate and, by using two reactions, produce a product of calcium carbonate and after the reaction, calculate the percent yield. Procedure Day 1: 1) Gather all equipment. 2) Weigh out approximately 2 g of calcium carbonate into a 250 mL beaker. Record the weight in the data table. 3) Weigh a piece of filter paper and record in in your table. ...read more.


fluid Table 3: Quantitative Observations after Reaction #1 Mass Na2CO3 2.01g Mass beaker and reaction 1 product 149.93g Table 4: Observations of Reaction #2 Quantitative Qualitative 0:01 seconds-0:20 seconds During the reaction, -The Na2CO3 rests in lump 1:00 minute After stirring, -Solution is more white in colour, yet still fluid Filtering, -Clear, solution, fluid coming out of filter -Solid/powder material rests on side of paper After filtering, -The powder on the filter paper is white and thick Table 5: Observations of the Product of Reaction #2 Quantitative Qualitative Mass of powder and paper: 3.26g -Chalky, soft, brittle -White powder Questions 1) What safety precautions were required for this experiment? Explain your reasoning. Although this experiment was not very dangerous, there were still some safety requirements. First of all, we put safety goggles to protect our face not necessarily from explosions, but to ensure our complete safety at all times, in case a substance, say, the product of hydrochloric acid and calcium carbonate were to go in our eyes. 2) ...read more.


While we filtered, there is a possibility that the filter paper could have ripped a little and this would have caused some of the solid to be filtered. As a result, the mass of calcium carbonate may be a little bit off. Other errors include the fact that not all reactants may have reacted due to some unknown random error and that not all reactants retrieved from the containers are 100% pure. Conclusion In this experiment, we learned how to calculate the percent yield by using the formulas of the reactions to first calculate the expected amount of product. When we reacted 2g of calcium carbonate, our result was 1.84 g. The expected yield was 2 g, and so we were both very close to the expected yield, as our percent yield for CaCO3 is 91%. In this experiment, we learned that it is not easy to get a high percent yield, and that exact measurements are crucial when conducting an experiment. To decrease the possibility of errors to the best of our ability, we must have the most exact measurements as possible. ...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. Calcium Carbonate and Hydrochloric Acid

    could be that some of the gas that is produced and is escaping, falls down again causing lower loss of weight at that moment. But as its only the 0,0828g reading that fits into that category it is unlikely to be the reason.

  2. Acids/Bases Design Lab. How does a change in the pH value of a solution ...

    The temperature of the hydrochloric acid solution should be at room temperature, as should the zinc metal strips being used in the investigation. The zinc metal strips, once exposed to the room temperature air, will adjust themselves to conform to the atmospheric temperature, and can do so as the investigator is setting up their materials.

  1. Chemistry Lab: Sodium Carbonate

    6. The calcium chloride solution was poured into the sodium carbonate solution. 7. The funnel was rested in a tall Erlenmeyer flask and the liquid was poured through into the filter paper which lined the inside of the funnel. This collected the solid.

  2. Rates of Reaction Lab

    3. Attach the other end of the delivery tube to a gas syringe and clamp it horizontally, making sure it doesn't oppose gravity. (Set apparatus should look like the diagram above) 4. Using an electronic balance, weigh out 0.2g of zinc dust in a piece of paper.

  1. Hydrogen Gas Collection Lab CE (6/6) A sample of solid magnesium ribbon, measuring approximately ...

    in = theoretical yield - experimental yield x 100 the reaction theoretical yield observed in the investigation = 0.0015 mol - 0.00156 mol x 100 between 6 mol dm-3 0.0015mol HCl(aq) and Mg(s) = 4% From the two calculations conducted, in regards to the percentage yield and percentage error of

  2. FInding the percentage purity of CACO3 in egg shell

    This was found by using the procedure of back titration.

  1. 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.

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

    = 0.9±0.1 Concentration of HCl = 1.66±0.1 Moles of CaCO3 = 0.045 ≈ 0.05 or 0.045±0.05 Mass of CaCO3 = 4.500 ≈ 5.0 or 4.50±0.1 Conclusion: The values obtained by me are completely based on the data recorded, but yes there were systematic and random error while calculating the values,

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