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

Volume of a Drop Lab

Extracts from this document...


Title: HOW DENSITY AFFECTS VOLUME Intorduction: Disposable pipets are often used in micro scale experiments and it is often assumed that one drop is the same as the next drop, when, in fact, several variables are changing that could affect the size of the drop. It is important to be able to control temperature because surface tension of the drop of water decreases as the operating temperature increases and as the concentration increases. The increasing temperature would increase pressure and vice versa, therefore these variables have to be fixed because increasing the pressure would reduce the volume and decreasing the pressure would increase the volume if the volume is not fixed - as in the case of this experiment. The mass would have to be different for the different sets of experiments since we are trying to compare the densities of a drop of liquid in order to determine the effect that the density has on the volume. ...read more.


Weigh the mass of the empty container on the balance. Record its mass (to .001 g) 3. Pour about 2/3 of the 100 g liquid sample into the container. Record the combined mass of the liquid and container. Then get mass by difference to figure out the mass of the liquid sample. 4. Find the moles of liquid using molar mass 5. Transfer the sample into the disposable pipet and let it drop into a 100mL graduated cylinder 6. Using the Ideal Gas Law (PV=nRT), find the volume of this sample of liquid. P would be the pressure of the liquid, n would be the moles, R would be the constant of 0.0821mol(K)/L(atm), and T would be the temperature. FOR COLUMN B: 1. Record the temperature and pressure again to make sure these numbers are relatively the same as it was in the first set of procedures. 2. ...read more.


Instrumental limitations: A digital balance showing three decimal places can only weigh to within 0.0005 g by its very nature and even then only if it rounds the figures to those three places. Also, analogue devices such as thermometers or pipets and graduated cylinders often require the observer to interpolate between graduations on the scale. Some people will be better at this than others. Observing: For example, to measure the temperature of the liquid sample, you will dip a thermometer into it. This will inevitably cool the liquid slightly. The amount of cooling is unlikely to be a source of major error, but it is there nevertheless External Influences: The balance or other equipment may not be accurate and we also have to take in consider the impurity of the liquid sample. Sampling: Just these two sets of experimental procedures may not be enough to completely determine accurately the intended purpose for this experiment. Therefore, there may not be enough evidence to support the hypothesis. ...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. Research question - How many molecules are there in a liquid drop?

    The drops were all of the same sizes, and hence of the same volume. the volume was kept constant by using the same dropper for each trial, and furthermore, by applying the same pressure (from the fingers) to the bulb of the dropper.

  2. How does density of a liquid affect the volume of its drop

    Methodology 1. 1. Gather all the apparatus. 2. 2. Attach pipette pump to the glass pipette. 3. 3. Extract 25cm3 of the liquid using the pipette pump and glass pipette. 4. 4. Clamp the glass pipette onto the stand. 5.

  1. Energetics Design Lab

    This limitation cannot be fully avoided but can be easily improved. Realistic improvements to this limitation include: * Doing the reaction straight in a Styrofoam cup and not in the copper cup which was placed in the Styrofoam cup. Due to the fact that copper is an extremely bad insulator,

  2. Investigating the effect of different liquid densities on the time taken to release ...

    For instance, larger volume of the same alcohol sample certainly takes longer time to be released. * The temperature of each alcohol sample need to remain constant for every test at 20 oC (293 K). The analysis, written by Weirauch, D.

  1. The Drop of Water

    Using the pipette bulb, fill the 1ml pipette with exactly 1ml of water from the first beaker 4. Carefully remove the bulb and hold your finger over the top of the pipette to retain all of the water 5. Slowly wiggle your finger back and forth to release the water one drop at a time into the second beaker 6.

  2. chem design lab 2

    23. Wash the beaker completely in the same type of water that was used to fill the beaker for the first one. 24. Then repeat the steps 18-23 two more times for the 3 minute trial. 25. After doing 3 minute trial, then Measure about 20 ml of water with the graduated cylinder for 4 minute trial.

  1. Chemitry Lab - Molar Volume of a Gas

    * The temperature did not change in flask B;however, it cannot be stated for sure as it was only compared with the temperature of flask A. * The temperature in flask A rose very quickly as the reaction started * The amount of hydrogen produced from the reaction was large

  2. Calculating Density -How can you find the volume and density of two regular solids, ...

    Set the weights until the triple beam balance is balanced. 12. Find the mass of the object in grams. 13.

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