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I cant figure out what i am suppose to do for this assignement that we are to do. it says to apply each lab that we have done in the class to our career . for example the lab on osmossis and diffusion how would i make three applications for that lab?

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Hi there!
<br><br>From your question it sounds like you need to learn about some applications of diffusion and osmosis to complement a lab you have done on these two processes. I will go over these two concepts separately, first briefly reviewing the main concepts, then will get into the applications of each. For your lab, I would recommend explaining these (or other) applications of osmosis and diffusion in your own words. It would also be helpful to construct diagrams to demonstrate the processes.
<br><br>Is the general process of the movement of molecules from a high concentration to a low concentration. This is due to the random motions and kinetic energy of the molecules. They will tend to spread out evenly, until the concentration is even. You can easily visualize this process when you think of dropping a drop of dye or food coloring into a glass of water. At first the dye is concentrated to the spot where it was added. Soon the dye spreads out evenly throughout the entire glass producing a uniform color. I have attached a diagram labeled "figure 1" that demonstrates this process.
<br><br>Osmosis is a specialized form of diffusion, it is a type of diffusion. It deals specifically with the movement of water molecules across a concentration gradient. I am guessing that you may have done an experiment with two solutions (a hyper and hypo tonic one) and seen the water diffuse across a membrane. Here it is demonstrated that ...

See Also This Related BrainMass Solution

Lab : Gases, Pressure and Stoichiometry

Add 0.5g of sodium bicarbonate, NaHCO3 into a flask. Record the initial pressure and temperature in the flask. Add 10 mL of water to the flask to dissolve the NaHCO3 then record the pressure as the initial pressure for the experiment. Record the gas volume as the initial volume. Add 1 mL of 1M HCl, allow the temperature in the flask to return to room temperature, and then record the pressure in the flask. Continue to add 1 mL increments of HCl solution. (observe whether a reaction has occurred).

These are the initial conditions of the closed flask with just the sodium carbonate inside. Assume that the sodium bicarbonate powder takes up a negligible volume in the flask.
(a) Initial pressure (atm): 1.072 atm
(b) Initial gas volume (mL): 139.72 mL
(c) Initial temperature (C): 21C
These are the final conditions of the closed flask:
(a) Final pressure (atm): 2.405 atm
(b) Final gas volume (mL): 131.92mL
(c) Final temperature (C): 21 C

1. Use the initial conditions and the ideal gas law to calculate the number of moles of air molecules (N2, O2, etc.) trapped in the flask. The gas constant, R = 0.082057 (L*atm)/(K*mole), so make sure to convert your temperature value to Kelvin.

2. The final conditions represent the air and CO2 from the reaction held in a smaller volume than at the start. Calculate the total moles of air and CO2 molecules from the ideal gas law, using the final conditions of pressure, volume and temperature. Record the total moles here.

3. Subtract the moles of air (from the initial conditions) from the total moles of gas at the end to find the moles of CO2 produced by the reaction.Record the moles of CO2 gas produced by the reaction:

4. You now have enough information to balance the equation: NaHCO3(s) + HCl(aq) --> CO2(g) + H2O(l) + NaCl(aq)
Calculate the following:
(a) Moles of NaHCO3 added to the flask (MW=84.007 g/mol):
(b) Moles of CO2 produced
(c) The ratio of (moles of CO2) divided by (moles of NaHCO3)
(d) What is the nearest whole number ratio for your experimentally-determined ratio? For example, if the experimental ratio is 1.75, then you would use a whole number ratio of 2 to 1. If the experimental ratio is 3.2, then you would use a whole number ratio of 3 to 1.
(e) Use the whole number ratio to balance the equation for the reaction. If your whole number ration is 2 to 1, then place a 2 next to the CO2 and a 1 next to the NaHCO3. Continue from there to balance the number of atoms on each side of the equation. Write the balanced equation here:
(f) Calculate the experimental error from the difference between the experimental ratio and the whole number ratio as follows:
% error = |real ratio - whole number ratio| / (whole number ratio) * 100%

5. (a) Could you boil off the liquid at the end of the experiment and weigh the NaCl left in the flask in order to balance the equation?
(b) Air usually contains water vapor. The air trapped in the flask was dry air with no water vapor. How would the presence of water vapor affect your calculations?
(c) Carbon dioxide is slightly soluble in water and its solubility increases with increasing pressure. How would the fact that some of the carbon dioxide produced by the reaction is dissolved in the aqueous solution affect your calculations?

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