kg 0.29367OsmkgH2O=0.226gM*9.876*10-3kg solvent 0.29367OsmkgH2O=22.88 gM*kgH2O M=22.880.29367 M=77.91gmol Based on the molar mass of calculated‚ the identity of the unknown substance D is Glycine. 2) Finding the concentration of a known solution Table 1.2: Table used for the preparation of the calibration curve used to find the concentration of alcohol in a wine. 0.2mL of each sample were taken and placed in the Osometer. Ethanol sample (g EtOH/100mL) | Osmolality (mOsm/kg H2O) | 5
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tablespoons * Green - 8 tablespoons 3. Label each cup with the amount of sugar added. 4. Stir the water until the sugar is dissolved. It is crutial that all of the sugar is dissolved in each cup. You may need to supersaturate the sugar water solution to get all of the sugar to dissolve. Place the cup in the microwave for 20-30 seconds to warm the water and dissolve more sugar. Continue stirring until all of the sugar is gone. 5. Start with the cup with the most sugar. Using a pipette‚ dropper
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of succinate broken down by the mitochondrial solution. We detected the amount of DPIP in the solution with a spectrophotometer and measuring the absorbance of light at the 600nm range. DPIP is a useful chemical to use in this experiment because it goes from a blue color when oxidized to a colorless liquid (Ogura‚ 281)‚ this is due to the hydrogen ions and electrons released during the transitional step between succinate and fumarate. The three solutions used contained the same amount of mitochondrial
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variable will be the sucrose concentration of water. This is controlled by using a specific amount of sugar that we pour into the distilled water. We will do the activity in the solutions with concentration of 0‚ 0.25‚ 0.50%. Dependent Variable The dependent variable will be the size of potato slices that goes into the solutions. This depends on the various environmental factors during making a slice of potato such as the thickness of core or the peel of potato. Thus it could differ during the experiment
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Purpose: Our purpose here to determine the affects of temperature on potassium nitrate’s solubility in water. Materials Used in the Experiment: Latex gloves Laboratory coat Safety goggles Thermometer Stir rod Test tubes Beaker Weighing dish Hot plate Potassium nitrate Distilled water Description of the Object of the Experiment Potassium Nitrate: The chemical compound potassium nitrate is a naturally occurring mineral source of nitrogen. It is a nitrate with chemical
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To begin the experiment‚ 8 ml of 0.1% Bromophenol blue (BPB) solution was made by diluting 0.25% BPB solution. From the 0.1% BPB solution‚ six diluted solutions‚ ranging from 1:50 to 1:10000‚ were prepared. Each solution was then run in the UV spectrophotometer to measure the absorbance at 590nm. DI water was used as a blank and samples were measured starting from the least concentrated one. The graph of concentration versus absorbance was plotted from the obtained data. In the second part‚ each
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saturated KHT solution. Several such solutions were prepared at various temperatures between 10°C and 50 °C‚ and filtrated into dry 250-mL conical flasks. For solutions made above or below the room temperature‚ their temperatures dropped or increased during filtrations. For each solution‚ two portion of 25.00±0.03 mL were pipetted into two 250-mL conical flasks and titrated with 0.07274 M of NaOH solution respectively with phenolphthalein as indicator. The temperatures of the KHT solutions and the corresponding
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the bottle. For about one minute the bottle was shaken. 3. The bottle was labeled with my name and set aside for a day. 4. Filter the contents of the bottle‚ into a dry conical flask. 5. Using a 10 cm3 pipette‚ transfer 10.0 cm3 calcium hydroxide solution to a conical flask‚ add a drop of phenolphthalein indicator and titrate against hydrochloric acid until the pink colour just disappears. 6. Perform three accurate titrations. 7. Record the temperature. Treatment of Results: Raw Data:
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The investigation was designed to determine the effect of the addition of increasing concentrations of a miscible liquid (ethanol) on the solubility of KNO3 in water. The results of the investigation support the hypothesis that water‚ which exhibits greater polarity‚ is able to dissolve a greater mass of KNO3 at lower temperatures compared to tested concentrations of Ethanol ranging from 12.5% to 30%. Furthermore‚ the results of the graph 1 show correspondence to the dielectric constant of each solvent
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