An Investigation to Find the Effect of Bile Salts of on the Digestion of Lipids

The procedure of this lab is to determine if liver and potato cells contain natural buffers that resist large change in pH as 1. NaCl or 1. NaOH are added to the solution.

We reject Ho if χ2 > χα2. At α=0.05, with 4 degrees of freedom, the critical value becomes χα2=9.488 (table E.4)

10. Which had the greatest average 1- OD (amount of bile acid adsorbed to meal particles), the standard meal with bile acid or the

4. Describe the hormonal control of the secretion of bile and pancreatic juice during the digestive process.

The digestion of lipids occurs mostly in the small intestine, mainly the upper jejunum. Lipases from the pancreas are secreted into the small intestine as a part of pancreatic enzyme and breakdown lipids to fatty acids. Bile salts, created by the liver, enter the duodenum to mix with fatty acids to form micelles. The development of these micelles allows the absorption of fatty acids at intestinal villi. Pancreatic lipase, bile salts and functioning lymphatic channels help break up fat if these are working correctly then steatorrhea

Triglyceride concentrations in the liver are much higher than the heart and kidney. The differences between triglyceride and glycerol concentrations were triglyceride includes the free glycerol plus the glycerol. Pure glycerol concentrations were not determined because of reagent availability. The triglyceride concentrations were assumed to be proportional to glycerol concentrations. (Figure 2)

The pH of the region is maintained at 7 or 8 this is the pH that is optimal for the enzymes to function. This is kept at a constant with the bile from the gallbladder.

To begin, three sets ofabout 0.3000g of KHP are weighed out on an analytical balance. Put the three sets of KHP into three separate, labeled flasks. All three sets of the KHP is then dissolved with approximately 50mL of deionized water. Next, a buret is used to start the actual titration. Buret is initially filled to 0.00mL mark with the NaOH solution, this is recorded as initial volume. Next, add 2-3 drops of phenolphthalein indicator into each of the three flasks containing KHP. A magnetic stir bar is then added to the first flask, and placed above a stir plate. Everything is positioned under the buret. Stirrer is put on medium speed and the titration can start. Slowly release the NaOH into the KHP flask. As the end point is reached, a pink color will be seen in the flask. When the lightest pink possible remains in the solution for more than 30 seconds titration is complete. The final volume is recorded, and the same steps are taken for the other two sets of KHP solution. Finally, blank titration is completed to determine deviation.

Fry Brothers heating and Air Conditioning, Inc. employs Larry Clark and George Murnen to make service calls to repair furnaces and air conditioning units in homes. Tom Fry, the owner, would like to know whether there is a difference in the mean number of service calls they make per day. Assume the population standard deviation for Larry Clark is 1.05 calls per day and 1.23 calls per day for George Murnen. A random sample of 40 days last year showed that Larry Clark made an average of

The main purpose of this lab is to identify and separate the main components of milk. To do this an understanding of the properties of these components in needed to separate them from one another. We will be separating the components with their polarity or non-polarity and the temperature at which specific components precipitate. To do this we will be using hot plates, gravity filters and vacuum filters1, water and ice baths, and blot drying.

By using acid-base titration, we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were unsuitable because their pH ranges for their color changes did not cover the equivalence points of the trials in which they were used. However, the

The second step is defining the significance level, determining the degrees of freedom and finding the critical value. The a-level shows that for a result to be statistically significant, it cannot occur more than the a-level percentage of time by chance. The critical value can be obtained by using the t-test table. The degrees of freedom is

The bile moves into the gallbladder via tiny tubes. The bile is stored in the gallbladder and waits, becoming concentrated, for the signal to be released into the duodenum aiding in digestion. Without bile, the body could not digest fats, as fats do not absorb into water. The bile acts as a detergent and allows the two to mix.

The primary function of the digestive system is to transfer nutrients, water, and electrolytes from the food consume into the body’s internal environment. The ingested food is essential as an energy source, or fuel, from which the cells can generate ATP to carry out their particular energy-dependent activities such as contraction, transport, synthesis, secretion and even renewal of body tissues. Three primary categories of food ingested by humans which are carbohydrates, proteins and fats emerge as large molecules. These large molecules cannot cross plasma membranes intact to be absorbed from the lumen of the digestive tract into the blood or lymph; hence, it must undergo degradation in size (Sherwood, 2013). This

For this experiment, a pH meter was used so this part of the experiment began with the calibration of the pH meter with specified buffers. The buret was then filled with the standard HCl solution and a set-up for titration was prepared. 200g of the carbonate-bicarbonate solid sample was weighed and dissolved in 100 mL of distilled water. The sample solution was then transferred into a 250-ml volumetric flask and was diluted to the 250-mL mark. The flask was inverted several times for uniform mixing. A 50-mL aliquot of the sample solution was measured and placed unto a beaker. 3 drops of the phenolphthalein indicator was added to the solution in the beaker. The electrode of the pH meter was then immersed in the beaker and the solution containing the carbonate-bicarbonate mixture was titrated with the standard HCl solution to the phenolphthalein endpoint. Readings of the pH were taken at an interval of 0.5 mL addition of the titrant. After the first endpoint is obtained, 3 drops of the methyl orange was added to the same solution and was titrated with the standard acid until the formation of an orange-colored solution. Readings of the pH were also taken at 0.5 mL addition of the titrant.