Equilibrium Reactions and Le Chatelier's Principle

If the broth turns yellow, it means that acid was produced and reported as A. If the organism can break down the amino acids be de-amination and ammonia is produced, this will raise the pH level turning it pink. This alkaline result was reported as K.

You find a sample of a solution that has a faint odor resembling vinegar. You are verifying that it is indeed vinegar and you add a few drops of phenolphthalein. The sample turns pink. What assumptions can you make about this sample?

The main objective of this experiment is to differentiate between a physical change and a chemical change.

Background Information: We are going to use our knowledge of the Le Chatelier’s principle in order to observe this experiment. The principle states that the equilibrium will shift in the direction that will minimize the effects of the change.

When the red Co(NO3)2*6H2O crystal was added to the white NH4 crystal, and water was added to dissolve, the solution turned blue in color. As the solution was nixed, the color changed to that of a blue-purple and a blue precipitate formed. When the 6 M NH3 began to be added, the color shifted to dark purple color after 15 mL of ammonia and the amount of the precipitate was less. After 20 mL of ammonia, the solution became a red brown with very little of the blue precipitate. After 30 mL of ammonia, the solution was similar in color to an iodine solution, a dark brown-red, almost black in color. At this point there was no visible precipitate on the surface of the solution. After 40 mL of the ammonia had been added, the solution was the same iodine like color as before. When closely examined, there was a black precipitate that had settled on the bottom of the beaker. At this point, hydrogen peroxide, 3% H2O2, was added to solution. After 4 mL of the H2O2 was added, the solution was the same color and the precipitate had not changes. After 8 mL of the H2O2, there was not noticeable change. After 12 mL of the H2O2, the solution was slightly redder in color but the precipitate had not changed. After 15 mL of H2O2, the solution was the same color and no changes had occurred to the precipitate. At 17 mL, the solution began to effervesce slightly, though there

The objective of the experiment is to apply Le Chatelier's Principle, which is a system that responds to an external stress and then adjusts itself in order to alleviate the stress when it is at equilibrium. A reactant is added, and the equilibrium is reestablished, resulting in more products and fewer reactants, and thus, the position of equilibrium is shifted to the right. When a product is added, the equilibrium position is shifted to the left because there are more reactants and fewer products.

Regarding temperature, Le Chatelier’s principle states that seeing as the production of COCl2 from CO + Cl2 comes about through a process of exothermic reaction, that the reverse would come about through a process of endothermic reaction. Therefore increasing the temperature would cause a reduction in the equilibrium yield of COCL2 favouring the original reactants CO + Cl2. (163)

C.|NH3 + BTB|A4|The mixture is a lighter royal blue under white paper and a darker royal blue under black paper. The mustard yellow would be an acidic indicator and the royal blue a basic indicator. |

This shows Le Chatelier’s principle as the system was able to neutralize the disturbance from its equilibrium.In this case, the change was the addition of molecules to the reactants. This caused an increase in the number effective collisions between the reactant’s molecules. Also, this raised the rate of the forward reaction. The system then has an increased amount of reactants and therefore has to travel in the forward direction to make extra products. This occurred in order to return the system to equilibrium by removing some of the excess reactants. By shifting in the forward direction, more products are being produced by the excess reactants. This ensures that the forward and reverse reaction rates are equal, which brings the system back to a state of

A system is Material moving most stable when it has reached equilibrium. A out of the cell system will tend to go to equilibrium (lowest, accessible energy state) in the absence of added energy (Figure 2).

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

2. In Part I of this experiment, acetic acid is titrated with NaOH. The net ionic equation for acetic acid reacting with NaOH is CH3COOH+ NaOH =NaC2H3O2+H2O. The equivalence point is when the moles of the titrant and other solution are equal.. You detect the equivalence point by obtaining the point on the graph where the steep pH occurs. In titrating acetic acid with NaOH, the pH is greater than 7 at the equivalence point because NaOH is a strong base so it results in a higher pH, due to the OH- ions in the solution.

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 purpose of this lab was to test the law of conservation of mass by comparing the total mass of the reactants in a chemical reaction with the total mass of the product.

In this lab a acid-base indicator phenolphthalein was used to determine endpoint of a reaction HCl(aq) and KOH(aq). At the end point all of the HCl(aq) would have reacted with KOH(aq), and the pH becomes 7. The phenolphthalein would changed colours from colourless to pink indication when enough KOH(aq) was added. The purpose of numerous trials was to use the average volume of the 3 trials with similar measurements.