Comparision Between Sulfuric Acid And Detergents

You know what color phenolphthalein and BTB turn when testing an acid or a base. Use three household cleaning products with BTB. Name the items tested and their results:

When the tip of the rod touched the pH paper, the color of the pH paper became blue.

In order to find the pH of each household item by using pH paper, the pH paper was placed on the drop plate. Using the dropper, start by having the household item dropped onto the pH paper. Immediately observe in order to spot any colour changes on the pH paper. To determine the pH by using the pH scale and record the pH on your table of observations. Depending on what the pH is, it could be very acidic, basic or neutral. Repeat these steps for the other products.

Solub. Or Reaction w/ hot H20: no change observed from the cool water and is soluble

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

Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.

weak bases). After ranking the pH of these solutions, you will then test your predictions in the laboratory.

The mixture might have contained more or less than 5 drops of bromophenol blue, which might have resulted in the indication of the lab.

The objective of this experiment, to determine the pKa of bromothymol blue, was accomplished spectrophotometrically. Bromothymol blue is a monoprotic acid (HIn), that is blue in basic solution and yellow in acidic solution:

The litmus paper turned a very light purple only changing the color of the paper slightly. Using the pH scale I would place the pH of the tap water at 9. After testing regular water I then took some soil from my flower bed and mixed it in a glass of water. Once, all the soil settled to the bottle of the glass I dipped my litmus paper into the water. The paper turned dark purple. Using the pH scale I think the pH of the mixture is

1. The conductivity experiment will allow us to determine the difference between ionic and molecular compounds. We will be able to identify the compounds as strong electrolytes, weak electrolytes, or nonelectrolytes. We will be able to conclude if ionic concentration and numbers of ion influence conductivity. Lastly, we will determine does polyatomic and monatomic ions influence conductivity.

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

Sodium hydrogen carbonate was added to the solution until it becomes neutral. Ph paper was used for this test to determine its ph value.

As someone living in Mississauga, I’ve always had a chance to be near one of the biggest lakes in the world, Lake Ontario. However, ever since I was a child, I was always told not to swim in the lake because it’s dirty, it would make me sick, etc. However, I realized that while by our first world standards the water is dirty, it’s still quite clean. This made me think: some of the water in the 3rd world countries across the world must have horrible quality of water. If we find the visually clean water in Lake Ontario to be dirty because of other properties, how can we tell if the water is clean or not? I did some research

The fifth, and final pigment, was Prussian blue. One milliliter of 0.5 M iron (III) chloride was measured into a test tube. Then, 0.25 M solution of potassium ferrocyanide was mixed in. They were then filtered, and left to dry. The next week there were four paint binding options: egg tempura, casein, acrylic, and water color or gum arabic. This experiment used watercolor. The first step was to grind the pigment with water to make a stiff paste. Then, gum Arabic was added in a 1:1 ratio.