Ph Lab Report

10. A pH scale describes the degree of acidity or alkalinity of a substance. 0 to 6.9 indicates an acidic solution, 7.1 to 14 indicates an alkaline solution, and 7 indicates a neutral solution.

An example would be pure water. Most of the time the pH is determined by pH paper but there are also other ways to determine the pH. For example, in this lab, cabbage juice was used. Cabbage juice is a great pH indicator because it can be homemade and easy to access.

twice. Place the pH probe in the beaker and record the pH in the data table. Drag the beaker to the red

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. |

Title: Using pHydrion paper to test the pH of vinegar, distilled water, laundry detergent, milk, NaOH, Mr. Clean, Baking Soda, Ammonia, 7up, Gatorade, and 4 unknown substances.

Explain the pH scale and how it is used to indicate acidic, alkaline, and neutral solutions.

PH is . a numeric scale used to specify the acidity or alkalinity of an aqueous solution. The tests my group and I did was Dissolved Oxygen, Nitrate, phosphate, and the alkalinity tests. We also tested the rocks to see if they could neutralize the rocks. Neutralize renders something in effective or harmless applying an opposite force of effect. The two rocks that we studied were limestone and sandstone.

In order for the media to show the change in acidity the solutions are modified and include an indicator chemical. This indicator will change color depending on the ph level of the media it is in. For all the media used in this experiment, the indicator changes to a yellow color when in the presence of an acid and turns magenta/pink when in the presence of a base or alkali.

Next, add enough bromothymol blue solution to each test tube until the water is blue. Next, using a straw, blow into the four test tubes until the color blue turns to the color of a yellowish/green. Then cut a sprig of Elodea from the plant and place one sprig into each of the four test tubes. Then the test tubes were sealed with a stopper. Two of the test tubes will be labeled light and placed into sunlight for about 2 hours. Then the other two test tubes will be placed into complete darkness for about 2 hours. After time is up, record the color of the solution from the four test tubes (Gunstream,

Can red cabbage juice indicator be used to determine the strength of acids and bases? Explain.

The listed materials were taken to a workstation and placed on a blue tray. Water was poured into the zip plastic bag. The red cabbage leaves were torn apart and crushed. They were then placed into the bag containing water. Pressure was then applied to the bag. The 8 cups were then placed on a piece of paper on the tray. The purple tinted water from the bag was then poured into the 5 clear plastic cups. The cream of tartar was then added to one of the 3 small cups. The vinegar was then added to the second small cup. The laundry detergent was then added to the last small cup. A toothpick was then dipped into the cream of tartar and then dipped into one of the 4 clear plastic cups. Observations were recorded. A separate toothpick was then dipped into the laundry detergent and then dipped into a different clear plastic cup than the last one. Observations were recorded. The final toothpick was then dipped

My science fair topic will be measuring the acidic levels in different companies of water bottles such as Aquafina, Dasani, Evian, Fiji, Miami Dade Tap Water, Penta, Publix Spring Water, Smart Water, Smart Water, Volvic, Voss, and Zephyrhills. Bottled water has been tested for its ppm (parts per million) to measure the amount of particles inside the water. The pH scale is a measurement of how acidic or basic an aqueous solution is. The pH scale has a range of 0-14; numbers less than 7 are considered acidic and numbers greater than 7 are considered basic. An acidic pH level means that the solution has more free hydrogen ions, and a basic pH level means that the solution has more free hydroxyl ions. pH is reported in logarithmic units and an increase or decrease of one on the pH scale has a 10-fold change. The negative logarithmic of the hydrogen ion concentration calculates the pH level of a solution. This is why pH stands for the potential of hydrogen and it calculate din

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

To better understand pH levels, it is essential to know the differences between an acid and a base or alkaline and what makes a food acidic or basic. Acids “taste sour, have a pH of less than 7, and will turn a pH strip red” (Science Geek). A neutral substance does not contain any of the characteristics of an acid or a base. It does not change the color of the pH strip and has a measurement close to a 7 on a digital pH meter. Alkaline foods “taste bitter, have a pH greater than 7, and will turn a pH strip blue” (Science Geek).

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.