Chemistry Project - Red Cabbage pH Indicator

How to Make Red Cabbage pH Indicator  

Red cabbage contains a pigment molecule called flavin (an anthocyanin). This water-soluble pigment is also found in apple skin, plums, poppies, cornflowers, and grapes. Very acidic solutions will turn anthocyanin a red color. Neutral solutions result in a purplish color. Basic solutions appear in greenish-yellow. Therefore, it is possible to determine the pH of a solution based on the color it turns the anthocyanin pigments in red cabbage juice.
The color of the juice changes in response to changes in its hydrogen ion concentration. pH is the -log[H+]. Acids will donate hydrogen ions in an aqueous solution and have a low pH (pH < 7). Bases accept hydrogen ions and have a high pH (pH > 7).

Project - III

Soil Permeability's Impact
On The
Movement Of Pollution To Ground Water
Thanks to : Brady L.
 
 

ABSTRACT

The purpose of this experiment is to see how different soil permeability’s prevent the   movement of pollutants through them.  My hypothesis is that the outcome of my experiment will show that soils with greater pore space will let more water pass through them.

Science Project - II

Soil contamination by hydrocarbons

Hypothesis

Oil absorbing polymers can effectively rehabilitate soil contaminated with motor oil and render the soil suitable for growth. Seeds will geminate in the rehabilitated soil that has been treated with oil absorbing polymers.

Science Project - I

Absorption of Pollutants in Different Soil Types

PURPOSE
The purpose of this experiment was to determine which polypedon  (type of soil) was most absorbent of liquid pollutants.
The information gained from this experiment will benefit farmers, gardeners and botanists who have soil pollution problems to better understand absorbency in different types of soil

ஹலோஜென் பற்றிய பாடல்...

இப்படியும் CHEMISTRY கத்துக்கலாம்....

LIQUFACTION OF CARBON-DI-OXIDE

I.               Dry ice is placed into an acrylic plastic cylinder. A valve is closed and pressure in the cylinder increases. When the pressure reaches 350 kPa (50 psi) it stops increasing and liquid CO₂ appears. The liquid begins to boil and when all solid CO₂ is gone, the pressure increases further. The valve is opened and the pressure drops again, holding constant for a while at 350 kPa. Eventually solid CO₂ reforms, the liquid disappears, and the pressure drops completely.

II.          The critical temperature for carbon dioxide is 304K (87.8°F [31°C]). That means that no amount of pressure applied to a sample of carbon dioxide gas at or above 304K (87.8°F [31°C]) will cause the gas to liquefy. At or below that temperature, however, the gas can be liquefied provided sufficient pressure is applied. The corresponding critical pressure for carbon dioxide at 304K (87.8°F [31°C]) is 72.9 atmospheres (~73000 kPa). In other words, the application of a pressure of 72.9 atmospheres of pressure on a sample of carbon dioxide gas at 304K (87.8°F [31°C]) will cause the gas to liquefy. 

III.          Two important properties of gases are important in developing methods for their liquefaction: critical temperature and critical pressure. The critical temperature of a gas is the temperature at or above which no amount of pressure, however great, will cause the gas to liquefy. The minimum pressure required to liquefy the gas at the critical temperature is called the critical pressure.

                         For example, the critical temperature for carbon dioxide is 304K (87.8°F [31°C]). That means that no amount of pressure applied to a sample of carbon dioxide gas at or above 304K (87.8°F [31°C]) will cause the gas to liquefy. At or below that temperature, however, the gas can be liquefied provided sufficient pressure is applied. The corresponding critical pressure for carbon dioxide at 304K (87.8°F [31°C]) is 72.9 atmospheres. In other words, the application of a pressure of 72.9 atmospheres of pressure on a sample of carbon dioxide gas at 304K (87.8°F [31°C]) will cause the gas to liquefy.

Differences in critical temperatures among gases means that some gases are easier to liquify than are others. The critical temperature of carbon dioxide is high enough so that it can be liquified relatively easily at or near room temperature. By comparison, the critical temperature ofnitrogen gas is 126K (-232.6°F [-147°C]) and that of helium is 5.3K (-449.9°F [-267.7°C]). Liquefying gases such as nitrogen and helium obviously present much greater difficulties than does the liquefaction of carbon dioxide.