Carbon dioxide (CO2)
Because the drink contains dissolved carbon-dioxide gas under pressure. When you release the cap, the pressure is released - allowing the dissolved CO2 to revert to its gaseous form - this causes the 'fizz'.
These is because, it contain's dissolved carbon dioxide (CO2) as the anion CO32-; carbon dioxide is added to improve the taste and for raising the acidity.
Sure! Some examples of gas solutions include air (a mixture of gases such as oxygen and nitrogen), carbonated water (carbon dioxide gas dissolved in water), natural gas (methane and other gases dissolved in a liquid), hydrogen gas dissolved in water, and oxygen gas dissolved in water.
Saturated solution is the ideal type of solution. The other is unsaturated, which is less saturated than what the solvent (water, liquid etc.), and it can dilute. The last one is supersaturated which mean the solution contains more solute (solid materials).
The dissolved substance is a called a solute.
AMOUNT OF CO2 DISSOLVED IN SOFTDRINKS?
Because the drink contains dissolved carbon-dioxide gas under pressure. When you release the cap, the pressure is released - allowing the dissolved CO2 to revert to its gaseous form - this causes the 'fizz'.
How about the little bubbles visible in softdrinks. They are CO2 in gaseous form.
These is because, it contain's dissolved carbon dioxide (CO2) as the anion CO32-; carbon dioxide is added to improve the taste and for raising the acidity.
This is a gas dissolved in a liquid.
This is a gas dissolved in a liquid.
This is a gas dissolved in a liquid.
it is a dissolved gas
Sure! Some examples of gas solutions include air (a mixture of gases such as oxygen and nitrogen), carbonated water (carbon dioxide gas dissolved in water), natural gas (methane and other gases dissolved in a liquid), hydrogen gas dissolved in water, and oxygen gas dissolved in water.
A liquid is capable of containing more dissolved gas when it is hot. This does not mean that it does contain more dissolved gas, simply that it can.
oxygen \
Henry's law states that the solubility of a gas is directly proportional to the partial pressure of that gas over the liquid. The higher the partial pressure, the more gas will be dissolved-- that's why your blood boils in a vacuum; there's not enough pressure to keep the gas in it dissolved.