Interesting observation regarding solubility of gases
An interesting point regarding solubility is that from the solubility curve, the general trend is that the solubility of solids increases as the temperature is increased. Look at all the examples such as NaNO3, KNO3, KCl, NaCl etc… they all increase as the temperature is increased. But when you look at the gases, such as NH3, it decreases as the temperature is increased.
Why is that?
As the temperature is increased, the energy in the gas molecules is also then increased. Since there is an increase of kinetic energy, the gas particles can escape the liquid more readily than if it were cooler with less kinetic energy.
Real life example: Heating up a soda pop will cause it to go flat a lot faster than if the soda pop were to be kept a lower temperature.
Global warming example. Since the temperature of the earth is increases, the solubility of oxygen into the ocean and lakes is decreased. Thus, the amount of dissolved oxygen lowers, which lowers the amount of life it can hold.
- Describe and give examples of various types of solutions. Include: all nine possible types
- Describe the structure of water in terms of electronegativity and the polarity of its chemical bonds.
- Explain the solution process of simple ionic and covalent compounds, using visual, particulate representations and chemical equations. Include: crystal structure, dissociation, hydration
- Interpreting a a solubility curve of a pure substance in water and differentiate among saturated, unsaturated, and supersaturated solutions.
- Explain how a change in pressure affects the solubility of gases.
- Explain freezing-point depression and boiling-point elevation at the molecular level. Examples: antifreeze, road salt…
- Include: grams per litre (g/L), % weight-weight (% w/w), % weight-volume (% w/v), % volume/volume (% v/v), parts per million (ppm), parts per billion (ppb), moles per litre (mol/L) (molarity)
- Prepare a solution, given the amount of solute (in grams) and the volume of solution (in millilitres), and determine the concentration in moles/litre. (Molarity)
- Solve problems involving the dilution of solutions.
Include: dilution of stock solutions, mixing common solutions with different volumes and concentrations