IN YOUR OWN WORDS With citations if applicable 1. Describe the different types o
ID: 1007816 • Letter: I
Question
IN YOUR OWN WORDS
With citations if applicable
1. Describe the different types of solutions that can be formed from the three states of matter.
2. Compare and contrast unsaturated, saturated, and supersaturated solutions.
3. Why is it important to be able to convert between percent by mass, mole faction, molarity, and molality?
4. Discuss Henry's law and the relationship between gas solubility and pressure. 5. Discuss in detail the rate of reaction based on activation energy, and a catalyst (enzyme). How does this apply to living organisms?
Explanation / Answer
1.
You can have solutions of solids in liquids (ocean water), dissolved gases in liquids (ammonia), solutions of liquid in liquid (vinegar), solutions of gas in gas (air), or solutions of solids in solids. If the solid-solid solution is metal, you would call that an alloy (like bronze).
An unusual solution is silver amalgam - liquid mercury dissolved in solid silver.
2.
Unsaturated Solution: The solution in which more amount of solute can be dissolved is called unsaturated solution.The quantity of solute is less than the solubility.
Supersaturated solution: The solution in which excess amount of solute is added is called unsaturated solution.The quantity of solute exceeds the solubility.
Saturated solution: The solution in which is an intermediate between unsaturated and Supersaturated solution. The quantity of solute equals the solubility.
3.
Solutions are homogeneous (single-phase) mixtures of two or more components. For convenience, we often refer to the majority component as the solvent; minority components are solutes. Solutions play a very important role in Chemistry because they allow intimate and varied encounters between molecules of different kinds, a condition that is essential for rapid chemical reactions to occur.
Concentration is a general term that defines the quantity of solute contained in a given amount of solution. Various ways of expressing concentration are in use; the choice is usually a matter of convenience in a particular application. One should become familiar with all of them.
The concentration is based on the quantity of solute in a fixed quantity of solution. The “quantities” referred to here can be expressed in weight, in volume, or both (i.e., the weight of solute in a given volume of solution.) In order to distinguish among these possibilities, the abbreviations (w/w), (v/v) and (w/v) are used.
Expressing a concentration as "percent mass" can be ambiguous. Where as the molarity of a solution will vary with its temperature, whereas molality and mole fraction do not.
4.
Henry's law states that, "At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid." In other words Henry's law is that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid:
C = k Pgas
C is the solubility of a gas at a fixed temperature in a particular solvent (in units of M or mL gas/L)
k is Henry's law constant (often in units of M/atm)
Pgas is the partial pressure of the gas (often in units of atm).