In redox reaction, one element or compound is reduced and gains electrons, while on the other hand, the other element or compound is oxidized and loses electrons. For this lab, through the given oxidation and reduction numbers from balancing the equation and the electrons, it was shown that Manganese was reduced while Iron was oxidized. Also from the equation, the movement of electrons can be noticed, as it was added or subtracted from the substances. In order to balance an equation, there must be same number of elements on both sides, with the exception of hydrogen and oxygen. From there, in order to balance oxygen, water molecules are enumerated to the opposite of the equation/reaction.
The first one are those that are more soluble in a given solvent than the main component. The second type are those that are less soluble in a given solvent than the main component.1 The process of recrystallization begins with dissolving the material to be purified in a correct hot solvent which forms a solution. The objective is to create a saturated solution. A saturated solution is a solution in which the dissolved solute is in dynamic equilibrium with the solid solute.3 When the solution cools, it becomes supersaturated and the excess solid precipitates out of solution.3 It is important to cool the solution slowly in order for the crystals to form. The solubility of solids in a solvent is very dependent on temperature.
* A large value of Keq indicated that the equilibrium mixture contants more products than reactants. * A small value for the equilibrium constant means that the equilibrium lies toward the reactant side. * The equilibrium constant expression and the equilibrium constant of the reverse of a reaction are the reciprocals of those of the forward reaction. Section 3 * Equilibria for which all substances in the same phase are called homogeneous equilibria. * In heterogeneous equilibria two or more phases are present.
The pH of a neutral is 7. Bases have a high number of hydroxide ions, but a low number of hydrogen ions. The pH of a base range from 7.1 to 14 on the pH scale. The more hydrogen ions a substance have the stronger the acid will be. The more hydroxide ions a substance has the stronger the base will be.
The two types of passive transport are diffusion and osmosis. Diffusion is the movement of materials down a concentration gradient from an area of high concentration to an area of lo concentration. Osmosis is the diffusion of water(movement of water down a concentration gradient from an area of high concentration to an area of low concentration. Both types of passive transport continue until equilibrium(the material or water is equal in all areas) is reached. When a solution a cell is placed in has more more atoms than the cell has the solution is known as a hypertonic solution while a solution holding less water than the cell it is known as a hypotonic solution.
Titration is an operation of a common laboratory method of quantitative chemical analysis, which determines the unknown concentration of a substance in a solution by adding to a standard reagent of known concentration, this is also known as volumetric analysis. In this case C1V1= C2V2 equation was used. pH is defined by the following equation; pH= -log10H+. pH is measured by the amount of H+ ions in the solution in comparison to OH- ions; therefore, a solution with the higher pH will contain higher concentration of OH-. A solution with a pH of 7 would be neutral, while an acidic solution would have a pH of lower than 7.
Topic 8, 18 Acids & Bases Problem Set 2 1. What is the Arrhenius definition of an acid? (1) a substance that when dissolved in water increases the concentration of hydrogen ion, H+ 2. What is the Arrhenius definition of a base? (1) a substance that when added to water increases the concentration of hydroxide ion, OH-(aq).
One vaporization and condensation cycle is called a theoretical plate. The greater the amount of theoretical plates, the better the separation will be. In this experiment, there are two theoretical plates. The first plate is the initial distillation where three different fractions are collected over different temperature ranges. The first fraction is collected at 60-75℃, the second fraction is collected at 75-85℃ and the final fraction is collected at 85-105℃.
Saturated solutions of salts present yet another type of chemical equilibria. Slightly soluble salts establish a dynamic equilibrium with the hydrated cations and anions in solution. • When the solid is first added to water, no ions are initially present. • As dissolution proceeds, the concentration of ions increases until equilibrium is established. This occurs when the solution is saturated.
Shifting the equilibrium with pH changes is a classic example of Le Chatelier’s principle at work. Le Chatelier's principle states that if a chemical dynamic equilibrium is disturbed by changing the conditions (concentration, temperature, volume or pressure), the position of equilibrium moves to counteract the imposed change. So if more reactant is added, the equilibrium shifts to the right in order to consume that extra reactant, which results in more product; also if the product is removed from the system, the equilibrium shifts to the right completely increasing the yield. Yellow chromate and orange dichromate are in equilibrium with each other in aqueous solution. The more acidic the solution, the more the equilibrium is shifted to the left towards the dichromate ion.