Acid Reaction Essay

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There were many things that I learned in Module 7 . Some of them where: what is the difference between an acid and a base; what is pH; what is equilibrium, what is Le Châtelier’s principle; and what is oxidation. Here are some of the things that I learned in lesson 07.01 (Acids and Bases) and lesson 07.02 (Acid-Base Reactions). An acid is a substance that produces hydrogen ions, H+ or hydrodium ionsH3O+ in solution. There are three “kinds of acids”: Arrhenius, BrØnsted-Lowry, and Lewis Acid. An Arrhenius acid is a substance the increases the concentration of hydrogen ion, H+ or hydronium ions H3O+when dissolved in water. You must have water. A BrØnsted-Lowry acid is any substance that donates a hydrogen ion, H+ to another substance. A Lewis acid is any substance that accepts a lone pair of electrons.A strong acid is one that breaks apart close to 100% when in solution (example HCl). When dissolved in water, HCl breaks apart into H+ and Cl- ions. Not all acids break apart. A weak acid is/are chemicals that do not break apart well. Acids have a sour taste, they are: corrosive and electrolytes. Acids react with active metals (group 1 or 2) to produce hydrogen gas, H2 They also react with bases to produce salt and water (a neutralization reaction). An Arrhenius base is any substance that increases the concentration of hydroxide ions (OH-) when dissolved in water. A BrØnsted-Lowry base is one that accepts a hydrogen ion, H+. A Lewis base is any substance that donates a lone pair of electrons. Bases have a bitter taste, bases react with acids to produce a neutralization reaction, and solutions that are basic feel slippery. On the pH scale, 7 is neutral. An acidic solution will have a greater hydrogen ion than hydroxide ion concent... ... middle of paper ... ... the reaction to shift to the right would be to remove products. A third way is to change the temperature. Since this is an endothermic reaction, +∆H, we can imagine that “heat” is a reactant. Thus, if we add heat, it will shift to the right. To be classified as a redox reaction, we need at least two elements to change oxidation states. The easiest way to look at a reaction and determine this is if you have an element by itself on one side of the reaction and it is in a compound on the other side. Most of the time, the oxidation number of each element in a compound is their common charge. The sum of oxidation numbers must equal the compounds overall charge. Elements in the natural state (by themselves) have an oxidation number of 0. The reducing agent is the species responsible for reducing the other chemical. Therefore, the reducing agent is oxidized itself.

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