There are two classifications comparing the strengths of acids and bases, weak or strong. There are typically considered 6 strong acids and 6 strong bases. The same would be true for any of the bases as well — 1 mole of KOH dissolved in water would result in 1 mole of potassium ions and 1 mole of hydroxide ions. However, be careful to watch the stoichiometry. The extent to which they ionize is dependent on the specific weak acid or base, and is denoted by the Ka value.
Major Species:. Because this is a weak acid, it will only partially dissociate. What components are major, and what are minor? As a quick trick that works majority of the time, you can assume that strong acids will dissociate into major species, while weak acids will dissociate into minor species. Conjugate Acids and Conjugate Bases:.
Conjugate acid and base simply means the complement of a base or acid, respectively. The conjugate acid will donate a proton and become the base, and the conjugate base will accept a proton to become the acid. Note that the acid pairs with the conjugate base, and the base pairs with the conjugate acid not acid with conjugate acid, and base with conjugate base. Water and KW:. In a neutral solution, the concentration of hydrogen ions is equal to the concentration of hydroxide ions.
Water is typically considered to be neutral, and KW is used to demonstrate the acidity of water. KW has a value of 1. By solving for either the concentration of hydronium ion or hydroxide ion, we take the square root of KW, 1. This is our baseline. If the concentration of hydrogen ions exceeds this, the solution will be acidic. If the concentration of hydroxide ions exceeds this, aka the concentration of hydrogen ions falls below this number, then the solution will be basic. Note that at different conditions, KW will no longer equal 1.
Solutions with a pH below 7 are considered acidic, while solutions with a pH above 7 are considered basic. Explanation: For a solution to be a good conductive is when it contains a high number of ions that will serve as electrons shuttles from one electrode to another. Images source: Zumdahl textbook. Related questions Question 14e Question 14e8a. What are some examples of ionic compounds? Why do metallic compounds conduct electricity as a solid?
Why are properties of covalent compounds so diverse? Why are metallic compounds malleable? What are metallic compounds and why are they conductive? Why are covalent compounds not conductive?
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