Key Terms and Concepts from the Module
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| Chemical Equilibrium | The point at which both the forward and reverse reactions in a chemical equation have equal reaction rates: When this occurs, the amounts of each substance in the chemical reaction will not change, despite the fact that both reactions still proceed.
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| Equilibrium Constant | K = Products/Reactants with the Stochiometric Coefficients as superscripts
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| When K is large, the equilibrium is | weighted toward the products side of the equation
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| When K is small, the equilibrium is | weighted toward the reactants side of the equation
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| When K is near unity, the equilibrium is | balanced between reactants and products
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| When a solid appears in a chemical equilibrium | it is not included in Equation (15.2)
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| When a liquid appears in a chemical equation | we do not include it in Equation (15.2). This applies only to the liquid phase; it does not apply to the aqueous phase.
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| When a stress (such as a change in concentration, pressure, or temperature) is applied to an equilibrium | the reaction will shift in a way that relieves the stress and restores equilibrium
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| Le Chatelier's principle ignores solids and liquids | as a source of stress to the equilibrium
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| When an equilibrium is subjected to an increase in pressure | it will shift away from the side with the largest number of gas molecules
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| If pressure decreases | the equilibrium will shift toward the side with the largest number of gas molecules
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| If there are no gases in the equation or if the number of gas molecules are the same on both sides | nothing will happen
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| When temperature is raised, an equilibrium will shift | away from the side of the equation that contains energy
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| When temperature is lowered, the reaction will shift | toward the side that contains energy
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| acid ionization reactions | The reaction in which an H + separates from an acid molecule so that it can be donated in another reaction
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| acid ionization constant | The equilibrium constant for an acid's ionization reaction
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| If the ionization constant of an acid is large | the acid is considered a strong acid
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| If the ionization constant is not large | we call it a weak acid
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| In general, the larger the ionization constant | the stronger the acid
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| base ionization reaction | combined with water and accepts H+
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| Solutions with pH 0 - 1.9 are considered | strongly acidic
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| solutions with pH 2 - 6.9 are considered | weakly acidic
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| solutions with pH 7.1 - 12 are considered | weakly basic
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| solutions with pH 12.1 - 14 are considered | strongly basic
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| A pH of 7 indicates a | neutral solution
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