Acidity in chemistry is defined by pH and pKa values, indicating hydrogen ion concentration and acid strength, respectively. The text delves into the Bronsted-Lowry theory, acid dissociation constants (Ka), and the use of ICE tables for pH calculations in weak acid solutions. It also discusses the significance of percent ionization in assessing acid strength and the practical applications of these concepts in predicting the behavior of acids and bases in solutions.
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The pH scale measures the hydrogen ion concentration in a solution, with lower values indicating higher acidity
The pKa value reflects an acid's strength and is derived from the acid dissociation constant (Ka)
The Bronsted-Lowry theory explains the relationship between acids and bases, with acids being proton donors and bases being proton acceptors
The acid dissociation constant (Ka) quantitatively defines an acid's strength and is calculated by measuring the degree of dissociation in water
The equilibrium expression for Ka is crucial for calculating the extent of dissociation in weak acids
ICE tables offer a structured approach for determining equilibrium concentrations in weak acid solutions
pH and pKa are closely related concepts, with pH being the negative logarithm of the hydrogen ion concentration and pKa being the negative logarithm of the acid dissociation constant
The Henderson-Hasselbalch equation provides a relationship between the pH of a buffer solution, the pKa of the acid, and the ratio of the conjugate base to the acid
pH and pKa can be calculated using the formulas pH = -log10[H+] and pKa = -log10(Ka), respectively
Percent ionization is a metric for evaluating an acid's strength and is calculated by determining the fraction of the acid that has dissociated into ions at equilibrium
Understanding percent ionization helps in comparing the relative strengths of acids and predicting their behavior under different chemical conditions
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The ______-______ theory defines acids as ______ ______ and bases as ______ ______.
Bronsted-Lowry
proton donors
proton acceptors
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Definition of Ka in acid dissociation
Ka = [H+][A-]/[HA], equilibrium constant for acid dissociation in water.
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Significance of large vs small Ka values
Large Ka indicates strong acid, complete dissociation; small Ka indicates weak acid, partial dissociation.
