BackWeak Base-Strong Acid Titrations definitions
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1/15BackSkip to main contentBackWeak Base
A substance that partially accepts protons in water, resulting in a basic solution with a pH above 7 before titration. Strong Acid
A substance that completely donates protons in water, causing a rapid decrease in pH when added to a base. Titrant
A solution of known concentration added during titration to react with the analyte and determine its quantity. Analyte
The substance in a titration whose concentration is being determined by reaction with a titrant. ICF Chart
A table tracking moles of reactants and products at initial, change, and final stages during titration. ICE Chart
A table using molarity to monitor concentrations at initial, change, and equilibrium for weak species. Equivalence Point
The stage in titration where moles of acid equal moles of base, resulting in complete neutralization. Buffer
A solution containing a weak acid and its conjugate base, resisting pH changes upon small additions of acid or base. Henderson-Hasselbalch Equation
A formula relating pH to pKa and the ratio of conjugate base to acid in a buffer system. Conjugate Acid
The species formed when a base accepts a proton, often influencing pH after neutralization. Conjugate Base
The species remaining after an acid donates a proton, often acting as a weak base in solution. Base Dissociation Constant
A value (Kb) expressing the extent to which a base dissociates in water, crucial for pH calculations. Acid Dissociation Constant
A value (Ka) indicating the degree to which an acid dissociates in water, derived from Kb for conjugate pairs. pOH
A measure of hydroxide ion concentration, calculated as the negative logarithm of [OH−], used to find pH. 5% Approximation
A shortcut for simplifying equilibrium calculations by neglecting small changes when the initial concentration greatly exceeds Kb.
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