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Acids & Bases Flashcards
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Acids & Bases Flashcards
Arrhenius theory acid
Acids produce hydrogen ions (H+/H3O+/hydronium ions) in aqueous solution
Arrhenius theory base
Bases produce hydroxide ions (OH-) in aqueous solution
Lowry-Brønsted theory acid
An acid is a proton (H+ ion) donor
Lowry-Brønsted theory base
A base is a proton (H+ ion) acceptor
Hydrolysis
The reaction of a salt with water
Equivalence point of a titration
The point at which the acid/base has completely reacted with the base/acid
Endpoint of a titration
The point where the indicator changes colour
Strong acids
Strong acids ionise completely in water to form a high concentration of H3O+ ions
Weak acids
Weak acids ionise incompletely in water to form a low concentration of H3O+ ions
Strong bases
Strong bases dissociate completely in water to form a high concentration of OH- ions
Weak bases
Weak bases dissociate/ionise incompletely in water to form a low concentration of OH- ions
Concentrated acids
Concentrated acids contain a large amount (number of moles) of acid in proportion to the volume of water
Concentrated bases
Concentrated bases contain a large amount (number of moles) of base in proportion to the volume of water
Dilute acids
Dilute acids contain a small amount (number of moles) of acid in proportion to the volume of water
Equivalence point
The equivalence point of a titration is the point at which the acid /base has completely reacted with the base/acid
Endpoint of a titration
The endpoint of a titration is the point where the indicator changes colour
The pH scale
The pH scale is a scale of numbers from 0 to 14 used to express the acidity or alkalinity of a solution
Kw is the equilibrium constant
Kw is the equilibrium constant for the ionisation of water or the ionic product of water or the ionisation constant of water
Auto-ionisation of water
The reaction of water with itself to form H3O+ions and OH-ions
Dilute bases
Dilute bases contain a small amount (number of moles) of base in proportion to the volume of water
Hydrolysis
The reaction of a salt with water
Kw
The equilibrium constant for the ionisation of water or the ion product of water or the ionisation constant of water, i.e. Kw = [H3O+][OH-] = 1 x 10^14 by 298 K
Ampholyte
A substance that can act as either an acid or a base
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Arrhenius theory acid
Acids produce hydrogen ions (H+/H3O+/hydronium ions) in aqueous solution
Arrhenius theory base
Bases produce hydroxide ions (OH-) in aqueous solution
Lowry-Brønsted theory acid
An acid is a proton (H+ ion) donor
Lowry-Brønsted theory base
A base is a proton (H+ ion) acceptor
Hydrolysis
The reaction of a salt with water
Equivalence point of a titration
The point at which the acid/base has completely reacted with the base/acid
Endpoint of a titration
The point where the indicator changes colour
Strong acids
Strong acids ionise completely in water to form a high concentration of H3O+ ions
Weak acids
Weak acids ionise incompletely in water to form a low concentration of H3O+ ions
Strong bases
Strong bases dissociate completely in water to form a high concentration of OH- ions
Weak bases
Weak bases dissociate/ionise incompletely in water to form a low concentration of OH- ions
Concentrated acids
Concentrated acids contain a large amount (number of moles) of acid in proportion to the volume of water
Concentrated bases
Concentrated bases contain a large amount (number of moles) of base in proportion to the volume of water
Dilute acids
Dilute acids contain a small amount (number of moles) of acid in proportion to the volume of water
Equivalence point
The equivalence point of a titration is the point at which the acid /base has completely reacted with the base/acid
Endpoint of a titration
The endpoint of a titration is the point where the indicator changes colour
The pH scale
The pH scale is a scale of numbers from 0 to 14 used to express the acidity or alkalinity of a solution
Kw is the equilibrium constant
Kw is the equilibrium constant for the ionisation of water or the ionic product of water or the ionisation constant of water
Auto-ionisation of water
The reaction of water with itself to form H3O+ions and OH-ions
Dilute bases
Dilute bases contain a small amount (number of moles) of base in proportion to the volume of water
Hydrolysis
The reaction of a salt with water
Kw
The equilibrium constant for the ionisation of water or the ion product of water or the ionisation constant of water, i.e. Kw = [H3O+][OH-] = 1 x 10^14 by 298 K
Ampholyte
A substance that can act as either an acid or a base