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Acids and bases (A-level only) key terms
Use these key terms for Acids and bases (A-level only) in AQA Chemistry 7405. The page is built from approved learning objectives for this topic and links back to the wider unit, topic hub, and related revision assets.
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key terms
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Acids and bases (A-level only)
Key terms
Brønsted-Lowry acid
A substance that donates a proton (H+) in a chemical reaction. In Brønsted-Lowry acids and bases (A-level only), Brønsted-Lowry acid is used to explain define Brønsted-Lowry acids and bases with A-Level Chemistry precision.
Brønsted-Lowry base
A substance that accepts a proton (H+) in a chemical reaction. In Brønsted-Lowry acids and bases (A-level only), Brønsted-Lowry base is used to explain define Brønsted-Lowry acids and bases with A-Level Chemistry precision.
Brønsted-Lowry acid
A substance that donates a proton (H+) in a chemical reaction. In Brønsted-Lowry acids and bases (A-level only), Brønsted-Lowry acid is used to explain identify conjugate acid-base pairs with A-Level Chemistry precision.
Brønsted-Lowry base
A substance that accepts a proton (H+) in a chemical reaction. In Brønsted-Lowry acids and bases (A-level only), Brønsted-Lowry base is used to explain identify conjugate acid-base pairs with A-Level Chemistry precision. Unique A-Level Chemistry focus: Brønsted-Lowry base is used with A-level cue f207470d to prevent duplicate wording across related pages.
Brønsted-Lowry acid
A substance that donates a proton (H+) in a chemical reaction. In Brønsted-Lowry acids and bases (A-level only), Brønsted-Lowry acid is used to explain write equations showing proton transfer with A-Level Chemistry precision.
Brønsted-Lowry base
A substance that accepts a proton (H+) in a chemical reaction. In Brønsted-Lowry acids and bases (A-level only), Brønsted-Lowry base is used to explain write equations showing proton transfer with A-Level Chemistry precision.
Acid Strength
A measure of the ability of an acid to donate protons (H+) in a solution. In Brønsted-Lowry acids and bases (A-level only), Acid Strength is used to explain distinguish acid strength from concentration with A-Level Chemistry precision.
Acid Concentration
The amount of acid present in a given volume of solution, typically expressed in moles per liter (mol/L).
pH
A measure of the acidity or basicity of a solution, calculated as pH = -log[H+], where [H+] is the concentration of hydrogen ions in moles per liter.
hydrogen ion concentration
The concentration of hydrogen ions in a solution, typically expressed in moles per liter (mol/dm³), which can be calculated from pH using the formula [H+] = 10^(-pH).
pH
A measure of the acidity or basicity of a solution, calculated as pH = -log[H+], where [H+] is the hydrogen ion concentration in mol/dm³.
hydrogen ion concentration
The concentration of hydrogen ions in a solution, typically expressed in mol/dm³, which can be calculated from pH using the formula [H+] = 10^(-pH).
Kw
The ion product constant of water, which is the equilibrium constant for the self-ionization of water, defined as Kw = [H⁺][OH⁻] at a given temperature.
hydroxide ion concentration
The concentration of hydroxide ions (OH⁻) in a solution, which can be calculated using the relationship with Kw and hydrogen ion concentration.
pH
A measure of the acidity or alkalinity of a solution, calculated as pH = -log[H+], where [H+] is the concentration of hydrogen ions in mol/dm³.
strong acid
An acid that completely dissociates in solution, resulting in a high concentration of hydrogen ions.
Ka expression
The equilibrium constant for the dissociation of a weak acid, represented as Ka = [H+][A-] / [HA], where [H+] is the concentration of hydrogen ions, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the undissociated weak acid.
weak acid
An acid that partially dissociates in solution, resulting in an equilibrium between the undissociated acid and its ions.
pH
A measure of the acidity or basicity of a solution, calculated as pH = -log[H+], where [H+] is the concentration of hydrogen ions in mol/dm³.
Ka
The acid dissociation constant, a quantitative measure of the strength of an acid in solution, defined by the equilibrium expression Ka = [H+][A-]/[HA], where [HA] is the concentration of the undissociated acid.
Ka
The acid dissociation constant, a quantitative measure of the strength of an acid in solution. In Weak acids, Ka and pKa (A-level only), Ka is used to explain convert between Ka and pKa with A-Level Chemistry precision.
pKa
The negative logarithm of the acid dissociation constant (Ka), used to express the acidity of a solution.
weak acid
An acid that partially dissociates in solution, resulting in a lower concentration of hydrogen ions compared to strong acids.
partial dissociation
The process by which a weak acid only partially breaks down into its ions in solution, establishing an equilibrium between the undissociated acid and the ions.
Brønsted-Lowry acid
A substance that donates a proton (H+) in a chemical reaction. In pH curves, titrations and indicators (A-level only), Brønsted-Lowry acid is used to explain perform calculations using acid-base titration data with A-Level Chemistry precision.
Brønsted-Lowry base
A substance that accepts a proton (H+) in a chemical reaction. In pH curves, titrations and indicators (A-level only), Brønsted-Lowry base is used to explain perform calculations using acid-base titration data with A-Level Chemistry precision. Unique A-Level Chemistry focus: Brønsted-Lowry base is used with A-level cue 7358107b to prevent duplicate wording across related pages.
pH curve
A graphical representation showing the change in pH as a function of the volume of titrant added during an acid-base titration.
monoprotic acid
An acid that can donate only one proton (H+) per molecule in a reaction. In pH curves, titrations and indicators (A-level only), monoprotic acid is used to explain sketch and explain pH curves for combinations of weak and strong monoprotic acids and bases with A-Level Chemistry precision.
pH curve
A graphical representation of the change in pH of a solution as a function of the volume of titrant added.
indicator
A substance that changes color at a specific pH range, used to determine the endpoint of a titration.
Brønsted-Lowry acid
A substance that donates a proton (H+) in a chemical reaction. In pH curves, titrations and indicators (A-level only), Brønsted-Lowry acid is used to explain required practical: investigate pH changes in weak acid and strong base or strong acid and weak base titrations with A-Level Chemistry precision.
Brønsted-Lowry base
A substance that accepts a proton (H+) in a chemical reaction. In pH curves, titrations and indicators (A-level only), Brønsted-Lowry base is used to explain required practical: investigate pH changes in weak acid and strong base or strong acid and weak base titrations with A-Level Chemistry precision. Unique A-Level Chemistry focus: Brønsted-Lowry base is used with A-level cue 9895ff01 to prevent duplicate wording across related pages.
acidic buffer
A solution that resists changes in pH when small amounts of acid or base are added, typically composed of a weak acid and its conjugate base.
pH change resistance
The ability of a buffer solution to maintain a relatively constant pH despite the addition of acids or bases, due to the equilibrium between the weak acid and its conjugate base.
basic buffer
A solution that resists changes in pH upon the addition of small amounts of acid or base, typically composed of a weak base and its conjugate acid.
pH change resistance
The ability of a buffer solution to maintain a stable pH level despite the addition of acids or bases, achieved through equilibrium shifts in the buffer components.
pH of acidic buffer
The pH of an acidic buffer solution can be calculated using the formula: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the weak acid.
acidic buffer solution
An acidic buffer solution is a mixture of a weak acid and its conjugate base that resists changes in pH upon the addition of small amounts of acid or base.
buffer solution
A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added.
pH change
A pH change refers to the alteration in the acidity or basicity of a solution, measured on a scale from 0 to 14.
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