Term
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Definition
| *Key Concept: Acids taste sour, will change the color of an acid-base indicator, and can be a strong or weak electrolyte in aqueous solutions* |
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Term
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Definition
| *Key Concepts: Bases taste bitter, feel slippery, will change the colour of an acid-base indicator, and can be a strong or weak electrolyte* |
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Term
| Arrhenius Acids and Bases |
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Definition
| *Key Concept: Arhenius said that acids are hydrogen containing compounds that ionize to yield hydrogen ions in an aqueous solution. He also said that bases are compounds that oxidize to yield hydroxide ions in an aqueous solution.* |
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Term
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Definition
| Acids which contain one ionizable hydrogen. Ex: Nitric Acid (HNO3) |
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Term
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Definition
| Acids that contain two ionizable hydrogens Ex: sulphuric acid (H2SO4) |
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Term
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Definition
| Acids that contain three ionizable hydrogens. Ex: Phosphoric Acid (H3PO4) |
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Term
| Bronsted-Lowry Acids and Bases |
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Definition
| *Key Concept: The Bronsted- Lowry theory defines an acid as a hydrogen ion donor and a base as a hydrogen-ion accepter.* |
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Term
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Definition
| The particle formed when a base gains a hydrogen ion. |
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Term
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Definition
| The particle that remains when an acid has donated a hydrogen ion |
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Term
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Definition
| Two substances related by the loss or gain of a single hydrogen ion. |
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Term
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Definition
| A water molecule that gains a hydrogen ion (becomes positively charged) |
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Term
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Definition
| A substance that can act as both an acid and a base. |
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Term
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Definition
| *Key Concept: Lewis Proposed that an acid accepts a pair of electrons during a reaction while a base donates a pair of electrons. |
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Term
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Definition
| A substance that can accept a pair of electrons to form a covalent bond. |
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Term
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Definition
| A substance that can donate a pair of electrons to form a covalent bond. |
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Term
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Definition
| The reaction in which water molecules produce the ions H+ and OH-. |
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Term
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Definition
| Any aqueous solution in which the [H+] and [OH-] are equal. |
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Term
| Ion Product Constant for Water |
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Definition
| *Key Concept: For aqueous solutions, the product of the hydrogen-ion concentration equals 1.0x10^-14 (Kw) |
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Term
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Definition
| One in which [H+] is greater than [OH-] |
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Term
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Definition
| One in which [H+] is less than [OH-] |
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Term
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Definition
| Another name for a basic solution. |
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Term
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Definition
the solution of the negative logarithm of the hydrogen-ion concentration. *Key Concept: In a solution in which [H+] is greater than 1x10^-7 M has a pH less than 7 and is an acid. The pH of pure water or a neutral aqueous solution is 7.0. A solution with a pH greater thab 7 is basic nd has [H+] of less than 1.0x10^-7
pH=-log[H+] |
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Term
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Definition
| *Key Concept: An indicator is a valuable tool for measuring pH because its acid form and base form have different colours in the solution |
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Term
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Definition
| Completely ionize in an aqueous solution. |
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Term
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Definition
| Ionize only slightly in aqueous solutions. |
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Term
| Acid Dissociation Constant |
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Definition
| The ratio of the concentration of the dissociated form of an acid to the concentration of the undissociated form. *Key Concept: Weak Acids have small Ka Values. The stronger an acid, the larder its Ka value.* |
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Term
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Definition
| Dissociate completely into metal ions and hydroxide ions. |
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Term
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Definition
| Reacts with water to form the hydroxide ions and the conjugate acid of the base. |
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Term
| Base Dissociation Constant |
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Definition
| (Kb) The ratio of the concentration of the conjugate acid times the concentration of the hydroxide ions to the concentration of the base. |
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Term
| Calculating Dissociation Constants |
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Definition
| *Key Concept: To find Ka of a weak acid or the Kb of a weak base, substitute the measured concentrations of all the substances present at equilibrium into the expression for Ka and Kb.* |
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Term
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Definition
| A reaction in which an acid and a base react in an aqueous solution to form a salt and water. *Key Concept: In general, the reaction of an acid with a base produces water and one of a class of compounds called salts.* |
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Term
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Definition
| When an acid and base are mixed, it is when the number of moles of hydrogen ions equals the number of moles of hydroxide ions. |
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Term
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Definition
| The process of adding a known concentration to determine the concentration of another solution. |
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Term
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Definition
| The solution of known concentration in a titration reaction. |
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Term
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Definition
| The point at which the indicator changes colour in a titration. *Key Concept: The point of neutralization is the endpoint of the titration.* |
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