Term
| What are the properties of acids and bases? |
|
Definition
| acids taste sour, will change the color of an acid-base indicator, and can be strong or weak electrolytes in aqueous solution. |
|
|
Term
| How did Arrhenius define an acid and a base? |
|
Definition
| Arrhenius said that acids are hydrogen-containing compounds that ionize to yield hydrogen ions (H+) in aqueous solution. He also said that bases are compounds that iionize to yield hydroxide ions (OH-) in aqueous solution. |
|
|
Term
| What distinguishes an acid from a base in the Bronsted-Lowry theory? |
|
Definition
| the Bronsted-Lowry theory defines an acid as a hydrogen-ion donor, and a base as a hydrogen-ion acceptor. |
|
|
Term
| How did Lewis define an acid and a base? |
|
Definition
| Lewis proposed that an acid accepts a pair of electrons during a reaction, while a base donates a pair of electrons. |
|
|
Term
|
Definition
| acids that contain one ionizable hydrogen, such as nitric acid (HNO3). |
|
|
Term
|
Definition
| acids that contain two ionizable hydrogens, such as sulfric acid (H2SO4). |
|
|
Term
|
Definition
| acids that contain three ionizable hydrogens, such as phosphoric acid (H3PO4). |
|
|
Term
|
Definition
| the particle formed when a base gains a hydrogen ion. |
|
|
Term
|
Definition
| the particle that remains when an acid has donated a hydrogen ion. |
|
|
Term
|
Definition
| consists of two substances related by the loss or gain of a single hydrogen ion. |
|
|
Term
|
Definition
| a water molecule that gains a hydrogen ion and becomes positively charged. |
|
|
Term
|
Definition
| a substance that can act as both an acid and a base. |
|
|
Term
|
Definition
| a substance that can accept a pair of electrons to form a covalent bond. |
|
|
Term
|
Definition
| a substance that can donate a pair of electrons to form a covalent bond. |
|
|
Term
| How are [H+] and [OH-] related in a aqueous solution? |
|
Definition
| for aqueous solutions, the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals 1.0x10^-14. |
|
|
Term
| How is the hydrogen-ion concentration used to classify a solution as neutral, acidic, or basic? |
|
Definition
| a solution in which [H+] is greater than 1x10^-7M has a pH less than 7.0 and is acidic. the pH of pure water or a neutral aqueous solution is 7.0. a solution with a pH greater than 7 is basic and has a [H+] of less than 1x10^-7M. |
|
|
Term
| What is the most important characteristic of an acid-base indicator? |
|
Definition
| an indicator is a valuable tool for measuring pH because its acid form and base form have different colors in solution. |
|
|
Term
|
Definition
| the reaction in which water molecules produce ions. |
|
|
Term
|
Definition
| any aqueous solution in which [H+] and [OH-] are equal. |
|
|
Term
| Ion-product constant for water (Kw) |
|
Definition
| the product of the concentrations of the hydrogen ions and hydroxide ioons in water. |
|
|
Term
|
Definition
| one in which [H+] is greater than [OH-] |
|
|
Term
|
Definition
| one in which [H+] is less than [OH-]. |
|
|
Term
|
Definition
| another name for basic solutions. |
|
|
Term
|
Definition
| the negative logarithm of the hydrogen-ion concentration. |
|
|
Term
| How does the value of an acid dissociation constant relate to the strength of an acid? |
|
Definition
| weak acids have small Ka values. The stronger an acid is, the larger its Ka value. |
|
|
Term
| How can you calculate an acid dissociation constant (Ka) of a weak acid? |
|
Definition
| to find the 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 or Kb. |
|
|
Term
|
Definition
| completely ionized in aqueous solution. |
|
|
Term
|
Definition
| ionize only slightly in aqueous solution. |
|
|
Term
| Acid dissociation constant (Ka) |
|
Definition
| the ratio of the concentration of the dissociation (or ionized) form of an acid to the concentration of the undissociated (nonioinized) form. |
|
|
Term
|
Definition
| dissociate completely into metal ions and hydroxide ions in aqueous solution. |
|
|
Term
|
Definition
| react with water to form the hydroxide ion and the conjugate acid of the base. |
|
|
Term
| Base dissociation constant (Kb) |
|
Definition
| the ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of the base. |
|
|
Term
| What are the products of the reaction of an acid with a base? |
|
Definition
| in general, the reaction of an acid with a base produces water and one of a class of compounds called salts. |
|
|
Term
| What is the endpoint of a titration? |
|
Definition
| the point of neutralization is the end point of the titration. |
|
|
Term
|
Definition
| reactions in which an acid and a base react in an aqueous solution to produce a salt and water. |
|
|
Term
|
Definition
| when the number of moles of hydrogen ions equals the number of moles of hydroxide ions. |
|
|
Term
|
Definition
| the process of adding a known amount of solution of known concentration to determine the concentration of another solution. |
|
|
Term
|
Definition
| the solution of known concentration. |
|
|
Term
|
Definition
| the point at which the indicator changes color. |
|
|
Term
| When is the solution of a salt acidic or basic? |
|
Definition
| in general, salts that produce acidic solutions contain positive ions that release protons to water. Salts that produce basic solutions contain negative ions that attract protons from water. |
|
|
Term
| What are the components of a buffer? |
|
Definition
| a buffer is a solution of a weak acid and one of its slats, or a solution of a weak base and one of its salts. |
|
|
Term
|
Definition
| the cations or anions of a dissociation salt remove hydrogen ions from or donate hydrogen ions to water. |
|
|
Term
|
Definition
| a solution in which the pH remains relatively constant when small amounts of acid or base are added. |
|
|
Term
|
Definition
| the amount of acid or base that can be added to a buffer solution before a significant change in pH occurs. |
|
|
