Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
chapter 20 & 21
| Term | Definition |
|---|---|
| Base | Compound that produces hydroxide ions when dissolved in water |
| Hydroxide ion (OH) | water molecule that gains a hydrogen ion ecomes a positively charged hydronium ion ion (h3o) |
| self-ionization | two water molecules produces ions of water to become changed into the form of ions, as by dissolving. |
| ion product constant for water | The product of the concentrations of the hydrogen ions and hydroxide ions in water |
| acidic solution | |
| acid | compound that produces hydrogen ions when dissolved in water |
| natural solution | pH is a measure of the acidity or basicity of a solution |
| Basic solution | one in which [H+] is less than [OH-]. Therefore, the [H+] of a basic solution is less than 1.0 X 10"7M |
| Monoprotic acids | acids that contain one ionizable hydrogen such as nitric acid |
| diprotic acids | two ionizable hydrogens sulfuric acid |
| triprotic acids | phosphoric acid |
| hydrogen-ion donor | an acid according to bronsted lowry theory |
| hydrogen - ion acceptor | Any substance that is capable of becoming reduced and accepting hydrogen atoms |
| conjugate base | the particle that remains when an acid has donated a hydrogen ion oh- is the conjugate base of acid water |
| conjugate acid | the particle formed when a base gains a hydrogen ion |
| conjugate acid base pair | two substances that are related by the loss or gain of a single hydrogen ion oh- is the conjugate acid-base pair |
| amphoteric | a substance that can be act as both an acid and a base, water is amphoteric |
| Lewis acid | any substance that can accept a pair of electrons to form a covalent bond |
| Lewis base | any substance that can donate a pair of electrons to form a covalent bond |
| strong acids | an acid that is completely ionized in aqueous solution |
| weak acids | an acid that is only slightly ionized in aqueous solution |
| acid dissociation constant | the ratio of the concentration of the dissociated form of an acid to the undissociated from stronger acids have larger k values than weaker acids |
| strong bases | a base that completetely dissociates into metal ions and hydroxide ions in aqueous solution |
| weak base | a base that does not dissociated completely in aqeous solution |
| base dissociation constant | the ratio of the concentration of the dissociated form of a base to the undissocited form |
| neutralization reactions | a reaction in which an acid and a base react in an aqueous solution to produce a salt and water |
| standard solution | a solution of known concentration used in carrying out a titration |
| titration | method used to determine the concentration of a solution |
| end point | the point in a titration at which netrutrazation is achieved |
| equivalent | the amount of an acid that can give one mole of hydrogen ions |
| gram equivalent mass | the mass of one equivalent of a substance |
| normality (N) | the concentration of a solution expressed as the number of equivalents of solute in 1 litter of solution |
| equlvance point | the point in a titration at which the number of equivalents of acid and base are equal |
| ph | pH is a measure of hydrogen ion concentration |
| ph meters |
Created by:
ash26
Popular Chemistry sets