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
Chemistry Unit 9
Unit 9: Acids & Bases
| Term | Definition |
|---|---|
| Molarity | The number of moles of solute dissolved in total liters of solution (expressed in units of mol/L or M) |
| Acid Characteristics | Sour Tasting, Turn litmus paper red, Neutralize bases, Solutions conduct electricity, React with many metals to produce H2 gas, React with carbonates to produce CO2 gas, Solutions are colorless in presence of phenolphthalein indicator |
| Base Characteristics | Bitter Tasting, Turns litmus paper blue, Neutralizes acids, Solutions conduct electricity, Feels slippery (dissolve fatty acids on fingers to form soap molecules), Solutions are pink in presence of phenolphthalein indicator |
| Acids (Bronsted-Lowry Model) | Donate protons (H+) |
| Bases (Bronsted-Lowry Model) | Accept protons |
| Conjugate Base (Bronsted-Lowry Model) | What's left of the acid after it has donated a proton |
| Conjugate Acid (Bronsted-Lowry Model) | What's formed after the base has accepted a proton |
| Amphoteric Substance | May act as an acid or base Ex: H2O |
| Form Ions | H2O reacts with other H2Os |
| Brackets | Around a species represents concentration in molarity (M) |
| Kw | The water dissociation constant |
| pH | "power of the Hydrogen ion". The pH scale is a logarithmic scale based on the power of 10 (log10) |
| Sig Figs | The number of decimal places in the log is equal to the number of significant figures in the original number. |
| Strong Acids | Acids that dissociate nearly completely |
| Weak Acids | Acids that do not dissociate to great extent |
| pOH | "power of the hydroxide ion" |
| Acid-Base Titration | Procedure used to determine the concentration of an acid or base of using a standard acid or base |
| Standard Solution | Solution whose concentration is known precisely. A standard solution is used to neutralize an acid/base of unknown concentration. (acid + base -> H2O + salt (ionic) |
| Equivalence Point | Point in a titration where mol H+=mol OH- (neutralization). Equivalence point can be detected using an acid-base indicator. |
| Indicators | Indicators change the color at certain pH levels. For phenolphthalein: pink when pH>8, colorless when pH<8. Different indicators have different endpoints. |
| Endpoint | Point in titration where the indicator changes color |
| Titration Calculations | Concentration of unknown acid/base is determined using the formula CaVa/CbVb=a/b |
Created by:
sara!
Popular Chemistry sets