| Term | Definition |
|---|
| It is a measure of how much solute will dissolve into the solvent | Solubility |
| Solutions of acids, bases, and salts contain mobile ions and conduct electricity are called | What are electrolytes? |
| They are ionic compounds that dissociate in water | What are Salts? |
| They are actually molecular compounds (covalently bonded) the become ions when dissolved in water | Acids |
| the formation of two new combinations of ions. | The double replacement or metathesis reaction can be defined as |
| low solubility (precipitate forms), weak electrolyte, gas formation, or complex ion formation. | In a metathesis reaction, the products may be more stable than the original due |
| The ionic equation | This type of chemical equation shows strong electrolytes as separate ions |
| The net equation | This type of chemical equation eliminates "spectator ions". |
| A substance that increases the [H+] in solution | According to Arrhenius the definition of an Acid is |
| Asubstance that increases the [OH–] in solution. | According to Arrhenius the definition of a base |
| Have more than one removable H ion (H2SO4) | Diprotic acids |
| the H+ and OH– ions form the very weak electrolyte... H2O (and a salt) | Acids and bases neutralize each other because |
| Are the partially neutralized polyprotic acids. NaH2PO4 or Na2HPO4 or NaHSO4, etc... solid acids. | Acid salts |
| A proton (H+) donor. | Definition of an acid according to Bronsted and Lowry |
| A proton acceptor. | Definition of a Base according to Bronsted and Lowry |
| H2SO4 | Best example of a Diprotic acid |
| The solubility will be INCREASED as the temperature is increased | If the solution process absorbs energy then |
| The solubility will DECREASE with increasing temperature | If the solution process releases energy then |
| The less soluble the substance will be | The larger the molecule or the higher its molecular weight |
| The larger the branching will reduce the size (or volume) of the molecule and make it easier to solvate the molecules with solvent. | In the case of organic compounds the amount of carbon "BRANCHING" will increase the solubility because |
| In polar solvents | Generally polar solute molecules will dissolve |
| In non-polar solvents | non-polar solute molecules will dissolve |
| Then positive ends of solvent molecules will attract negative ends of solute molecules | If the solvent molecule is also polar |
| Are always soluble. | Salts of ammonium (NH4 +) and Group IA |
| AgCl, Hg2Cl2, and PbCl2 | All chlorides (Cl-) are soluble Except |
| AgBr, Hg2Br2, HgBr2, and PbBr2 | All bromides (Br-) are soluble Except |
| AgI, Hg2I2, HgI2, and PbI2 | All iodides (I-) are soluble except |
| Are soluble | Chlorates (ClO3 -), nitrates (NO3 -), and acetates (CH3COO-) are |
| CaSO4, SrSO4, BaSO4, Hg2SO4, HgSO4, PbSO4, and Ag2SO4 | Sulfates (SO4 -2) are soluble except |
| NH4 + and Group IA compounds. | Phosphates (PO4 -3), and carbonates (CO3 -2) are insoluble except |
| NH4 + and Group IA compounds. | All metallic oxides (O-2) are insoluble except |
| NH4 + and Group IA and Group IIA from calcium down. | All metallic hydroxides (OH-) are insoluble except |
| NH4 + and Groups IA and IIA. | All sulfides (S-2) are insoluble except |
| Are oxides such as (SO3, CO2, N2O5) whose aqueous solutions contain H3O+ | Acidic Anhydrides |
| Soluble metal oxides as (NaOH, Ca(OH)2) react with water to form the hydroxide ion | Basic Anhydrides |
| Are strong electrolytes because they completely dissociate in water | Strong Acids |
| Are weak electrolytes because just a small percentage of the acid dissociates | Weak Acids |
| Are metal hydroxides because they have high solubility | Strong Bases |
| Are molecular bases (ammonia) because they have a low percentage ionization | Weak Bases |
| Water (H2O) | Neutralization of Strong acids-bases yields |
| Water (H2O) and a salt | Neutralization of a weak acid and strong base yields |
| the base salt | Neutralization of a strong acid and weak base yields |
| Ammonium ion | The net ionic equation of ammonia and hydrochloric acid yields |
| water and carbon dioxide | Decomposition of Carbonates and Bicarbonates yields |
| An analytical procedure in which a solution of unknown concentration is combined slowly with a standard solution until a colour change of some indicator | Titration |
| The solution added from a buret during a titration | Titran |
| is a dye that has one colour in an acid solution and a different colour in a basic solution | Acid-base indicator |
| When, during titration, the colour of the solution change | End Point |
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