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Solutions Acids Base
| Question | Answer |
|---|---|
| Solution | a homogeneous mixture |
| Solute | the substance being dissolved; the substance of which there is less |
| Solvent | the substance that is doing the dissolving; the substance of which there is more |
| Colloid | a mixture of medium-size particles that do not settle out; the particles can scatter a light beam |
| Suspension | a heterogeneous mixture of large particles that will settle out if not stirred |
| Tyndall Effect | the observed scattering of light when shone through a colloid |
| How to tell the difference between a solution and a colloid | use the Tyndall Effect |
| How to tell the difference between a colloid and a suspension | filter them; the particles in a colloid will go through the filter paper; the particles in a suspension will be captured |
| Miscible | two liquids that can be mixed in any proportion, example: alcohol and water |
| Immiscible | two liquids that cannot be mixed in any proportion; example: oil and water |
| Like Dissolves Like | substances with the same polarity are soluble in each other; water is a polar solvent, CCl4 is a nonpolar solvent; alcohols can dissolve in both; ionic substances are treated like polar substances |
| Polar Molecule | a molecule with a dipole (positive and negative difference) |
| Polarity of Water | water is polar |
| Solubility | measures the amount of solute that can be dissolved in a given amount of solvent at a specific temperature |
| Solubility of a solid | solubility increases as temperature increases; pressure does not affect a solid’s solubility |
| Solubility of a gas | solubility decreases as temperature decreases; an increase in pressure can increase a gas’s solubility |
| Soluble | can be dissolved |
| Unsaturated solution | more solute can be dissolved |
| Saturated solution | the maximum amount of solute is dissolved |
| Supersaturated solution | more than the maximum amount of solute is dissolved |
| Solubility curve | a graph that plots the saturated solutions at a given temperature; grams per 100g of water |
| Homogeneous mixture | mixture with no visible differences |
| Heterogeneous mixture | mixture with visible differences |
| Dissolution | the process of being dissolved |
| Three ways to increase the rate of dissolution of a solid | heat, agitate(stir or shake), crush the solute |
| Why does heating increase the rate of dissolution | heat with increase the kinetic energy of the solvent particles; the more energy particles hit the solute harder and more often thus breaking it apart faster |
| Why does crushing increase the rate of dissolution | crushing a substance increases the surface area which is where the dissolving is going on |
| Why does stirring increase the rate of dissolution | it brings fresh solvent in contact with the solute’s surface |
| Dissociation/Ionization Equations | equation that shows how a solid breaks apart into ions when dissolved in water; example: KOH K+ + OH- |
| Net Ionic Equation | an equation that shows the ions that form the precipitate in a double-replacement reaction; example: Pb2+(aq) + S2-(aq) PbSO4(s) |
| Electrolyte | a solution of ions that can conduct an electric current |
| Nonelectrolyte | a solution with no ions; it cannot conduct an electric current |
| Strong electrolyte | a substance that dissociates 100%; it can conduct a strong electric current |
| Weak electrolyte | a substance that does not dissociate 100%; it can conduct a weak electric current |
| Properties of Acids | electrolyte, taste sour, turn litmus paper red, react with metals to form hydrogen gas, react with bases to form a salt and water |
| Properties of Bases | electrolyte, taste bitter, turn litmus paper blue, feel slippery, react with acids to form a salt and water |
| Arrhenius Acid | a substance that increases the hydrogen ion concentration; must contain H |
| Arrhenius Base | a substance that increases the hydroxide ion concentration; must contain OH |
| Bronsted-Lowery Acid | a substance that can donate a proton; must contain H |
| Bronsted-Lowery Base | a substance that can accept a proton; includes OH or a negative charge |
| Proton | a hydrogen ion |
| [H+] | hydrogen ion concentration |
| [OH-] | hydroxide ion concentration |
| Hydronium ion | H3O+ |
| Self-ionization of water | H2O + H2O OH- + H3O+ |
| Conjugate pair | two substances that differ by one hydrogen; the substance with more hydrogens is the conjugate acid and the other is the conjugate base |
| NH4+ and NH3 | NH4+ is an acid; NH3 is a base |
| Amphoteric substance | a substance that can act as an acid or a base (according to Bronsted-Lowery); usually has hydrogen and a negative charge; water is amphoteric; |
| Concentration | measures the amount of solute dissolved in the solvent |
| Weak/Strong Concentration | weak concentrations are dilute solutions; strong concentrations are concentrated solutions |
| Strong Acid/Base | an acid or base that dissociates completely; it’s a strong electrolyte; this is not related to being a strong concentration; strength is measured with an ionization constant (Ka); larger numbers (smaller exponents) are stronger acids |
| Weak Acid/Base | an acid or base that does not dissociate completely; it’s a weak electrolyte; this is not related to being a weak concentration; strength is measured with an ionization constant (Kb); larger numbers (smaller exponents) are weaker acids |
| Ionization constant | K; measures the degree to which a substance dissociates; larger numbers (small exponents) dissociate more |
| Polyprotic acid | an acid with more than one hydrogen; example: H2CO3 |
| Molarity | moles per liter; measures concentration |
| Molarity by Dilution | M1V1=M2V2 |
| pH | equation is –log[H+]; used to determine if a substance is an acid, base or neutral |
| pOH | equation is –log[OH-] |
| pH scale | acids have a pH less than 7; bases have a pH greater than 7; neutral is 7; scale ranges from 0 to 14 |
| pH+pOH | pH + pOH |
| How to find concentration given pH | the molarity equals 10 raised to the –pH |
| Sig figs for pH | the number of sig figs in the concentration equals the number of decimal places in the pH |
| Neutralization Reaction | acid + base --> salt + water; example: HF + KOH --> KF + H2O |
| Titration | a process that determines the concentration of an unknown acid |
| Salt | any ionic substance that can be formed from a neutralization reaction |
| Indicator | a chemical that changes its color based on the pH |
| Phenolphthalein | an indicator that is clear in an acid and pink in a base |
| Acid Names | ide is hydro__ic acid; ite is __ous acid; ate is ___ic acid |
| strong acids will have ____ conjugate bases | weak |
| weak acids will have ___ conjugate bases | strong |
| strong bases will have ____ conjugate acides | weak |
| weak bases will have ___ conjugate acids | strong |
Created by:
ehsanip
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