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Chem110 Test 8 rev
Chemistry 110 Deltech Owens Test 8 Review
| Question | Answer |
|---|---|
| Name 2 theories of acids and bases. | Arrhenius and Bronsted-Lowry theory |
| An Arrhenius acid is defined as... | a substance that dissociates in water to form hydrogen ions. (H+) |
| What kind of acid is HCl? | an Arrhenius acid, also a strong acid |
| An Arrhenius base is defined as... | a substance that dissociates in water water to form hydroxide (OH-) ions. |
| NaOh is what kind of base? | an Arrhenius base |
| What is an acid? | a substance that dissociates to produce hydrogen ions when dissolved in water. |
| Acids are proton _. | donors |
| A substance with a pH value less than _ is an acid. | 7 |
| What is a base? | a substance that dissociates to produce hydroxide ions when dissolved in water. |
| Bases are proton _. | acceptors |
| A substance with a pH value of more than _ is a base. | 7 |
| The range of pH values is _ | 0-14 |
| Acids have the following qualities: | sour taste, dissolve metals, cause plant dye to change color |
| Bases have the following qualities: | bitter tasted, slippery, corrosive |
| Bleach is a _ | base |
| The strength of a base or acid is really a measure of __ | disassociation--the more it disassociates, the stronger it is. |
| Chemical formulas that start with an H are usually __ | acids |
| Chemical formulas that end with an H are usually __ | bases (most end with OH) |
| A strong acids reaction with water is about _%. | 100 |
| Acids and bases are both _ | electrolytes |
| An example of a strong acid includes | HNO3 (nitric acid), HCl (hydrochloric acid) |
| An example of a weak acid includes | HF (hydrogen fluoride), H2S (hydrogen sulfide), C2H4O2 (acetic acid) |
| Methaline (CH3NH2) is a __ __ | weak base |
| An example of a strong base includes | NaOH (sodium hydroxied) |
| Ionization is | the dissociation of acids and bases |
| Amphiprotic refers to | a substance that is both a proton acceptor and a donator (a substance with the qualities of both an acid and a base is technically amphoteric) |
| A conjugate acid is | what the base becomes after it accepts a proton |
| A conjugate base is | what the acid become after it donates a proton |
| Which side of an equation are conjugate bases and acids written on? | the right |
| A conjugate acid-base pair is | the acid and base on opposite sides of a solution |
| pH scale measures | the acidity or basicity of a solution |
| What unit does the pH scale use? | it is unitless |
| The pH scale is defined as | pH = -log[H3O+] |
| A neutralization reaction is | the reaction of an acid with a base that produces salt and water |
| Titration is | adding a measured amount of a standard solution to a 2nd, unknown solution to neutralize the solution |
| A standard solution is | a solution of known concentration |
| An indicator is | a substance which changes color as pH changes. |
| A buret | is a long glass tube calibrated in mLs that contains a standard solution |
| A polyprotic substance | donates or accepts more than one proton per formula unit |
| A diprotic substance | donates or accepts 2 protons per formula unit; note that diprotic solutions are also polyprotic |
| A monoprotic substance | donates or accepts 1 proton per formula unit |
| Is sulfuric acid (H2SO4) diprotic or monoprotic? | diprotic |
| Is HCl (hydrochloric acid) polyprotic or monoprotic? | monoprotic |
| A buffer solution | is a solution that resists large changes in pH when an acid or base is added |
| Buffers establish an __ between conjugate acid-base pairs. | equilibrium |
| LeChatelier's Principle is a | buffer in action. |
| Buffer capacity is a | measure of a solution's ability to resist large changes in pH when a strong acid or base is added |
| Oxidation, as it relates to oxidation-reduction processes, is | a loss of electrons, loss of hydrogen atoms, a gain of oxygen (EHO - Lose Oxygen/more losses than gains) |
| Reduction, as it relates to oxidation-reduction processes, is | a gain of electrons, gain of hydrogen atoms, a loss of oxygen |
| Corrosion is | the decay of metals caused by oxidation-reduction processes |
| An example of corrosion is | rust |
| A voltaic cell | is an electrochemical cell that converts stored chemical energy into electrical energy |
| An anode is | the electrode where oxidation occurs in a voltaic cell |
| A cathode is | the electrode where reduction occurs in a voltaic cell (Cathy loses weight; cathode=reduction) |
| An electrolysis reaction is | a nonspontaneous oxidation-reduction reaction that's driven by an electric current |
| __ __ are rechargeable. | electrolitic cells |
| A reducing agent is the | substance that donates an electron to another species in a reduction-oxidation reaction |
| An oxidizing agent is the | substance that accepts an electron from another species during a reduction-oxidation reaction |
| A reducing reaction is a | half-reaction where a chemical species decreases its oxidation number. |
| In a reducing reaction, the electron (e-) will on which side of the arrow? | right |
| In an oxidizing reaction, the electron (e-) will on which side of the arrow? | left |
| An oxidizing reaction is a | half-reaction where a chemical species increases its oxidation number |
| Hydrogen ions are called | protons |
| Reversible arrows mean | the acid or base in the formula is weak and therefore reversible |
| Single direction arrows mean | the acid or base in the formula is strong and therefore irreversible |
| H3O+ is called an | hydronium ion |
| Kw is the | ion product for water |
| The Henderson-Hasselbach equation is: | pKa=pH - log (formulas) |
| Respiration is | an electron-transport chain that uses reversible oxidation and reduction of iron atoms in cytochrome c |
| Metabolism is | the break down of molecules into smaller pieces by enzymes |
| Spectator ions | are the parts of a net ionic equation that remain unchanged |
| If hydronium (H3O+) is present on the far right of the equation, then the chemical at the opposite end (the far left) must be a | weak acid |
| If hydroxide (OH-) is present on the far right of the equation, then the chemical at the opposite end (the far left) must be a | weak base |
| Any molecule that loses, or donates, an electron in an equation is | an acid |
| Any molecule that gains, or accepts, an electron in an equation is | a base |
| The acid on the left of an equation will be the __ on the right side. | conjugate base |
| The base on the left side of an equation will be the __ on the right side. | conjugate acid |
| The negative superscript number in an equilibrium expression tells us the __ of the substance. | concentration |
| The negative superscript number in an ion product of water (Kw) expression tells us the __ of the substance. | pH value |
| If you add an acid to a solution, the pH goes | down |
| If you add a base to a solution, its pH goes | up |
| A net ionic equation is written with only the __ __ showing. | changed components |
| In an equilibrium constant solution, __ go over __. | products go over reactants (or substances on the right side of the arrow get written above those on the left) |
Created by:
IsaacJ
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