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