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39 Cards in this Set
- Front
- Back
Homogeneous vs Heterogeneous equilibrium
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homo- all same state (gases, aqueous) |
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Relationship between Kc and Kp
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Kp=Kc(RT)^deltan |
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Arrhenius definition of Acid and Base
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Acid: a substance, that when dissolved in water, increases the concentration of hydrogen ions (H+) |
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Bronsted-Lowry definition of Acid and Base
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Acid: a proton donor |
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What happens when an acid dissolved in water
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Water acts as a Bronsted-Lowry base and abstracts a proton (H+) from the acid |
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Strong vs Weak Acids
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-Strong acids are completely dissociated in water (create incredibly weak bases- almost negligible) |
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How does acid/base strength affect eh side of equilibrium a reaction favors
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Equilibrium favors the reaction that moves the proton to a stronger base |
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What is amphiprotic and give examples |
molecule that can be either an acid or base |
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What is the autoionization of water
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in pure water a few molecules will dissociate to act as acids or bases forming OH and H30
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Ion Product Constant of Water |
equilibrium expression for the autoionization of water |
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what is pH
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the negative base-10 logarithm for the concentration of hydronium ion |
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using "p" scales |
the p in pH stants for negative base-10 log |
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using pH to determine acid or base |
in pure water, pH=7 |
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How do [H+] and [OH-] compare in acidic and basic solutions |
neutral: [H+] = [OH-] |
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How do logarithms affect significant figures
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-when taking the log, use as many digits to the right of the decimal as significant figures in the original |
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what is pKw |
-log (Kw) |
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converting between [OH-] [H+] pOH and pH |
two options |
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Characteristivs of a strong acid
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strong electrolytes
exist totally as ions in aqueous soultions |
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What are the Seven Strong Acids |
HCl |
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finding the pH of a monoprotic acid |
in a monoprotic (one H) acid, the [H+] is the same as the concentration of the acid |
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characteristics of a strong base |
strong electrolytes |
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what are the strong bases? |
- alkali metal hydroxides (far left row of periodic table) |
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finding the pH of a strong base |
the pH of a strong base aqueous solution can be determined using the concentration of the strong base |
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Dissociation Constants
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Ka and Kb |
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Calculating percent ionization
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percent ionization = [H3O+] at equilibrium/ [Hacid] inital x100
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relationship between Ka and Kb |
Ka * Kb= Kw (if you know one you can calculate the other) |
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Reactions of cations and anions with water |
Anions (negative charge) are bases- will form OH and a conjugate acid |
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Effect of Cations and Anions on pH |
-an anion that is the conjugate base of a strong acid will not affect the pH |
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Factors affecting the Strength of Acids |
1. larger the Ka- the stronger the acid |
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Binary Acids
Oxyacids Definitions |
Binary Acids: Basic Formula HA (H is hydrogen and A is other element or ion) |
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Definition of Lewis Acid and Base
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Lewis Acid: an electron pair acceptor *must have empty valence orbital |
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The Common-Ion Effect
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in a solution where two parts share a common ion (usually H) the H3O may take the concentration of that ion |
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Buffer
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a solution that resists a change in pH when a small amount of acid or base is added |
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Henderson-Hasselbalch Equation
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used to find the pH of a buffer |
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Buffer capactity
Buffer pH range |
the amount of acid or base a buffer can neutralize before the pH begins to change |
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Titration |
a known concentration of base (or acid) is slowly added to a solution of acid (or base) |
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Factors affecting Solubility |
-pH: if a substance is a basic anion it will be more soluble in an acidic solution, if a substance is an acidic cation it will be more soluble in a basic solution |
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Will a precipitate form if
Q=Ksp QQ>Ksp |
Q=Ksp: at equilibrium and solution is saturated |
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Fundamental of Acid-Base Equilibria
(4 types of acid-base equilibria) |
1. Dissociation of a weak acid |