Acid-Base Equilibria Review
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| 16.1) What is an Arrhenius acid? | A substance that, when dissolved in water, increases the concentration of H+ ions.
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| 16.1) What is an Arrhenius base? | A substance that, when dissolved in water, increases the concentration of OH- ions.
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| 16.1) What are the seven most common strong acids? | HCl, HNO3, H2SO4, HBr, HI, HClO3, HClO4
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| 16.2) Can H+ and H3O+ be used interchangeably? | Yes
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| 16.2) What is a Bronsted-Lowry acid? | A species that donates H+
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| 16.2) What is a Bronsted-Lowry base? | A species that accepts H+
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| 16.2) What kind of substance can behave either as an acid or a base? | Amphiprotic
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| 16.2) What is the name for a reactant and product that differ only in the presence or absence of a proton? | Conjugate acid-base pair
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| 16.2) If an acid is very strong, will the conjugate base very strong or very weak? | Very weak
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| 16.2) If an acid is weak, is the conjugate base strong or weak? | Weak
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| 16.2) What type of acid completely transfers its protons to water? | Strong
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| 16.2) Is acetic acid a strong or weak acid, and is its conjugate base strong or weak? | Weak, Weak
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| 16.2) What is the strongest acid that can exist in equilibrium in aqueous solution? | H+
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| 16.2) What is the strongest base that can exist in equilibrium in aqueous solution? | OH-
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| 16.3) What is K sub W? | Ion-product constant
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| 16.3) Is a solution acidic, basic, or neutral if [OH-]=[H3O+]? | Neutral
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| 16.3)Is a solution acidic, basic, or neutral if [OH-]<[H3O+]? | Acidic
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| 16.3) Is a solution acidic, basic, or neutral if [OH-]>[H3O+]? | Basic
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| 16.4)What is the equation used to calculate pH? | pH=-log[H+]
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| 16.4) A pH change of 1 unit results from the [H+]changing by how many units? | 10
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| 16.4) As the pH of a solution decreases, is the acidity of the solution increasing or decreasing? | Increasing
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| 16.4) As the pH of a solution increases, is the acidity of the solution increasing or decreasing? | Decreasing
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| 16.4) What is the equation used to calculate pOH? | pOH=-log[OH-]
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| 16.5)Are strong acids strong electrolytes or weak electrolytes? | Strong
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| 16.5) What are the most common strong bases? | Ionic hydroxides of the alkali metals and heavier alkaline metals
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| 16.6) What is K sub a? | Acid-dissociation constant
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| 16.6) If (K sub a)>>1, is the acid very strong or very weak? | Very strong
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| 16.6) What type of acid has more than one ionizable proton? | Polyprotic
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| 16.7) What is K sub b? | Base-dissociation constant
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| 16.7) If (K sub b)>>1, is the base very strong or very weak? | Very strong
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| 16.8) Which equation relates Ka, Kb, and Kw? | Ka*Kb=Kw
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| 16.9) Are salts generally strong or weak electrolytes? | Strong
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| 16.11) What is a lewis acid? | Electron pair acceptor
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| 16.11) What is a lewis base? | Electron pair donor
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