Inorganic Chemistry – Acids & Bases, Solubility, Trends in Periodic Table – Flashcards
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Relationship between pH and pOH?
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pH + pOH = 14
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Relationship between pKa & pKb?
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pKa + pKa = 14
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Relationship between Ka & Kb?
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Ka*Kb = Kw
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Acid dissociation constant
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K_a = [H+][A-]/[HA]
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Base equilibrium constant
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K_b = [OH-][BH+]/[B]
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Strong acids/bases have:
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high K's and small pK's
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Roots of polynomial equation:
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x = (-b +/- (b^2 - 4ac)^(1/2))/2a
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Henderson Hasselbach equation
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pH = pK_a + log([A-]/[HA])
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Solubility: The solubility of most solids ????? with an increase in temperature.
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increases
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Solubility: The solubility of most gases ????? with an increase in temperature.
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decreases
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Solubility: The solubility of most solids/liquids ????? with an increase in pressure.
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does not change
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Solubility: The solubility of most gases ????? with an increase in pressure.
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increases
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Henrys Law Equation
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P = k_h*X
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Henrys Law Definition
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the amount of gas dissolved in a solution is directly proportional to the pressure of THE gas above the solution
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Trends in Atomic Size: 1) Going down a group (next Period) & 2) Going across a period
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increase, decrease
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Trends in Ionization Energy: 1) Going down a group (next Period) & 2) Going across a period
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decrease, increase
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Trends in Electron Affinity: 1) Going down a group (next Period) & 2) Going across a period
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decreases (generally), increases (many exceptions)
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Trends in Electronegativity: 1) Going down a group (next Period) & 2) Going across a period
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decrease, increase
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Trends in Metallic Character: 1) Going down a group (next Period) & 2) Going across a period
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increase, decrease
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Definition: Ionization Energy
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energy required to remove highest energy electron from atom or ion in gaseous state
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Definition: Electron affinity
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energy change associated with the addtion of an electron to a gaseous atom
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Definition: Electronegativity
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the ability of a atom in a molecule to attract shared electrons to itself
