Equilibrium constants, Le Chatelier, pH, buffers, Ksp, titration curves and thermodynamics of reactions.
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- What does the equilibrium constant K express?
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The ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients, at equilibrium.- How does K relate to the direction of a reaction?
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K > 1 favors products; K < 1 favors reactants; K = 1 means neither is favored.- What is the difference between Kc and Kp?
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Kc uses molar concentrations in solution or gas phase; Kp uses partial pressures of gases only.- How is Kp related to Kc?
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Kp = Kc(RT)^(delta n), where delta n is the change in moles of gas.- What is Ka?
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The acid dissociation constant, expressing the equilibrium for a weak acid donating a proton.- What is Kb?
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The base dissociation constant, expressing the equilibrium for a weak base accepting a proton.- State Le Chatelier's principle.
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When a system at equilibrium is disturbed, it shifts to counteract the disturbance and restore equilibrium.- How does increasing pressure affect a gaseous equilibrium?
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The system shifts toward the side with fewer moles of gas.- How does increasing temperature affect an exothermic reaction at equilibrium?
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The equilibrium shifts toward reactants, favoring the endothermic direction.- How does a catalyst affect the equilibrium position?
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A catalyst does not change the equilibrium position; it only speeds up how fast equilibrium is reached.- What is pH?
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The negative logarithm of hydrogen ion concentration: pH = -log[H+].- What is the relationship between pH and pOH?
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pH + pOH = 14 (at 25 degrees Celsius in aqueous solution).- What is a neutral solution's pH at 25 degrees Celsius?
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pH = 7 ([H+] = 10^-7 M).- How do you calculate [H+] from pH?
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[H+] = 10^-pH.- What does it mean when a weak acid has a small Ka?
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The weak acid poorly dissociates, so it remains mostly un-ionized in solution.
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