Flashcard library · Chemistry
AP Chemistry: Acids & Bases
Master the fundamentals of acids and bases with this comprehensive flashcard set designed for AP Chemistry students. This deck covers essential definitions, calculations, and core concepts like pH, pOH, titrations, buffers, and strong vs. weak acids/bases. Sharpen your understanding for exams and problem-solving success!
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What is the Brønsted-Lowry definition of an acid?
A Brønsted-Lowry acid is a species that donates a proton (H+).
What is the Brønsted-Lowry definition of a base?
A Brønsted-Lowry base is a species that accepts a proton (H+).
Identify the conjugate base of H2SO4.
The conjugate base of H2SO4 is HSO4- (by losing one H+).
Identify the conjugate acid of NH3.
The conjugate acid of NH3 is NH4+ (by gaining one H+).
Name three common strong acids.
Common strong acids include HCl, HBr, HI, HNO3, H2SO4, and HClO4.
How does the strength of an acid relate to the strength of its conjugate base?
A strong acid has a very weak conjugate base, while a weak acid has a relatively stronger conjugate base.
What is the value of the autoionization constant of water (Kw) at 25°C?
At 25°C, Kw = 1.0 x 10^-14.
If the pH of a solution is 3.5 at 25°C, what is its pOH?
Since pH + pOH = 14 at 25°C, the pOH is 14 - 3.5 = 10.5.
How is the pH of a strong monoprotic acid solution calculated?
For a strong monoprotic acid, [H+] is equal to the initial acid concentration, so pH = -log[H+].
What is a buffer solution?
A buffer solution is a mixture of a weak acid and its conjugate base (or a weak base and its conjugate acid) that resists significant changes in pH upon the addition of small amounts of strong acid or base.
State the Henderson-Hasselbalch equation.
The Henderson-Hasselbalch equation is pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the weak acid.
Describe the equivalence point in an acid-base titration.
The equivalence point is reached when the moles of added titrant (acid or base) exactly neutralize the moles of the substance being titrated. The pH at this point depends on the strengths of the acid and base involved.
How does electronegativity affect the strength of oxyacids with the same number of oxygen atoms?
For oxyacids with the same number of oxygen atoms, acid strength increases with increasing electronegativity of the central atom because it more effectively pulls electron density away from the O-H bond, making it more polar and easier to ionize.
What is the relationship between Ka and Kb for a conjugate acid-base pair?
For a conjugate acid-base pair, Ka × Kb = Kw, where Kw is the autoionization constant of water.
What happens to the pH when a salt formed from a strong acid and a weak base dissolves in water?
The cation from the weak base will hydrolyze water to produce H3O+, making the solution acidic (pH < 7).