16.1 Flashcards
An acid is a substance that, when…
dissolved in water, increases the concentration of H+ ions.
A base is a substance that, when…
dissolved in water, increases the concentration of OH- ions.
An acid is a…
proton donor
A base is a…
proton acceptor
Water is amphiprotic. What does this mean
It can act as a base and an acid depending on the equation
In an equation, Acid turns into …
Base to…
Acid to … conjugate base (conjugate base loses an H compared to acid)
Base to…conjugate acid (conjugate acid gains an H compared to base)
Stronger acid + Stronger base =
Weaker base + weaker acid
Weaker acid + Weaker base =
stronger acid + stronger abse
Water is amphoteric.
In pure water, a few molecules act as bases and a few act as acids.
This is referred to as…
autoionization
- If a solution is neutral…
- If a solution is acidic…
- If a solution is basic…
- [H+] = [OH-]
- [H+] > [OH-]
- [H+] < [OH-]
Two ways to measure pH is with a…
pH meter
pH meters are used for accurate measurement of pH; electrodes indicate small changes in voltage to detect pH.
Another method is with indicators.
They give less accurate, but quick measurements.
An indicator is a compound that has one color in its acid form and another color in its basic form.
The larger the value of Ka…
The stronger the acid
Polyprotic acids have more than…
one acidic proton.
It is always easier to remove the first proton than any successive proton.
Salts are…
by-products of neutralization reactions.
They can be made by many other reactions.
The main product of the neutralization reaction is water.
Salts are
ionic compounds and many ions are acidic or basic!
The cation can be…
acidic or neutral.
The anion can be…
acidic, basic, or neutral.
Anions of strong acids (conjugate bases of strong acids) are…
neutral
Anions of weak acids (conjugate bases of weak acids) are…
basic
Transition and post-transition metal cations are…
acidic
Polyatomic cations are typically…
the conjugate acids of a weak base, so they are acidic (ex. NH4+)
In the period, polarity is more important, as the electronegativity of A increases…
Acid strength increases
Two contributions to H-A strength
H—A bond polarity: H-A bond must be polarized with δ+ on the H atom and δ– on the A atom.
Bond strength: weaker H-A bonds can be broken more easily, making the acid stronger.
In the group, bond strength is more important, going down in the group…
acid strength increases (longer bonds are weaker).
- Oxyacids consist of…
- Generally, as the electronegativity of the nonmetal (X) increases
- H, O, and one other element, which typically is a nonmetal.
- the acidity increases for acids with the same structure.
Oxyacids:
If the oxidation number increases…
the acidity increases
Carboxylic acids are…
organic acids containing the —COOH group
A Brønsted–Lowry (B-L) acid must have
at least one removable (acidic) proton (H+) to donate.
A Brønsted–Lowry (B-L) base
must have at least one nonbonding pair of electrons to accept a proton (H+).
