Exam 4 Random Things to Remember

Front

When you use the 5% rule, what MUST you do?

Back

Check that x/initial concentration is <5%! Don't forget to show this or you will lose points

Front

For relative strength of binary acids, which trend do you use?

Back

Atomic size (NOT electronegativity)

Front

As atomic size increases, acid strength __________.

Back

increases

(this makes sense because bigger atoms have more electrons, which makes the H--A bond longer and weaker, which makes it easier to lose a proton, which makes the acid stronger)

Front

When determining the relative strength of oxyacids, which trend should you use?

Back

increasing electronegativity (NOT atomic size) increases acid strength

Front

How do convert between Ka and Kb

Back

Kw = Ka(Kb)

Front

True or false: you can make a buffer with HNO₃/NaNO₃

Back

false

This is a strong acid/base conjugate. A buffer has to be with a weak acid/base conjugate

Front

The pH at the equivalence point is =7, >7, and <7 when....

Back

=7 when it's a strong acid and strong base

>7 when it's a weak acid and strong base. This makes sense because the base dominates

<7 when it's a weak base and strong acid. This makes sense because the acid dominates

Front

HClO₄ + H₂O (--> or <-->) ClO_4^- + H₃O⁺

Back

-->

strong acids or bases ionize fully. Equilibrium arrows are for weak acids or bases.

Front

What are the strong acids

Back

HClO₄

HCl

HBr

HI

HNO₃

H₂SO₄

Front

What are the strong bases

Back

LiOH

NaOH

KOH

Ca(OH)₂

Sr(OH)₂

Ba(OH)₂