0.55

1.82

5.56

0.18

Increase by one

Increase tenfold

Decrease by one

Decrease tenfold

Colloidal

Buffer action

Acidity

Salt balance

0.2 M $NH_4OH$ and 0.1 M $NH_4Cl$

0.1 M Triethylamine and 0.1 M Triethylammonium chloride

0.1 M $CH_3COOH$ and 0.1 M $NaOH$

0.1 M $NH_3$ and 0.1 M $NH_4NO_3$

${\rm{pOH}} = {\rm{p}}{K_b} + \log \frac{{\left[ {{\rm{Conjugate\; acid}}} \right]}}{{\left[ {{\rm{\;Base}}} \right]}}$

${\rm{pOH}} = {\rm{p}}{K_b} - \log \frac{{\left[ {{\rm{Conjugate\; acid}}} \right]}}{{\left[ {{\rm{\;Base}}} \right]}}$

${\rm{pOH}} = {\rm{p}}{K_b} + \log \frac{{\left[ {{\rm{Base}}} \right]}}{{\left[ {{\rm{Conjugate\; acid}}} \right]}}$

${\rm{pOH}} = {\rm{p}}{K_b} - \log \frac{{\left[ {{\rm{Base}}} \right]}}{{\left[ {{\rm{Conjugate\; acid}}} \right]}}$

Increases

Decreases

Remains unchanged

Not predictable

0.1 mol $NH_3$ + 0.1 mol $NH_4Cl$ in 1 L of water

0.1 mol $HCl$ + 0.1 mol $NaOH$ in 1 L of water

0.1 mol $CH_3COOH$ + 0.1 mol $CH_3COONa$ in 1 L of water

0.1 mol $HCl$ + 0.1 mol $NH_3$ in 1 L of water

HA (the weak acid)

NaA (the sodium salt)

Water (H2O)

Hydroxide ions (OH-)

[A$^-$] = [HA]

[A$^-$] < [HA]

[A$^-$] > [HA]

HA is a strong acid

Not a buffer solution with pH < 7

Not a buffer solution with pH > 7

A buffer solution with pH < 7

A buffer solution with pH > 7

$2 imes {10^{ - 4}}$

$3.7$

$2.7$

$1.85$