Acids and Bases

Accepts a proton

Donates a proton

Accepts an electron pair

Donates an electron pair

$PO_4^{3-}$

$HCO_3^-$

$CO_3^{2-}$

$HCl$

$SO_4^{2-}$

$H_2SO_4$

$OH^-$

$SO_3^{2-}$

$O_2$

$H_2$

$CO_2$

$Cl_2$

A substance that produces $OH^-$ ions in aqueous solution

A proton ($H^+$) acceptor

An electron pair donor

A proton ($H^+$) donor

Oxygen

Carbon dioxide

Hydrogen

Sulfur dioxide

$1.0 \times 10^{-5}$

$1.0 \times 10^{-9}$

$5.0 \times 10^{-1}$

$1.0 \times 10^{-14}$

0.0

1.0

14.0

7.0

It increases by a factor of 2

It decreases by a factor of 2

It decreases by a factor of 100

It increases by a factor of 100

$CH_{3}COOH$

$H_{3}PO_{4}$

$HF$

$HCl$

The weak acid will cause the bulb to glow more brightly than the strong acid.

The strong acid will produce no gas at the electrodes.

The strong acid will cause the bulb to glow more brightly than the weak acid.

Both solutions will cause the bulb to glow with equal intensity.

$NH_{3}$

$NaOH$

$Ba(OH)_{2}$

$KOH$

Acidic fog

Acidic snow

Sulfate pellets falling to the ground

Dilute sulfuric acid in rain

$CaCO_3(s) + H_2SO_4(aq) \rightarrow CaSO_4(aq) + H_2O(l) + CO_2(g)$

$CaO(s) + H_2SO_4(aq) \rightarrow CaSO_4(aq) + H_2O(l)$

$Ca(OH)_2(s) + 2HNO_3(aq) \rightarrow Ca(NO_3)_2(aq) + 2H_2O(l)$

$CaCO_3(s) + 2HCl(aq) \rightarrow CaCl_2(aq) + H_2O(l) + CO_2(g)$

$N_2$

$N_2O$

$NO_2$

$NH_3$

As a Brønsted-Lowry acid

As a Lewis acid

As a reducing agent

As a Lewis base

Ionic bond

Coordinate covalent bond

Hydrogen bond

Metallic bond

$BF_{3}$

$AlCl_{3}$

$NH_{3}$

$H^{+}$

$3.5 \times 10^{-4}$

$5.0 \times 10^{-4}$

$3.16 \times 10^{-3}$

$3.16 \times 10^{-4}$

$50\text{ cm}^3$ of $0.1\text{ M } HCl$ and $50\text{ cm}^3$ of $0.1\text{ M } NaCl$

$50\text{ cm}^3$ of $0.1\text{ M } NaOH$ and $50\text{ cm}^3$ of $0.1\text{ M } CH_3COONa$

$50\text{ cm}^3$ of $0.1\text{ M } CH_3COOH$ and $25\text{ cm}^3$ of $0.1\text{ M } NaOH$

$50\text{ cm}^3$ of $0.1\text{ M } NH_3$ and $50\text{ cm}^3$ of $0.1\text{ M } NH_4Cl$

12.00

12.30

1.70

2.00

The region where the pH changes most rapidly near the equivalence point

The region where the pH remains relatively constant despite the addition of small amounts of base

The region where only the salt and water are present

The region after the equivalence point where excess hydroxide ions determine the pH

Phenolphthalein ($pK_{In} = 9.6$)

Bromothymol blue ($pK_{In} = 7.0$)

Methyl orange ($pK_{In} = 3.7$)

Alizarin yellow ($pK_{In} = 11.0$)

At the initial point before any base is added

At the equivalence point

At the half-equivalence point

At the end-point where the indicator changes color