General Chemistry/Properties and Theories of Acids and Bases/Answers

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a) hydrobromic acid
b) sulfuric acid
c) potassium hydroxide, base
d) sulfurous acid
e) phosphoric acid
f) bromous acid
g) sodium chloride, neutral salt

2. Substance: conjugate acid; conjugate base

a) water (H2O): hydronium (H3O+); hydroxide (OH-)
b) ammonia (NH3): ammonium (NH4+); amide (NH2-)
c) bisulfate ion (HSO4-): sulfuric acid (H2SO4); sulfate ion (SO42-)
d) zinc hydroxide (Zn(OH)2): Zn(OH)+; no conjugate base
e) hydrobromic acid (HBr): no conjugate acid; Br-
f) nitrite ion (NO2-): nitrous acid (HNO2); no conjugate base
g) dihydrogen phosphate ion (H2PO4-): phosphoric acid (H3PO4); biphosphate ion (HPO42-)


a) A, E
b) B, C
c) A, B, C, E
d) D
e) No. Both acids and bases will conduct electricity.

4. Conjugate acids are underlined. Conjugate bases are in bold font.

a) HCl + H2O → H3O + Cl-
b) HClO + H2O → ClO- + H3O
c) CH3CH2NH2 + H2O → CH3CH2NH3+ + OH-


a) strontium hydroxide: both
b) butyllithium (C4H9Li): Brønsted-Lowry (reacts with protons to form C4H10 + Li)
c) ammonia: Brønsted-Lowry
d) potassium hydroxide: both
e) potassium iodide: neither

6. No, pure water can still have a very minute amount of dissolved ions.

H2O + H2O → H3O+ + OH-