Problem 1
What is an electrolyte? How can you differentiate experimentally between a weak electrolyte and a strong electrolyte? Give an example of each.
Problem 2
Name two acids that are strong electrolytes and one acid that is a weak electrolyte. Name two bases that are strong electrolytes and one base that is a weak electrolyte.
Problem 3
Which compound or compounds in each of the following groups is (are) expected to be soluble in water? (a) \(\mathrm{CuO}, \mathrm{CuCl}_{2}, \mathrm{FeCO}_{3}\) (b) \(\mathrm{AgI}, \mathrm{Ag}_{3} \mathrm{PO}_{4}, \mathrm{AgNO}_{3}\) (c) \(\mathrm{K}_{2} \mathrm{CO}_{3}, \mathrm{KI}, \mathrm{KMnO}_{4}\)
Problem 4
Which compound or compounds in each of the following groups is (are) expected to be soluble in water? (a) \(\mathrm{BaSO}_{4}, \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{BaCO}_{3}\) (b) \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{NaClO}_{4}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}\) (c) \(\mathrm{AgBr}, \mathrm{KBr}, \mathrm{Al}_{2} \mathrm{Br}_{6}\)
Problem 5
The following compounds are water-soluble. What ions are produced by each compound in aqueous solution? (a) KOH (c) \(\mathrm{LiNO}_{3}\) (b) \(\mathrm{K}_{2} \mathrm{SO}_{4}\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\)
Problem 6
The following compounds are water-soluble. What ions are produced by each compound in aqueous solution? (a) \(\mathrm{KI}\) (c) \(\mathrm{K}_{2} \mathrm{HPO}_{4}\) (b) \(\mathrm{Mg}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}\) (d) NaCN
Problem 7
Decide whether each of the following is water-soluble. If soluble, tell what ions are produced. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (c) NiS (b) \(\mathrm{CuSO}_{4}\) (d) \(\mathrm{BaBr}_{2}\)
Problem 8
Decide whether each of the following is water-soluble. If soluble, tell what ions are produced. (a) \(\mathrm{NiCl}_{2}\) (c) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) (b) \(\mathrm{Cr}\left(\mathrm{NO}_{3}\right)_{3}\) (d) \(\mathrm{BaSO}_{4}\)
Problem 9
Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species \((s, \ell, \text { aq, or } g\) ). $$\mathrm{CdCl}_{2}+\mathrm{NaOH} \longrightarrow \mathrm{Cd}(\mathrm{OH})_{2}+\mathrm{NaCl}$$
Problem 10
Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species (s, \(\ell\), aq, or g). $$\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{CO}_{3} \longrightarrow \mathrm{NiCO}_{3}+\mathrm{NaNO}_{3}$$
