91Ó°ÊÓ

Decide whether each of the following is watersoluble. If soluble, tell what ions are produced when the compound dissolves in water. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (b) \(\mathrm{CuSO}_{4}\) (c) NiS (d) \(\mathrm{BaBr}_{2}\)

Decide whether each of the following is watersoluble. If soluble, tell what ions are produced when the compound dissolves in water. (a) \(\mathrm{NiCl}_{2}\) (b) \(\operatorname{Cr}\left(\mathrm{NO}_{3}\right)_{3}\) (c) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) (d) \(\mathrm{BaSO}_{4}\)

Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species \((\mathrm{s}, \ell, \mathrm{aq}\) or g). $$\mathrm{CdCl}_{2}+\mathrm{NaOH} \rightarrow \mathrm{Cd}(\mathrm{OH})_{2}+\mathrm{NaCl}$$

Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species \((\mathrm{s}, \ell, \mathrm{aq}\) or g). $$\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NiCO}_{3}+\mathrm{NaNO}_{3}$$

Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation. (a) \(\mathrm{NiCl}_{2}(\mathrm{aq})+\left(\mathrm{NH}_{4}\right)_{2} \mathrm{S}(\mathrm{aq}) \rightarrow\) (b) \(\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{Na}_{3} \mathrm{PO}_{4}(\mathrm{aq}) \rightarrow\)

Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation. (a) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{KBr}(\mathrm{aq}) \rightarrow\) (b) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{KF}(\mathrm{aq}) \rightarrow\) (c) \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(\mathrm{aq}) \rightarrow\)

Write a balanced equation for the ionization of nitric acid in water.

Write a balanced equation for the ionization of perchloric acid in water.

Phosphoric acid can supply one, two, or three \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions in aqueous solution. Write balanced equations (like those for sulfuric acid on page 142 ) to show this successive loss of hydrogen ions.

Write a balanced equation for reaction of the basic oxide, magnesium oxide, with water.