Chapter 8

Indicate whether a precipitate forms when these solutions are mixed, and write the formula of the precipitate if one forms: (a) Silver nitrate and potassium iodide (b) Lithium sulfate and silver acetate (c) Sodium chloride and ammonium sulfate

What does it mean when the label (aq) is attached to the formula for an ionic compound?

The \(\quad\) ionic equation for a reaction is obtained by canceling the spectator ions in the ionic equation.

Write the balanced equation, the complete ionic equation, and the net ionic equation for the reaction between aqueous potassium chloride and lead(II) nitrate that produces lead chloride and potassium nitrate.

Acids produce ions when dissolved in water, and bases produce ions when dissolved in water.

The reaction between an acid and a base is called an acid-base reaction.

Write the balanced equation for the reaction that occurs when an aqueous solution of carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}\), is mixed with an aqueous solution of lithium hydroxide, \(\mathrm{LiOH}\).

Of the types of reactions discussed in the chapter, list three ways the reaction \(\mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{CaSO}_{4}+2 \mathrm{H}_{2} \mathrm{O}\) can be classified.

(a) True or false? It is possible for a reaction to be simultaneously a single-replacement reaction and a combination reaction. (b) True or false? It is possible for a reaction to be simultaneously a double-replacement reaction and a neutralization reaction. If either statement is false, explain why.

Would you expect a reaction in which all reactants are in the gas phase to go faster, slower, or remain at the same rate if the size of the container is increased while everything else is held constant? Explain.

Nitrous oxide, \(\mathrm{N}_{2} \mathrm{O}\), is produced when ammonium nitrate, \(\mathrm{NH}_{4} \mathrm{NO}_{3}\), is heated gently. Water is also produced in the reaction. Write the balanced equation for the reaction.

Write the complete ionic equation and the net ionic equation for the reaction that occurs between aqueous solutions of: (a) Silver nitrate and potassium iodide (b) Lithium sulfate and silver acetate

Write a balanced chemical equation for each reaction: (a) Calcium metal reacts with solid phosphorus, \(\mathrm{P}_{4}\), to form calcium phosphide. (b) Sodium metal reacts with water to produce aqueous sodium hydroxide and hydrogen gas. (c) Ammonium nitrate powder explodes to form nitrogen gas, oxygen gas, and water vapor.

Ammonia gas reacts with fluorine gas to form ammonium fluoride and nitrogen gas. (a) Write a balanced chemical equation for this reaction. (b) Draw a picture representing the molecular view of the reactant mixture. (c) Draw a picture representing the molecular view of the product mixture.

Write the complete ionic equation and net ionic equation for the neutralization reaction between aqueous hydrobromic acid and barium hydroxide.

In the chapter, we saw the combustion reaction for methane. This was actually a complete combustion reaction because carbon ended up as carbon dioxide. If the same reaction is carried out where the oxygen supply is limited, incomplete combustion takes place, yielding toxic carbon monoxide, CO, instead of \(\mathrm{CO}_{2}\). Write the balanced reaction for the incomplete combustion of methane. Make sure it is balanced.

\( \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\) (lead (II) nitrate), upon sufficient heating, turns into \(\mathrm{PbO}\) (lead (II) oxide), oxygen gas, and nitrogen dioxide gas. Write a balanced equation for this reaction, and classify the reaction type.

Simple soaps, like sodium laurate, \(\mathrm{NaC}_{12} \mathrm{H}_{22} \mathrm{O}_{2}\) are ionic compounds with small cations and large covalent anions. These soaps are somewhat soluble in water but form a soap scum if the water is "hard," which means it contains calcium ions \(\mathrm{Ca}^{2+}\) or magnesium ions, \(\mathrm{Mg}^{2+}\). Write a net ionic equation for the formation of soap scum. Also classify the reaction type or types.

Ammonia, \(\mathrm{NH}_{3}\), is a gas, but it is very soluble in water, so when you bubble ammonia gas into water you produce an aqueous solution of ammonia. Interestingly, this solution is basic (hydroxide ions are formed). Postulate a reaction that occurs between ammonia and water to make the solution basic, and classify the reaction type.

When you strike a match, trace amounts of white phosphorus \(\left(\mathrm{P}_{4}\right)\) are converted into an oxide of phosphorus, \(\mathrm{P}_{4} \mathrm{O}_{10}\). This conversion releases sufficient heat to ignite the match head. Write a balanced reaction for this conversion, and classify the reaction type(s).

Starting from 1,3 -butadiene, how would you prepare 2,3-dibromobutane?