Chapter 5

What is an aqueous solution? What is the difference between the solute and the solvent?

Explain how a strong electrolyte, a weak electrolyte, and a noneloctolute differ.

Lxplain the dilterence betwecn a strong acid and a weak acid.

What does it mean for a compound to be soluble? Insoluble?

What is a precipitation reaction? Give an example.

How can you predict whether a precipitation reaction will occur upon mixing two aqueous solutions?

Explain how a molecular equation, a complete ionic equation, and a net ionic equation differ.

What is the Arrhenius definition of an acid? A base?

What is an acid-base reaction? Give an example.

Explain the principles behind an acid-base titration. What is an indicator?

What is a gas-evolution reaction? Give an example.

What is an oxidation-reduction reaction? Give an example.

How can oxidation states be used to identify redox reactions?

Calculate the molarity of each solution. a. 3.25 mol of LiCl in 2.78 L solution b. \(28.33 \mathrm{gC}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) in \(1.28 \mathrm{~L}\) of solution c. \(32.4 \mathrm{mg} \mathrm{NaCl}\) in \(122.4 \mathrm{~mL}\) of solution

What is the molarity of \(\mathrm{Cl}^{-}\) in each solution? a. \(0.200 \mathrm{M} \mathrm{NaCl}\) b. \(0.150 \mathrm{M} \mathrm{SrCl}_{2}\) c. \(0.100 \mathrm{M} \mathrm{AlCl}_{3}\)

How many moles of \(\mathrm{KCl}\) are contained in each solution? b. 1.8 L of a 0.85 M KCl solution c. \(114 \mathrm{~mL}\) of a \(1.85 \mathrm{M}\) KCl solution

What volume of \(0.200 \mathrm{M}\) ethanol solution contains eacl amount in moles of ethanol? a. 0.45 mol ethanol b. 1.22 mol ethanol c. \(1.2 \times 10^{-2}\) mol ethanol

A laboratory procedure calls for making \(400.0 \mathrm{~mL}\) of a \(1.1 \mathrm{M}\) NaNO \(_{3}\) solution. What mass of \(\mathrm{NaNO}_{3}\) (in g) is needed?

If \(123 \mathrm{~mL}\) of a \(1.1 \mathrm{M}\) glucose solution is diluted to \(500.0 \mathrm{~mL}\), what is the molarity of the diluted solution?

If \(3.5 \mathrm{~L}\) of a \(4.8 \mathrm{M} \mathrm{SrCl}_{2}\) solution is diluted to \(45 \mathrm{~L},\) what is the molarity of the diluted solution?

To what volume should you dilute \(50.0 \mathrm{~mL}\) of a \(12 \mathrm{M}\) stock HNO solution to obtain a \(0.100 \mathrm{M}\) HNO \(_{3}\) solution?

To what volume should you dilute \(25 \mathrm{~mL}\) of a \(10.0 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution to obtain a \(0.150 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution?

Consider the reaction: $$ \mathrm{Li}_{2} \mathrm{~S}(a q)+\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow 2 \mathrm{LiNO}_{3}(a q)+\operatorname{coS}(s) $$ What volume of \(0.150 \mathrm{M} \mathrm{Li}_{2} \mathrm{~S}\) solution is required to completely react with \(125 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2} ?\)

What is the molarity of \(\mathrm{ZnCl}_{2}\) that forms when \(25.0 \mathrm{~g}\) of zinc completely reacts with \(\mathrm{CuCl}_{2}\) according to the following reaction? Assume a final volume of \(275 \mathrm{~mL}\). $$ \mathrm{Zn}(s)+\mathrm{CuCl}_{2}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{Cu}(s) $$

For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. \(\mathrm{CsCl}\) b. \(\mathrm{CH}_{3} \mathrm{OH}\) c. \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\) d. \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\)

Classify each compound as a strong electrolyte or nonelectrolyte. a. \(\mathrm{MgBr}_{2}\) b. \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) c. \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) d. \(\mathrm{KOH}\)

Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. \(\mathrm{AgNO}_{3}\) b. \(\mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) c. \(\mathrm{KNO}_{3}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{~S}\)

Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgI b. \(\mathrm{Cu}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) c. \(\mathrm{CoCO}_{3}\) d. \(\mathrm{K}_{3} \mathrm{PO}_{4}\)

Complete and balance each equation. If no reaction occurs, write "NO REACTION." a. \(\operatorname{Lil}(a q)+\) BaS \((a q) \longrightarrow\) b. \(\operatorname{KCl}(a q)+\operatorname{CaS}(a q) \longrightarrow\) c. \(\operatorname{CrBr}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \longrightarrow\) d. \(\mathrm{NaOH}(a q)+\mathrm{FeCl}_{3}(a q) \longrightarrow\)

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write "NO REACTION." a. potassium carbonate and lead(II) nitrate b. lithium sulfate and lead(II) acetate c. copper(II) nitrate and magnesium sulfide d. strontium nitrate and potassium iodide

Write a molecular equation for the precipitation reaction that pccurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write "NO REACTION." a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate

Write balanced complete ionic and net ionic equations for each reaction? a. HCl(aq) \(+\operatorname{LiCl}(a q)\) b. \(\mathrm{CaS}(a q)+\mathrm{CuCl}_{2}(a q) \longrightarrow \mathrm{CuS}(s)+\mathrm{CaCl}_{2}(a q)\) c. \(\mathrm{NaOH}(a q)+\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) d. \(\mathrm{Na}_{3} \mathrm{PO}_{4}(a q)+\mathrm{NiCl}_{2}(a q) \longrightarrow \mathrm{Ni}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\mathrm{NaCl}(a q)\)

Write balanced complete ionic and net ionic equations for each reaction. $$ \begin{array}{l} \text { a. } \mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{CaI}_{2}(a q) \longrightarrow \mathrm{CaSO}_{4}(s)+\mathrm{KI}(a q) \\ \text { b. } \mathrm{NH}_{4} \mathrm{Cl}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NH}_{3}(g)+\mathrm{NaCl}(a q) \\ \text { c. } \mathrm{AgNO}_{3}(a q)+\mathrm{NaCl}(a q) \longrightarrow \mathrm{AgCl}(s)+\mathrm{NaNO}_{3}(a q) \\ \text { d. } \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{K}_{2} \mathrm{CO}_{3}(a q) \stackrel{ }{\mathrm{H}_{2} \mathrm{O}(l)}+\mathrm{CO}_{2}(g)+\mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q) \end{array} $$

Mercury(I) ions \(\left(\mathrm{Hg}_{2}^{2+}\right)\) can be removed from solution by precipitation with \(\mathrm{Cl}^{-}\). Suppose that a solution contains aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2} .\) Write complete ionic and net ionic equations for the reaction of aqueous \(\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}\) with aqueous sodium chloride to form solid \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) and aqueous sodium nitrate.

Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations for the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.

Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.

Complete and balance each acid-base equation. a. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\) b. \(\mathrm{HClO}_{4}(a q)+\mathrm{KOH}(a q) \longrightarrow\) c. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{NaOH}(a q) \longrightarrow\)

Complete and balance each acid-base equation. a. \(\mathrm{HI}(a q)+\mathrm{LiOH}(a q) \longrightarrow\) b. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\) c. \(\mathrm{HCl}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \longrightarrow\)

Write balanced complete ionic and net ionic equations for each acid-base reaction. a. \(\mathrm{HBr}(a q)+\mathrm{NaOH}(a q)\) b. \(\mathrm{HF}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{RbOH}(a q) \longrightarrow\)

Write balanced complete ionic and net ionic equations for each acid-base reaction. a. \(\mathrm{HI}(a q)+\mathrm{RbOH}(a q) \longrightarrow\) b. \(\mathrm{HCHO}_{2}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) \(\mathbf{c .} \mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{LiOH}(a q) \longrightarrow\)

A 25.00-mL sample of an unknown HClO solution requires titration with \(22.62 \mathrm{~mL}\) of \(0.2000 \mathrm{M} \mathrm{NaOH}\) to reach the equivalence point. What is the concentration of the unknown \(\mathrm{HClO}_{4}\) solution? The neutralization reaction is \begin{equation} \mathrm{HClO}_{4}(a q)+\mathrm{NaOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaClO}_{4}(a q) \end{equation}

A 30.00 -mL sample of an unknown \(\mathrm{H}_{3} \mathrm{PO}_{4}\) solution is titrated with a 0.100 M \(\mathrm{NaOH}\) solution. The equivalence point is reached when \(26.38 \mathrm{~mL}\) of \(\mathrm{NaOH}\) solution is added. What is the concentration of the unknown \(\mathrm{H}_{3} \mathrm{PO}_{4}\) solution? The neutralization reaction is $$ \mathrm{H}_{3} \mathrm{PO}_{4}(a q)+3 \mathrm{NaOH}(a q) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(I)+\mathrm{Na}_{3} \mathrm{PO}_{4}(a q) $$

Complete and balance each gas-evolution equation. a. \(\mathrm{HBr}(a q)+\mathrm{NiS}(s) \longrightarrow\) b. \(\mathrm{NH}_{4} \mathrm{I}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) c. \(\operatorname{HBr}(a q)+\mathrm{Na}_{2} \mathrm{~S}(a q) \longrightarrow\) d. \(\mathrm{HClO}_{4}(a q)+\mathrm{Li}_{2} \mathrm{CO}_{3}(a q) \longrightarrow\)

Complete and balance each gas-evolution equation. a. \(\mathrm{HNO}_{3}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{3}(a q) \longrightarrow\) b. \(\mathrm{HCl}(a q)+\mathrm{KHCO}_{3}(a q) \longrightarrow\) c. \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)+\mathrm{NaHSO}_{3}(a q) \longrightarrow\) \(\mathbf{d .}\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ca}(\mathrm{OH})_{2}(a q) \longrightarrow\)

Assign oxidation states to each atom in each element, ion, or compound. a. \(\mathrm{Cl}_{2}\) b. \(\mathrm{Fe}^{3+}\) c. \(\mathrm{CuCl}_{2}\) d. \(\mathrm{CH}_{4}\) e. \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}\) f. \(\mathrm{HSO}_{4}^{-}\)

What is the oxidation state of \(\mathrm{Cr}\) in each compound? a. \(\mathrm{CrO}\) b. \(\mathrm{CrO}_{3}\) c. \(\mathrm{Cr}_{2} \mathrm{O}_{3}\)

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. \(4 \mathrm{Li}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~L}_{2} \mathrm{O}(s)\) b. \(\mathrm{Mg}(s)+\mathrm{Fe}^{2+}(a q) \longrightarrow \mathrm{Mg}^{2+}(a q)+\mathrm{Fe}(s)\) c. \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+2 \mathrm{NaNO}_{3}(a q)\) d. \(\operatorname{HBr}(a q)+\mathrm{KOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{KBr}(a q)\)

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. \(\mathrm{Al}(s)+3 \mathrm{Ag}^{+}(a q) \longrightarrow \mathrm{Al}^{3+}(a q)+3 \mathrm{Ag}(s)\) b. \(\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(I) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)\) c. \(\mathrm{Ba}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{BaCl}_{2}(s)\) d. \(\mathrm{Mg}(s)+\mathrm{Br}_{2}(l) \longrightarrow \mathrm{MgBr}_{2}(s)\)

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write "NO REACTION." a. \(\mathrm{HCl}(a q)+\mathrm{Hg}_{2}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow\) b. \(\mathrm{KHSO}_{3}(a q)+\mathrm{HNO}_{3}(a q) \longrightarrow\) c. aqueous ammonium chloride and aqueous lead(II) nitrate d. aqueous ammonium chloride and aqueous calcium hydroxide