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Chapter 4: Problem 51

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide

Short Answer

Expert verified
a. \(Ba^{2+} (aq) + SO_4^{2-} (aq) → BaSO_4 (s)\) b. \(Pb^{2+} (aq) + 2 Cl^- (aq) → PbCl_2 (s)\) c. No reaction d. No reaction e. \(Cu^{2+} (aq) + 2 OH^- (aq) → Cu(OH)_2 (s)\)

Step by step solution

01

a. Ammonium sulfate and barium nitrate

Start by writing the reactants and products of the possible double replacement reaction: (Ammonium ion: NH₄⁺, Sulfate ion: SO₄²⁻, Barium ion: Ba²⁺, Nitrate ion: NO₃⁻) NH₄₂SO₄ (aq) + Ba(NO₃)₂ (aq) → 2 NH₄NO₃ (aq) + BaSO₄ (s) Since barium sulfate is insoluble, a reaction occurs. Now, write the net ionic equation by omitting the spectator ions (NH₄⁺ and NO₃⁻): Ba²⁺ (aq) + SO₄²⁻ (aq) → BaSO₄ (s)
02

b. Lead(II) nitrate and sodium chloride

Write the reactants and products of the possible double replacement reaction: (Lead(II) ion: Pb²⁺, Nitrate ion: NO₃⁻, Sodium ion: Na⁺, Chloride ion: Cl⁻) Pb(NO₃)₂ (aq) + 2 NaCl (aq) → 2 NaNO₃ (aq) + PbCl₂ (s) Since lead(II) chloride is insoluble, a reaction occurs. Write the net ionic equation by omitting the spectator ions (NO₃⁻ and Na⁺): Pb²⁺ (aq) + 2 Cl⁻ (aq) → PbCl₂ (s)
03

c. Sodium phosphate and potassium nitrate

Write the reactants and products of the possible double replacement reaction: (Sodium ion: Na⁺, Phosphate ion: PO₄³⁻, Potassium ion: K⁺, Nitrate ion: NO₃⁻) Na₃PO₄ (aq) + 3 KNO₃ (aq) → 3 NaNO₃ (aq) + K₃PO₄ (aq) Since all the compounds are soluble, no reaction occurs, and no net ionic equation needs to be written.
04

d. Sodium bromide and rubidium chloride

Write the reactants and products of the possible double replacement reaction: (Sodium ion: Na⁺, Bromide ion: Br⁻, Rubidium ion: Rb⁺, Chloride ion: Cl⁻) NaBr (aq) + RbCl (aq) → NaCl (aq) + RbBr (aq) Since all the compounds are soluble, no reaction occurs, and no net ionic equation needs to be written.
05

e. Copper(II) chloride and sodium hydroxide

Write the reactants and products of the possible double replacement reaction: (Copper(II) ion: Cu²⁺, Chloride ion: Cl⁻, Sodium ion: Na⁺, Hydroxide ion: OH⁻) CuCl₂ (aq) + 2 NaOH (aq) → 2 NaCl (aq) + Cu(OH)₂ (s) Since copper(II) hydroxide is insoluble, a reaction occurs. Write the net ionic equation by omitting the spectator ions (Na⁺ and Cl⁻): Cu²⁺ (aq) + 2 OH⁻ (aq) → Cu(OH)₂ (s)

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Most popular questions from this chapter

In a 1-L beaker, \(203 \mathrm{~mL}\) of \(0.307 \mathrm{M}\) ammonium chromate was mixed with \(137 \mathrm{~mL}\) of \(0.269 \mathrm{M}\) chromium(III) nitrite to produce ammonium nitrite and chromium(III) chromate. Write the balanced chemical reaction occurring here. If the percent yield of the reaction was \(88.0 \%\), what mass of chromium(III) chromate was isolated?

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of \(204.22 \mathrm{~g} / \mathrm{mol}\). In the titration, \(34.67 \mathrm{~mL}\) of the sodium hydroxide solution was required to react with \(0.1082\) g KHP. Calculate the molarity of the sodium hydroxide.

The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every \(10^{6}\) parts of solution. Mathematically, by mass: $$ \mathrm{ppm}=\frac{\mu \mathrm{g} \text { solute }}{\mathrm{g} \text { solution }}=\frac{\mathrm{mg} \text { solute }}{\mathrm{kg} \text { solution }} $$ In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to \(1.0 \mu \mathrm{g}\) of solute per \(1.0 \mathrm{~mL}\), which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. \(5.0 \mathrm{ppb} \mathrm{Hg}\) in \(\mathrm{H}_{2} \mathrm{O}\) b. \(1.0 \mathrm{ppb} \mathrm{CHCl}_{3}\) in \(\mathrm{H}_{2} \mathrm{O}\) c. \(10.0 \mathrm{ppm}\) As in \(\mathrm{H}_{2} \mathrm{O}\) d. \(0.10\) ppm DDT \(\left(\mathrm{C}_{14} \mathrm{H}_{9} \mathrm{Cl}_{5}\right)\) in \(\mathrm{H}_{2} \mathrm{O}\)

What mass of solid \(\mathrm{AgBr}\) is produced when \(100.0 \mathrm{~mL}\) of \(0.150 \mathrm{M}\) \(\mathrm{AgNO}_{3}\) is added to \(20.0 \mathrm{~mL}\) of \(1.00 M \mathrm{NaBr} ?\)

Assign the oxidation state for nitrogen in each of the following. a. \(\mathrm{Li}_{3} \mathrm{~N} \quad\) f. \(\mathrm{NO}_{2}\) b. \(\mathrm{NH}_{3} \quad\) g. \(\mathrm{NO}_{2}^{-}\) c. \(\mathrm{N}_{2} \mathrm{H}_{4} \quad\) h. \(\mathrm{NO}_{3}\) d. NO i. \(\mathrm{N}_{2}\) e. \(\mathrm{N}_{3} \mathrm{O}\)
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