Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 108

Describe the synthesis of each of the following ionic compounds, starting from solutions of sodium and nitrate salts. Then write the net ionic equation for each synthesis. (a) \(\mathrm{Zn}_{3}\left(\mathrm{PO}_{4}\right)_{2};\) (b) \(\mathrm{Cu}(\mathrm{OH})_{2};\) (c) \(\mathrm{NiCO}_{3}.\)

Short Answer

Expert verified
The balanced equations for the syntheses are \(3Zn(NO3)2 + 2Na3PO4 → Zn3(PO4)2 + 6NaNO3\), \(Cu(NO3)2 + 2NaOH → Cu(OH)2 + 2NaNO3\), and \(Ni(NO3)2 + Na2CO3 → NiCO3 + 2NaNO3\). The net ionic equations are \(3Zn^{2+} + 2PO4^{3-} → Zn3(PO4)2\), \(Cu^{2+} + 2OH- → Cu(OH)2\), and \(Ni^{2+} + CO3^{2-} → NiCO3\).

Step by step solution

01

Synthesize Zn3(PO4)2

To form zinc phosphate (\(\mathrm{Zn}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)), you need a nitrate salt of zinc (\(Zn(NO3)2\)) and a sodium phosphate salt (\(Na3PO4\)). Mixing these two, you would use the technique of double displacement, leaving sodium nitrate (\(NaNO3\)), in the solution forming a precipitate of zinc phosphate. The balanced chemical equation for this reaction is: \[3Zn(NO3)2 + 2Na3PO4 → Zn3(PO4)2 + 6NaNO3\]
02

Write the net ionic equation for Zn3(PO4)2

The net ionic equation cancels out the spectator ions. Sodium and nitrate ions are the spectator ions, so the net ionic equation becomes: \[3Zn^{2+} + 2PO4^{3-} → Zn3(PO4)2\]
03

Synthesize Cu(OH)2

To form copper(II) hydroxide (\(Cu(OH)2\)), you need a nitrate salt of copper (\(Cu(NO3)2\)) and sodium hydroxide (\(NaOH\)). Mixing these two, the sodium and nitrate ions are left in the solution. The balanced chemical equation for this reaction is: \[Cu(NO3)2 + 2NaOH → Cu(OH)2 + 2NaNO3\]
04

Write the net ionic equation for Cu(OH)2

Removing the sodium and nitrate ions (spectator ions) from the equation, the net ionic equation is: \[Cu^{2+} + 2OH- → Cu(OH)2\]
05

Synthesize NiCO3

To form nickel(II) carbonate, you need a nitrate salt of nickel (\(Ni(NO3)2\)) and sodium carbonate (\(Na2CO3\)). Mixing these two, sodium and nitrate ions will be left in the solution. The balanced chemical equation for this reaction is: \[Ni(NO3)2 + Na2CO3 → NiCO3 + 2NaNO3\]
06

Write the net ionic equation for NiCO3

Eliminating the sodium and nitrate ions (spectator ions) from the equation, the net ionic equation is: \[Ni^{2+} + CO3^{2-} → NiCO3\]

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which aqueous solution has the greatest \(\left[\mathrm{H}^{+}\right]:\) (a) \(0.011 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH} ;\) (b) \(0.010 \mathrm{M} \mathrm{HCl} ;\) (c) \(0.010 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4} ;\) (d) \(1.00 \mathrm{M} \mathrm{NH}_{3} ?\) Explain your choice.

Which of the following reactions are oxidationreduction reactions? (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})\) (b) \(2 \mathrm{Li}(\mathrm{s})+2 \mathrm{H}_{2} \mathrm{O}(1) \longrightarrow 2 \mathrm{LiOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})\) (c) \(4 \mathrm{Ag}(\mathrm{s})+\mathrm{PtCl}_{4}(\mathrm{aq}) \longrightarrow 4 \mathrm{AgCl}(\mathrm{s})+\mathrm{Pt}(\mathrm{s})\) (d) \(2 \mathrm{HClO}_{4}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq}) \longrightarrow\) \(2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Ca}\left(\mathrm{ClO}_{4}\right)_{2}(\mathrm{aq})\)

When treated with dilute \(\mathrm{HCl}(\mathrm{aq}),\) the solid that reacts to produce a gas is (a) \(\mathrm{BaSO}_{3} ;\) (b) \(\mathrm{ZnO};\) (c) \(\mathrm{NaBr} ;\) (d) \(\mathrm{Na}_{2} \mathrm{SO}_{4}\).

When concentrated \(\mathrm{CaCl}_{2}(\mathrm{aq})\) is added to \(\mathrm{Na}_{2} \mathrm{HPO}_{4}(\mathrm{aq}),\) a white precipitate forms that is \(38.7 \%\) Ca by mass. Write a net ionic equation representing the probable reaction that occurs.

A \(7.55 \mathrm{g}\) sample of \(\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{s})\) is added to \(125 \mathrm{mL}\) of a vinegar that is \(0.762 \mathrm{M} \mathrm{CH}_{3} \mathrm{COOH} .\) Will the resulting solution still be acidic? Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free