Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 104

To precipitate \(\mathrm{Zn}^{2+}\) from \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}),\) add (a) \(\mathrm{NH}_{4} \mathrm{Cl} ;\) (b) \(\mathrm{MgBr}_{2} ;\) (c) \(\mathrm{K}_{2} \mathrm{CO}_{3} ;\) (d) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\).

Short Answer

Expert verified
Only option (c) \(\mathrm{K}_{2} \mathrm{CO}_{3}\) will precipitate \(\mathrm{Zn}^{2+}\) from \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})\). The rest of the options will not form a precipitate with it.

Step by step solution

01

Analyze Option (a)

Option (a) involves adding \(\mathrm{NH}_{4} \mathrm{Cl}\) to the solution. Since \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{Cl}^{-}\) are both common ions that form soluble compounds, they will not produce a precipitate with \(\mathrm{Zn}^{2+}\). Therefore, option (a) will not precipitate \(\mathrm{Zn}^{2+}\).
02

Analyze Option (b)

Option (b) involves adding \(\mathrm{MgBr}_{2}\) to the solution. Here, \(\mathrm{Mg}^{2+}\) is a common cation that forms soluble compounds, while \(\mathrm{Br}^{-}\) is a common anion, also forming soluble compounds. Therefore, adding \(\mathrm{MgBr}_{2}\) will not produce a precipitate with \(\mathrm{Zn}^{2+}\). Hence, option (b) will not precipitate \(\mathrm{Zn}^{2+}\).
03

Analyze Option (c)

Option (c) involves adding \(\mathrm{K}_{2} \mathrm{CO}_{3}\) to the solution. Here, \(\mathrm{CO}_{3}^{2-}\) tends to form insoluble compounds according to the solubility rules. Therefore, adding \(\mathrm{K}_{2} \mathrm{CO}_{3}\) will produce a precipitate with \(\mathrm{Zn}^{2+}\). Hence, option (c) will precipitate \(\mathrm{Zn}^{2+}\). It is noteworthy that \(\mathrm{K}^{+}\) forms soluble compounds, but it does not influence the precipitation of \(\mathrm{Zn}^{2+}\).
04

Analyze Option (d)

Option (d) involves adding \((\mathrm{NH}_{4})_{2} \mathrm{SO}_{4}\) to the solution. Both \(\mathrm{NH}_{4}^{+}\) and \(\mathrm{SO}_{4}^{-}\) form soluble compounds and will not produce a precipitate with \(\mathrm{Zn}^{2+}\). Therefore, option (d) will not precipitate \(\mathrm{Zn}^{2+}\).

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

A piece of marble (assume it is pure \(\mathrm{CaCO}_{3}\) ) reacts with \(2.00 \mathrm{L}\) of \(2.52 \mathrm{M} \mathrm{HCl}\). After dissolution of the marble, a \(10.00 \mathrm{mL}\) sample of the resulting solution is withdrawn, added to some water, and titrated with 24.87 mL of 0.9987 M NaOH. What must have been the mass of the piece of marble? Comment on the precision of this method; that is, how many significant figures are justified in the result?

Balance these equations for disproportionation reactions. (a) $\mathrm{Cl}_{2}(\mathrm{g}) \longrightarrow \mathrm{Cl}^{-}+\mathrm{ClO}_{3}^{-}$ (basic solution) (b) $\mathrm{S}_{2} \mathrm{O}_{4}^{2-} \longrightarrow \mathrm{S}_{2} \mathrm{O}_{3}^{2-}+\mathrm{HSO}_{3}^{-}$ (acidic solution)

Predict in each case whether a reaction is likely to occur. If so, write a net ionic equation. (a) $\mathrm{AgNO}_{3}(\mathrm{aq})+\mathrm{CuCl}_{2}(\mathrm{aq}) \longrightarrow$ (b) $\mathrm{Na}_{2} \mathrm{S}(\mathrm{aq})+\mathrm{FeCl}_{2}(\mathrm{aq}) \longrightarrow$ (c) $\mathrm{Na}_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq}) \longrightarrow$

Following are some laboratory methods occasionally used for the preparation of small quantities of chemicals. Write a balanced equation for each. (a) preparation of \(\mathrm{H}_{2} \mathrm{S}(\mathrm{g}): \mathrm{HCl}(\mathrm{aq})\) is heated with \(\mathrm{FeS}(\mathrm{s})\) (b) preparation of \(\mathrm{Cl}_{2}(\mathrm{g}): \mathrm{HCl}(\mathrm{aq})\) is heated with \(\mathrm{MnO}_{2}(\mathrm{s}) ; \mathrm{MnCl}_{2}(\mathrm{aq})\) and \(\mathrm{H}_{2} \mathrm{O}(1)\) are other products (c) preparation of \(\mathrm{N}_{2}: \mathrm{Br}_{2}\) and \(\mathrm{NH}_{3}\) react in aqueous solution; \(\mathrm{NH}_{4} \mathrm{Br}\) is another product (d) preparation of chlorous acid: an aqueous suspension of solid barium chlorite is treated with dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\)

A sample of battery acid is to be analyzed for its sulfuric acid content. A \(1.00 \mathrm{mL}\) sample weighs \(1.239 \mathrm{g}\). This \(1.00 \mathrm{mL}\) sample is diluted to \(250.0 \mathrm{mL}\), and \(10.00 \mathrm{mL}\) of this diluted acid requires \(32.44 \mathrm{mL}\) of \(0.00498 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) for its titration. What is the mass percent of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in the battery acid? (Assume that complete ionization and neutralization of the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) occurs.)
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

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