Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 4: Problem 7

The labels have fallen off three bottles containing powdered samples of metals; one contains zinc, one lead, and the other platinum. You have three solutions at your disposal: \(1 \mathrm{M}\) sodium nitrate, \(1 \mathrm{M}\) nitric acid, and \(1 \mathrm{M}\) nickel nitrate. How could you use these solutions to determine the identities of each metal powder? [Section 4.4]

Short Answer

Expert verified
To identify the metal powders, perform reactions with the given solutions and observe their behavior: 1. React samples with 1M sodium nitrate: - Zinc forms zinc nitrate and sodium. - Lead and Platinum do not react. 2. React samples with 1M nitric acid: - Zinc and Lead form zinc nitrate and lead nitrate with hydrogen gas, respectively. - Platinum does not react. 3. React samples with 1M nickel nitrate: - Zinc forms zinc nitrate and nickel. - Lead and Platinum do not react. Finally, identify the metal powders based on reactivity: - Zinc reacts with all three solutions. - Lead reacts only with nitric acid. - Platinum does not react with any solution.

Step by step solution

01

Understanding the Reactivity Series

The Reactivity Series of metals is a list of elements organized by their reactivity, with the most reactive metals at the top and least reactive at the bottom. The order of reactivity for the given metals in this exercise is: Zinc > Lead > Platinum. Platinum being the least reactive metal will not react with any of the given solutions while zinc being the most reactive will react with most of them.
02

Reacting with Sodium Nitrate

Add a portion of each metal powder to three separate test tubes. Then add 1M sodium nitrate solution to each test tube. Observe the reactions: - Zinc will react with sodium nitrate to form zinc nitrate and sodium. - Lead will not react with sodium nitrate since its reactivity is lower. - Platinum will not react with sodium nitrate as it's the least reactive.
03

Reacting with Nitric Acid

Add a portion of each metal powder to three new test tubes. Then add 1M nitric acid solution to each test tube. Observe the reactions: - Zinc will react with nitric acid to form zinc nitrate and hydrogen gas. - Lead will react with nitric acid to form lead nitrate and hydrogen gas. - Platinum will not react with nitric acid due to its low reactivity.
04

Reacting with Nickel Nitrate

Add a portion of each metal powder to three new test tubes. Then add 1M nickel nitrate solution to each test tube. Observe the reactions: - Zinc will react with nickel nitrate to form zinc nitrate and nickel. - Lead will not react with nickel nitrate since its reactivity is lower. - Platinum will not react with nickel nitrate as it's the least reactive.
05

Identifying the Metal Powders

Based on the observations from the reactions with the three solutions, we can determine the identities of the metal powders: - Zinc will react with all three solutions (sodium nitrate, nitric acid, and nickel nitrate). - Lead will only react with nitric acid. - Platinum will not react with any of the solutions. Thus, by observing which metal powder reacts with which solutions, we can identify the contents of the three bottles.

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

You know that an unlabeled bottle contains an aqueous solution of one of the following: \(\mathrm{AgNO}_{3}, \mathrm{CaCl}_{2},\) or \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} . \mathrm{A}\) friend suggests that you test a portion of the solution with \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) and then with NaCl solutions. According to your friend's logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle? (a) Barium sulfate could precipitate. (b) Silver chloride could precipitate. (c) Silver sulfate could precipitate. (d) More than one, but not all, of the reactions described in answers a-c could occur. (e) All three reactions described in answers a-c could occur.

(a) Is the number of moles of ions present in a solution an intensive or an extensive property? (b) Can you identify which one between $0.10 \mathrm{~mol} \mathrm{ZnCl}_{2}\( and \)0.1 \mathrm{M} \mathrm{ZnCl}_{2}$ contains more \(\mathrm{Zn}^{2+}\) ion? Why?

(a) How many milliliters of \(0.120 \mathrm{M} \mathrm{HCl}\) are needed to completely neutralize \(50.0 \mathrm{~mL}\) of $0.101 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}$ solution? (b) How many milliliters of \(0.125 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) are needed to neutralize \(0.200 \mathrm{~g}\) of \(\mathrm{NaOH}\) ? (c) If $55.8 \mathrm{~mL}\( of a \)\mathrm{BaCl}_{2}$ solution is needed to precipitate all the sulfate ion in a \(752-\mathrm{mg}\) sample of $\mathrm{Na}_{2} \mathrm{SO}_{4}\(, what is the molarity of the \)\mathrm{BaCl}_{2}$ solution? (d) If \(42.7 \mathrm{~mL}\) of \(0.208 \mathrm{MHCl}\) solution is needed to neutralize a solution of \(\mathrm{Ca}(\mathrm{OH})_{2}\), how many grams of \(\mathrm{Ca}(\mathrm{OH})_{2}\) must be in the solution?

Classify each of the following substances as a nonelectrolyte, weak electrolyte, or strong electrolyte in water: (a) HF, (b) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\) (benzoicacid), (c) \(\mathrm{C}_{6} \mathrm{H}_{6}\) (benzene), (d) \(\mathrm{CoCl}_{3}\) (e) \(\mathrm{AgNO}_{3}\)

The distinctive odor of vinegar is due to aceticacid, $\mathrm{CH}_{3} \mathrm{COOH}$, which reacts with sodium hydroxide according to: \(\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NaOH}(a q) \longrightarrow\) $$ \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{NaCH}_{3} \mathrm{COO}(a q) $$ If \(3.45 \mathrm{~mL}\) of vinegar needs \(42.5 \mathrm{~mL}\) of $0.115 \mathrm{M} \mathrm{NaOH}$ to reach the equivalence point in a titration, how many grams of acetic acid are in a \(1.00-\) qt sample of this vinegar?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Ionic and Molecular Compounds

Read Explanation

The Earths Atmosphere

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