/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 72 One of the classic methods for t... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 21: Problem 72

One of the classic methods for the determination of the manganese content in steel involves converting all the manganese to the deeply colored permanganate ion and then measuring the absorption of light. The steel is first dissolved in nitric acid, producing the manganese(II) ion and nitrogen dioxide gas. This solution is then reacted with an acidic solution containing periodate ion; the products are the permanganate and iodate ions. Write balanced chemical equations for both of these steps.

Short Answer

Expert verified
The balanced chemical equations for determining the manganese content in steel are: 1. \(Mn(s) + 2 \ HNO_{3}(aq) \rightarrow Mn^{2+}(aq) + 2 \ NO_{2}(g) + 2 \ H^{+}(aq) \) 2. \(5 \ Mn^{2+}(aq) + 12 \ IO_{4}^{-}(aq) + 16 \ H^{+}(aq) \rightarrow 5 \ MnO_{4}^{-}(aq) + 12 \ IO_{3}^{-}(aq) + 8 \ H_{2}O(l) \)

Step by step solution

01

Identify the chemical formulas

First, let us determine the chemical formulas for all the species involved in both reactions: 1. Steel: Primarily composed of Iron (Fe) and Manganese (Mn). 2. Nitric acid: HNO3 3. Manganese(II) ion: Mn^(2+) 4. Nitrogen dioxide gas: NO2 5. Periodate ion: IO4^(-) 6. Acidic solution: H+ ions are present, usually from a strong acid like H2SO4 or HCl. 7. Permanganate ion: MnO4^(-) 8. Iodate ion: IO3^(-) Now that we have the chemical formulas, we can write the unbalanced equations.
02

Write the unbalanced chemical equations

For the first reaction, Manganese in steel + Nitric acid -> Manganese(II) ion + Nitrogen dioxide gas Mn(s) + HNO3(aq) -> Mn^(2+)(aq) + NO2(g) For the second reaction, Manganese(II) ion + Periodate ion + Acidic solution -> Permanganate ion + Iodate ion Mn^(2+)(aq) + IO4^(-)(aq) + H+(aq) -> MnO4^(-)(aq) + IO3^(-)(aq)
03

Balance the chemical equations

Balance the first chemical equation: \(Mn(s) + 2 \ HNO_{3}(aq) \rightarrow Mn^{2+}(aq) + 2 \ NO_{2}(g) + 2 \ H^{+}(aq) \) Balance the second chemical equation: \(5 \ Mn^{2+}(aq) + 12 \ IO_{4}^{-}(aq) + 16 \ H^{+}(aq) \rightarrow 5 \ MnO_{4}^{-}(aq) + 12 \ IO_{3}^{-}(aq) + 8 \ H_{2}O(l) \) Now we have the balanced chemical equations for determining the manganese content of steel: 1. \(Mn(s) + 2 \ HNO_{3}(aq) \rightarrow Mn^{2+}(aq) + 2 \ NO_{2}(g) + 2 \ H^{+}(aq) \) 2. \(5 \ Mn^{2+}(aq) + 12 \ IO_{4}^{-}(aq) + 16 \ H^{+}(aq) \rightarrow 5 \ MnO_{4}^{-}(aq) + 12 \ IO_{3}^{-}(aq) + 8 \ H_{2}O(l) \)

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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 of the following crystal field diagram(s) is(are) correct for the complex given? a. \(\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\) (tetrahedral) b. \(\operatorname{Mn}(\mathrm{CN})_{6}^{3-}\) (strong field) c. \(\mathrm{Ni}(\mathrm{CN})_{4}^{2-}\) (square planar, diamagnetic)

A certain first-row transition metal ion forms many different colored solutions. When four coordination compounds of this metal, each having the same coordination number, are dissolved in water, the colors of the solutions are red, yellow, green, and blue. Further experiments reveal that two of the complex ions are paramagnetic with four unpaired electrons and the other two are diamagnetic. What can be deduced from this information about the four coordination compounds?

What causes high-altitude sickness, and what is high-altitude acclimatization?

\(\mathrm{CoCl}_{4}^{2-}\) forms a tetrahedral complex ion and \(\mathrm{Co}(\mathrm{CN})_{6}^{3-}\) forms an octahedral complex ion. What is wrong about the following statements concerning each complex ion and the \(d\) orbital splitting diagrams? a. \(\mathrm{CoCl}_{4}^{2-}\) is an example of a strong-field case having two unpaired electrons. b. Because \(\mathrm{CN}^{-}\) is a weak-field ligand, \(\mathrm{Co}(\mathrm{CN})_{6}^{3-}\) will be a low-spin case having four unpaired electrons.

Figure 21.17 shows that the cis isomer of \(\mathrm{Co}(\mathrm{en})_{2} \mathrm{Cl}_{2}^{+}\) is optically active while the trans isomer is not optically active. Is the same true for \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}+?\) Explain.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

Read Explanation

Chemical Analysis

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.