/*! 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 69 The major use of \(\mathrm{Ca}_{... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 21: Problem 69

The major use of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) is in the tempering of metals phosphorus for fireworks acid neutralization the production of phosphoric acid the vulcanization of rubber

Short Answer

Expert verified
The major use of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) is in the production of phosphoric acid.

Step by step solution

01

Identify the Compound

Calcium phosphate, represented by the chemical formula \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\), is the compound in question. We need to identify its major industrial use.
02

List Possible Uses

Although \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) could have various applications, the given options are: 1) tempering metals, 2) providing phosphorus for fireworks, 3) acid neutralization, 4) the production of phosphoric acid, and 5) rubber vulcanization.
03

Analyze Phosphoric Acid Production

\(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) plays a significant role in the production of phosphoric acid. This compound is often treated with sulfuric acid to produce phosphoric acid and calcium sulfate as a by-product.
04

Conclusion

Given the well-known industrial process involving \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\), its major use is the production of phosphoric acid, widely used in fertilizers, food additives, and cleaning agents.

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!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Industrial Use of Calcium Phosphate
Calcium phosphate, chemically depicted as \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\), is a vital compound in numerous industrial processes. One of its most significant applications is in the manufacture of phosphoric acid. Given the diversity of minerals and chemical processes, calcium phosphate's industrial relevance cannot be overstated.
Industries widely utilize calcium phosphate for :
  • The production of fertilizers, which play a critical role in agriculture.
  • Food additives, enhancing nutritional value in various food products.
  • Cleaning agents, which include applications in personal care products and industrial cleaners.
These uses highlight the compound's critical role in improving agricultural output and in various consumer products.
Production of Phosphoric Acid
The production of phosphoric acid from calcium phosphate is an essential chemical reaction in industry. This process generally involves the reaction of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\) with sulfuric acid \(\mathrm{H}_{2}\mathrm{SO}_{4}\).
Here's how it works:
  • Calcium phosphate is treated with sulfuric acid.
  • This interaction yields phosphoric acid and calcium sulfate \((\mathrm{CaSO}_{4})\) as a by-product.
The reaction is represented by the equation:\[\mathrm{\mathrm{Ca}_{3}(\mathrm{PO}_{4})_{2} + 3 \mathrm{H}_{2}\mathrm{SO}_{4} \rightarrow 2\mathrm{H}_{3}\mathrm{PO}_{4} + 3\mathrm{CaSO}_{4}}\]This method efficiently produces phosphoric acid, significantly used in various industries, mainly fertilizer manufacturing.
Chemical Reactions of Calcium Phosphate
Calcium phosphate undergoes several chemical reactions, which highlight its versatility in different applications. The reaction with sulfuric acid to produce phosphoric acid is among the most critical.
Key reactions include:
  • Treatment with sulfuric acid to yield phosphoric acid and calcium sulfate, crucial for fertilizer production.
  • Reaction with nitric acid, often used in a different process to produce different forms of phosphates.
  • Calcium phosphate can also undergo thermal decomposition, producing phosphorus pentoxide, another valuable industrial chemical.
These reactions not only underscore the flexibility of calcium phosphate in synthetic applications but also demonstrate its pivotal role in industrial chemistry.
Applications in Industry
Calcium phosphate's applicability in industry extends beyond just chemical production. It is a multifaceted compound providing numerous industrial benefits.
Important industrial applications include:
  • Use in food production as a fortifying agent to enhance nutritional content.
  • In the pharmaceutical industry, calcium phosphate is used as an excipient in tablet production.
  • The manufacture of enamel and porcelain benefits from its use as a glaze substance.
Notably, colloidal and dispersible forms of calcium phosphate are used to stabilize creams and cosmetics, indicating its multifarious industrial uses.
Chemical Formulas
Understanding the chemical formulas of compounds like calcium phosphate is crucial for grasping their properties and reactions. Calcium phosphate is represented by \(\mathrm{Ca}_{3}(\mathrm{PO}_{4})_{2}\).
This formula indicates that each molecule contains:
  • Three calcium atoms \((\mathrm{Ca})\)
  • Two phosphate groups \((\mathrm{PO}_{4})\)
The phosphate group itself has an essential structure with one phosphorus atom bonded to four oxygen atoms.
Knowing these compositions helps in predicting and understanding chemical reactions, as it allows chemists to foresee how these molecules will interact with other substances, playing an integral role in both educational and practical chemical science.

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

Xenon trioxide, \(\mathrm{XeO}_{3},\) is reduced to xenon in acidic solution by iodide ion. Iodide ion is oxidized to iodine, \(\mathrm{I}_{2}\). Write a balanced chemical equation for the reaction.

Write balanced equations for each of the following. Solid calcium fluoride is heated with sulfuric acid to give hydrogen fluoride vapor. Solid potassium chlorate is carefully heated to yield potassium chloride and potassium perchlorate.

You have the following substances: \(\mathrm{NH}_{3}, \mathrm{O}_{2}, \mathrm{Pt},\) and \(\mathrm{H}_{2} \mathrm{O}\). Write equations for the preparation of \(\mathrm{N}_{2} \mathrm{O}\) from these substances.

Sulfur is formed in volcanic gases when sulfur dioxide reacts with hydrogen sulfide. The same reaction has been proposed as a method of removing sulfur dioxide from the gases emitted from coal-fired electricity generation plants. The emitted gases, containing sulfur dioxide, are bubbled through an aqueous solution of hydrogen sulfide. Write the balanced chemical equation for the reaction of sulfur dioxide gas with hydrogen sulfide gas to produce solid sulfur and water vapor. Suppose \(5.00 \mathrm{~L}\) of sulfur dioxide at \(748 \mathrm{mmHg}\) and \(22^{\circ} \mathrm{C}\) reacts with \(15.1 \mathrm{~g}\) of hydrogen sulfide. How many grams of sulfur would be produced?

Indicate the oxidation state for the element noted in each of the following: \(\begin{array}{ll}\text { H in } \mathrm{CaH}_{2} & \mathrm{~b} \mathrm{H} \text { in } \mathrm{H}_{2} \mathrm{O}\end{array}\) \(\mathrm{C}\) in \(\mathrm{CH}_{4}\) $$ \text { d } \mathrm{S} \text { in } \mathrm{H}_{2} \mathrm{SO}_{4} $$
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation

Chemistry Branches

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.