/*! 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 51 Magnesium ions are removed in wa... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 18: Problem 51

Magnesium ions are removed in water treatment by the addition of slaked lime, \(\mathrm{Ca}(\mathrm{OH})_{2}\). Write a balanced chemical equation to describe what occurs in this process.

Short Answer

Expert verified
The balanced chemical equation for the removal of magnesium ions in water treatment by the addition of slaked lime is: \[ \mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{Mg}(\mathrm{OH})_{2} + \mathrm{Ca}^{2+} \]

Step by step solution

01

Write the unbalanced chemical equation

Write the unbalanced chemical equation for the removal of magnesium ions (Mg虏鈦�) in water treatment by the addition of slaked lime (Ca(OH)鈧�). \[ \mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \]
02

Identify the products of the reaction

The reaction between magnesium ions and slaked lime will produce magnesium hydroxide (Mg(OH)鈧�), a solid precipitate, and calcium ions (Ca虏鈦�): \[ \mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{Mg}(\mathrm{OH})_{2} + \mathrm{Ca}^{2+} \]
03

Balance the chemical equation

To balance the chemical equation, make sure the number of atoms of each element is equal on both the reactant and product side of the equation. The unbalanced equation is \[ \mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{Mg}(\mathrm{OH})_{2} + \mathrm{Ca}^{2+} \] Looking at the equation, we have one Mg虏鈦� ion, one Ca虏鈦� ion, and two OH鈦� ions on both sides of the equation, so the equation is already balanced: Balanced chemical equation: \[ \mathrm{Mg}^{2+} + \mathrm{Ca}(\mathrm{OH})_{2} \rightarrow \mathrm{Mg}(\mathrm{OH})_{2} + \mathrm{Ca}^{2+} \]

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.

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.

Chemical Reactions in Water Treatment
Ensuring that water is clean and safe for consumption is essential, and chemical reactions play a fundamental role in the treatment process.

During water treatment, various contaminants are removed, including bacteria, organic compounds, and inorganic minerals such as magnesium. The removal of magnesium ions (Mg虏鈦�) involves a chemical reaction where a reagent, such as slaked lime (Ca(OH)鈧�), is added to the water. This reaction is vital for softening water, as magnesium can cause hardness, which is undesirable for many everyday uses.

By understanding the chemistry behind water treatment, we improve the efficiency and effectiveness of the purification process, making it not only a technical endeavor but also a scientific one that hinges on precise chemical changes.
Precipitation Reaction
A precipitation reaction is a vital type of chemical reaction where soluble ions in a solution react to form insoluble compounds that precipitate out of the solution as a solid.

In our example, when slaked lime is added to water containing magnesium ions, magnesium hydroxide (Mg(OH)鈧�) is formed. This new compound is not soluble in water and hence precipitates out as a solid. This process can be visually observed and is a critical step in water treatment for removing certain ions, such as magnesium.

Precipitation reactions are not only important in environmental applications but are also extensively used in various industries, including pharmaceuticals and metallurgy. By identifying the insoluble compounds that form, we can predict and utilize precipitation reactions for numerous practical applications.
Stoichiometry
Stoichiometry is the part of chemistry that deals with the quantities of substances involved in reactions.

It enables us to understand the proportions in which different substances react and to predict the amounts of products formed. For a balanced chemical equation, such as the one between magnesium ions and slaked lime, stoichiometry tells us that one mole of Mg虏鈦� reacts with one mole of Ca(OH)鈧� to produce one mole of Mg(OH)鈧� and one mole of Ca虏鈦�.

This stoichiometric relationship is key to designing processes with the correct amounts of reactants, ensuring that the reaction proceeds efficiently and that resources are not wasted. For students tackling chemistry problems, a strong grasp of stoichiometry is indispensable for solving quantitative exercises and understanding the fundamental principles underlying chemical reactions.

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

In the following three instances, which choice is greener in each situation? Explain. (a) Benzene as a solvent or water as a solvent. (b) The reaction temperature is 500 \(\mathrm{K}\) or 1000 \(\mathrm{K}\) . (c) Sodium chloride as a by-product or chloroform \(\left(\mathrm{CHCl}_{3}\right)\) as a by-product.

In the lime soda process once used in large scale municipal water softening, calcium hydroxide prepared from lime and sodium carbonate are added to precipitate \(\mathrm{Ca}^{2+}\) as \(\mathrm{CaCO}_{3}(s)\) and \(\mathrm{Mg}^{2+}\) as \(\mathrm{Mg}(\mathrm{OH})_{2}(s) :\) $$\begin{array}{c}{\mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q) \longrightarrow \mathrm{CaCO}_{3}(s)} \\ {\mathrm{Mg}^{2+}(a q)+2 \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{MgOH}_{2}(a q)}\end{array}$$ How many moles of \(\mathrm{Ca}(\mathrm{OH})_{2}\) and \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) should be added to soften (remove the \(\mathrm{Ca}^{2+}\) and \(\mathrm{Mg}^{2+} ) 1200 \mathrm{L}\) of water in which $$\begin{array}{l}{\left[\mathrm{Ca}^{2+}\right]=5.0 \times 10^{-4} M \text { and }} \\ {\left[\mathrm{Mg}^{2+}\right]=7.0 \times 10^{-4} \mathrm{M?}}\end{array}$$

The average bond enthalpies of the \(\mathrm{C}-\mathrm{F}\) and \(\mathrm{C}-\) Cl bonds are 485 \(\mathrm{kJ} / \mathrm{mol}\) and 328 \(\mathrm{kJ} / \mathrm{mol}\) , respectively. (a) What is the maximum wavelength that a photon can possess and still have sufficient energy to break the \(\mathrm{C}-\mathrm{F}\) and \(\mathrm{C}-\mathrm{Cl}\) bonds, respectively? (b) Given the fact that \(\mathrm{O}_{2}, \mathrm{N}_{2},\) and \(\mathrm{O}\) in the upper atmosphere absorb most of the light with wavelengths shorter than \(240 \mathrm{nm},\) would you expect the photodissociation of \(\mathrm{C}-\mathrm{F}\) bonds to be significant in the lower atmosphere?

What properties of CFCs make them ideal for various commercial applications but also make them a long-term problem in the stratosphere?

The atmosphere of Mars is \(96 \% \mathrm{CO}_{2},\) with a pressure of approximately \(6 \times 10^{-3}\) atm at the surface. Based on measurements taken over a period of several years by the Rover Environmental Monitoring Station (REMS), the average daytime temperature at the REMS location on Mars is \(-5.7^{\circ} \mathrm{C}\left(22^{\circ} \mathrm{F}\right),\) while the average nighttime temperature is \(-79^{\circ} \mathrm{C}\left(-109^{\circ} \mathrm{F}\right) .\) This daily variation in temperature is much larger than what we experience on Earth. What factor plays the largest role in this wide temperature variation, the composition or the density of the atmosphere?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

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.