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Chapter 4: Problem 87

Explain how a mixture of anion and cation exchangers can be used to deionize water.

Short Answer

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Question: Explain how a mixture of anion and cation exchangers can be used to deionize water. Answer: A mixture of anion and cation exchangers can be used to deionize water by first passing the water through a cation exchanger containing H+ ions, which removes unwanted cations and replaces them with H+ ions. Next, the water is passed through an anion exchanger containing OH- ions, which removes unwanted anions and replaces them with OH- ions. The H+ and OH- ions combine to form water molecules, effectively neutralizing the solution and resulting in deionized water with no residual cations or anions present.

Step by step solution

01

1. Understanding Anions and Cations

Anions are negatively charged ions while cations are positively charged ions. In water, many dissolved salts are present in the form of these ions (for example, Na+ and Cl- in table salt).
02

2. Ion Exchange Process

Ion exchange is a process where unwanted ions present in a solution are replaced by other ions with a similar charge. An ion exchange resin is used, which has ions attached to a solid support. When the resin comes into contact with the solution containing unwanted ions, the ions on the resin are exchanged with those in the solution.
03

3. Cation Exchangers

Cation exchangers are ion exchange resins where the attached ions are cations. They are used to remove unwanted cations from a solution by exchanging them with ions present on the resin. For example, a common cation exchanger uses hydrogen ions (H+) as the exchanging cations.
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4. Anion Exchangers

Anion exchangers are ion exchange resins where the attached ions are anions. They are used to remove unwanted anions from a solution by exchanging them with ions present on the resin. For example, a common anion exchanger uses hydroxide ions (OH-) as the exchanging anions.
05

5. Deionization of Water

Deionization of water involves removing dissolved salts in the water by removing both cations and anions. This process ensures that the water is free from any dissolved ions and suitable for use in different applications, such as laboratory experiments and certain industrial processes.
06

6. Using a Mixture of Anion and Cation Exchangers

To deionize water, a mixture of anion and cation exchangers can be used. The cation exchanger will remove the cations by exchanging them with H+ ions, while the anion exchanger will remove the anions by exchanging them with OH- ions. When these two exchangers are used together, both cations and anions are removed, thus deionizing the water. Here is a summary of the step-by-step process: 1. Pass the water through a cation exchanger containing H+ ions. The unwanted cations in the water are replaced by H+ ions, resulting in a slightly acidic solution. 2. Pass the slightly acidic water through an anion exchanger containing OH- ions. The unwanted anions in the water are replaced by OH- ions, which then combine with the H+ ions present in the water to form water molecules, effectively neutralizing the solution. 3. The resulting water is now deionized, with no residual cations or anions. This method can effectively deionize water by using a combination of anion and cation exchangers to remove unwanted ions and produce deionized water that meets the specific requirements of various applications.

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Key Concepts

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

Ion Exchange Process
Ion exchange is a fascinating chemical process used to purify, separate, and decontaminate solutions. It is widely recognized for its effectiveness in removing unwanted ions from a solution. Here鈥檚 how it works:
  • It involves ion exchange resins, which are polymers that act as media for the exchange process.
  • These resins contain positively or negatively charged ions attached to them.
  • When these resins interact with a solution containing unwanted ions, the resin's ions trade places with the unwanted ones.
This swapping of ions helps purify the solution by replacing harmful or undesired ions with harmless or beneficial ones. The entire process can be thought of as a highly selective filtration method, where certain ions are retained while others are discarded. Through this method, water can be purified, as unwanted ions are replaced by those present on the resin, such as H+ or OH-.
Such a process can be pivotal in industrial settings, laboratories, and even in the production of drinking water.
Cation Exchangers
Cation exchangers are specialized ion exchange resins designed to specifically remove cations, which are positively charged ions in the water.
  • In cation exchanger systems, the resin beads hold onto hydrogen ions (H+) or other positive ions.
  • When cation-rich water is passed over these beads, the unwanted cations in the water, like calcium (Ca2+) or sodium (Na+), are replaced with H+ ions.
  • This substitution results in the elimination of cations from the water, essentially purifying it.
The process is important in contexts where mineral content needs to be reduced, thus softening the water. Hard water, which is rich in calcium and magnesium, can be softened using cation exchangers, making it more compatible with certain industrial and domestic applications.
Anion Exchangers
Anion exchangers target negatively charged ions, known as anions, in the water. These ion exchange resins are integral in achieving complete deionization when used alongside cation exchangers.
  • They operate by substituting undesired anions in the solution with hydroxide ions (OH-).
  • For instance, when chloride (Cl-) or sulfate (SO4(2-)) ions are present, they are exchanged for the OH- ions on the resin.
  • The substitution is vital for neutralizing the water once both anions and cations are removed.
After cation exchange has replaced positive ions with H+, anion exchange takes the subsequent step by replacing negative ions with OH-. When the two are combined, they produce H2O, or water molecules, effectively deionizing the water. This removal process is fundamental in ensuring the water's suitability for applications requiring minimal ion content, such as in scientific laboratories or in certain industrial settings.

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Most popular questions from this chapter

Write the net ionic equation for the neutralization of a strong acid by a strong base.

Earth's Crust The following chemical reactions have helped to shape Earth's crust. Determine the oxidation numbers of all the elements in the reactants and products, and identify which elements are oxidized and which are reduced. a. \(3 \mathrm{SiO}_{2}(s)+2 \mathrm{Fe}_{3} \mathrm{O}_{4}(s) \rightarrow 3 \mathrm{Fe}_{2} \mathrm{SiO}_{4}(s)+\mathrm{O}_{2}(g)\) b. \(\operatorname{SiO}_{2}(s)+2 \operatorname{Fe}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{Fe}_{2} \mathrm{SiO}_{4}(s)\) c. \(4 \mathrm{FeO}(s)+\mathrm{O}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(\ell) \rightarrow 4 \mathrm{Fe}(\mathrm{OH})_{3}(s)\)

(a) Use the solubility rules to write the balanced net ionic equation for each of the following "molecular" reactions. If there is no net reaction, write "NR." (b) Which of these three reactions give clear visual evidence of the ion exchange process? 1\. \(\mathrm{BaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow \mathrm{BaCO}_{3}(s)+\mathrm{NaCl}(a q)\) 2\. \(\mathrm{NaCl}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{NaOH}(a q)+\mathrm{KCl}(a q)\) 3\. \(\mathrm{Na}_{3} \mathrm{PO}_{4}(a q)+\mathrm{CaCl}_{2}(a q) \rightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\mathrm{NaCl}(a q)\)

Behavior of Honey Honey is a concentrated solution of sugar molecules in water. Clear, viscous honey becomes cloudy after being stored for long periods. Explain how this transition illustrates supersaturation.

Toxic chromate can be precipitated from an aqueous solution by bubbling \(\mathrm{SO}_{2}\) through the solution. How many grams of \(\mathrm{SO}_{2}\) are required to treat \(3.0 \times 10^{8} \mathrm{L}\) of \(0.050 \mathrm{mM} \mathrm{CrO}_{4}^{-} ?\) $$\begin{aligned} &2 \mathrm{CrO}_{4}^{2-}(a q)+3 \mathrm{SO}_{2}(g)+4 \mathrm{H}^{+}(a q) \rightarrow\\\ &\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}(s)+2 \mathrm{H}_{2} \mathrm{O}(\ell) \end{aligned}$$
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