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Chapter 7: Problem 90

When carbon dioxide is bubbled through a clear calcium hydroxide solution, the solution appears milky. Write an equation for the reaction, and explain how this reaction illustrates that \(\mathrm{CO}_{2}\) is an acidic oxide.

Short Answer

Expert verified
CO2 reacts with Ca(OH)2 to form CaCO3 and H2O, illustrating CO2 as an acidic oxide.

Step by step solution

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01

Understand the Reaction

When carbon dioxide (\(\mathrm{CO}_2\)) is bubbled through a calcium hydroxide (\(\mathrm{Ca(OH)_2}\)) solution, the solution becomes milky due to the formation of calcium carbonate (\(\mathrm{CaCO_3}\)). This reaction illustrates a chemical transformation where \(\mathrm{CO}_2\) behaves as an acidic oxide.
02

Write the Chemical Equation

The reaction between carbon dioxide and calcium hydroxide can be represented by the following equation: \[ \mathrm{CO_2 (g) + Ca(OH)_2 (aq) \rightarrow CaCO_3 (s) + H_2O (l)} \]This equation shows that \(\mathrm{CO_2}\) reacts with \(\mathrm{Ca(OH)_2}\) to form calcium carbonate (solid, precipitate) and water.
03

Explain the Reaction as \(\mathrm{CO}_2\) being an Acidic Oxide

An oxide is termed acidic if it reacts with a base to form a salt and water. In this reaction, \(\mathrm{CO_2}\) acts as an acidic oxide because it reacts with the base \(\mathrm{Ca(OH)_2}\) (a hydroxide) to produce a salt (calcium carbonate) and water. Thus, the reaction confirms the acidic nature of \(\mathrm{CO}_2\) as per the classical definition of acidic oxides.

Key Concepts

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

Calcium Hydroxide
Calcium hydroxide, chemically written as \(\mathrm{Ca(OH)_2}\), is a noteworthy compound in chemistry. Often used in various applications, it is commonly known as slaked lime.

One of its key properties is being a strong base. This means that it can readily donate hydroxide ions (\(\mathrm{OH^-}\)) in solution.
When it dissolves in water, it dissociates to form calcium ions and hydroxide ions, making the solution basic:
  • Calcium ions: \(\mathrm{Ca^{2+}}\)
  • Hydroxide ions: \(\mathrm{OH^-}\)
This basic solution will often react with gases like carbon dioxide (\(\mathrm{CO_2}\)) in the air.

It's crucial to remember that the basic nature of calcium hydroxide makes it ideal for neutralizing acidic substances. Hence, when \(\mathrm{CO_2}\) is bubbled through it, we observe a reaction that demonstrates both the basicity of \(\mathrm{Ca(OH)_2}\) and the acidic nature of \(\mathrm{CO_2}\).
Calcium Carbonate
Calcium carbonate is an interesting compound with the chemical formula \(\mathrm{CaCO_3}\).

It's a white, insoluble solid that often appears as a precipitate in chemical reactions between strong bases and acidic gases like \(\mathrm{CO_2}\).
In everyday life, calcium carbonate is found in various natural forms, such as limestone, chalk, and marble. One of the key features of \(\mathrm{CaCO_3}\) is its role in the reaction with calcium hydroxide and carbon dioxide:
  • The \(\mathrm{CO_2}\) gas reacts with the \(\mathrm{Ca(OH)_2}\) solution to form calcium carbonate.

  • This reaction forms a cloudy or milky suspension due to the solid \(\mathrm{CaCO_3}\) particles, observable as a white precipitate.
This reaction is essential not only in illustrating the interaction between acidic oxides and bases but also in numerous industrial applications such as the production of building materials and environmental applications like water treatment.
Chemical Reaction Equation
The concept of a chemical reaction equation is integral to understanding how substances interact and transform. A chemical equation is a symbolic representation where the reactants are transformed into products.

Key features to note:
  • Reactants are placed on the left side, and products on the right side of the equation.

  • Equations must be balanced, meaning the number of each type of atom on both sides should be equal.

  • States of matter (solid, liquid, gas, aqueous) are indicated, usually in parentheses.
In the reaction involving \(\mathrm{CO_2}\) and \(\mathrm{Ca(OH)_2}\):
  • \(\mathrm{CO_2 (g)}\) and \(\mathrm{Ca(OH)_2 (aq)}\) are reactants combining to form \(\mathrm{CaCO_3 (s)}\) and \(\mathrm{H_2O (l)}\).
  • This reaction represents the interaction of an acidic oxide and a base, forming a salt (calcium carbonate) and water, illustrating classic acid-base reaction properties.
Understanding and writing chemical reaction equations accurately is critical in predicting and explaining the outcomes of chemical interactions.

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Most popular questions from this chapter

Predict the products of the following oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}, \mathrm{~N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions. Specify whether the oxides are acidic, basic, or amphoteric.

What is the most reactive element on the periodic table?

Which is the smallest atom in Group \(7 \mathrm{~A}\) ?

On the basis of their positions in the periodic table, select the atom with the larger atomic radius in each of the following pairs: (a) \(\mathrm{Na}\), Si; (b) \(\mathrm{Ba}, \mathrm{Be} ;(\mathrm{c}) \mathrm{N}, \mathrm{F}\) (d) \(\mathrm{Br}, \mathrm{Cl} ;(\mathrm{e}) \mathrm{Ne}, \mathrm{Kr}\).

Write the ground-state electron configurations of the following ions: (a) \(\mathrm{Li}^{+},(\mathrm{b}) \mathrm{H}^{-},(\mathrm{c}) \mathrm{N}^{3-},(\mathrm{d}) \mathrm{F}^{-},\) (e) \(\mathrm{S}^{2-}\) (f) \(\mathrm{Al}^{3+},(\mathrm{g}) \mathrm{Se}^{2-}\) (h) \(\mathrm{Br}^{-}\) (i) \(\mathrm{Rb}^{+},(\mathrm{j}) \mathrm{Sr}^{2+},(\mathrm{k}) \mathrm{Sn}^{2+}\) (1) \(\mathrm{Te}^{2-} \cdot(\mathrm{m}) \mathrm{Ba}^{2+}\) (n) \(\mathrm{Pb}^{2+}\) (o) \(\mathrm{In}^{3+},(\mathrm{p}) \mathrm{Tl}^{+}\) (a) \(\mathrm{Tl}^{3+}\)
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