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Chapter 5: Problem 17

Write a balanced equation for reaction of the basic oxide, magnesium oxide, with water.

Short Answer

Expert verified
\( \text{MgO} + \text{H}_2\text{O} \rightarrow \text{Mg(OH)}_2 \) is the balanced equation.

Step by step solution

01

Identify the Chemical Components

The basic oxide given in this problem is magnesium oxide, which has the chemical formula \( \text{MgO} \). It reacts with water, which is \( \text{H}_2\text{O} \). We need to identify both reactants to write the chemical equation.
02

Determine the Products of Reaction

A basic oxide reacts with water to form a basic hydroxide. When magnesium oxide reacts with water, it will form magnesium hydroxide. The chemical formula for magnesium hydroxide is \( \text{Mg(OH)}_2 \).
03

Write the Unbalanced Chemical Equation

Based on the reactants and products, the unbalanced equation for the reaction is \( \text{MgO} + \text{H}_2\text{O} \rightarrow \text{Mg(OH)}_2 \).
04

Balance the Chemical Equation

Check if the equation is balanced by counting the number of atoms on each side. In this equation, we have 1 magnesium atom, 2 oxygen atoms, and 2 hydrogen atoms on both sides. Since the number of each type of atom is equal on both sides, the equation is already balanced.

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Key Concepts

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

Magnesium Oxide
Magnesium oxide is a simple compound consisting of magnesium and oxygen atoms. It is represented chemically as \( \text{MgO} \). This compound is known as a basic oxide because it has the ability to react with water, forming a base. Magnesium oxide is commonly encountered in chemistry and everyday products like antacids.

When magnesium oxide comes into contact with water, a chemical reaction takes place. This reaction is significant in various fields, including material science and environmental chemistry. Understanding magnesium oxide鈥檚 tendency to form hydroxide compounds with water provides insights into its practical applications.
  • Magnesium oxide plays a crucial role in reactions that involve neutralization, where it reduces acidity.
  • As a refractory material, it withstands high temperatures, crucial for applications requiring heat resistance.
Magnesium Hydroxide
Magnesium hydroxide is the product formed when magnesium oxide reacts with water. Its chemical formula is \( \text{Mg(OH)}_2 \), indicating that it contains magnesium, oxygen, and hydrogen atoms. This compound is often utilized in medicine as an antacid and laxative.

When seen from a chemical perspective, magnesium hydroxide is a base, meaning it can neutralize acids in chemical reactions, a process critical in digestion and industrial applications. It exhibits limited solubility in water, forming a milky suspension known as milk of magnesia.

Here's why magnesium hydroxide is important:
  • It鈥檚 a safe, effective component used in over-the-counter medications for stomach discomfort.
  • Its basic nature makes it suitable for neutralizing acidic environments, both in the laboratory and in the body.
Chemical Reaction Steps
To understand any chemical reaction, we break it down into steps for clarity. This helps in visualizing how reactants transform into products, step by step.

For instance, in the reaction between magnesium oxide and water:
  • Step 1: Identify the Reactants: Here, we begin by identifying magnesium oxide and water as the reactants.
  • Step 2: Anticipate the Products: Mixing a basic oxide with water typically results in the formation of a hydroxide, which is magnesium hydroxide in this context.
  • Step 3: Form the Unbalanced Equation: Initial setup gives us \( \text{MgO} + \text{H}_2\text{O} \rightarrow \text{Mg(OH)}_2 \).
  • Step 4: Balance the Equation: This final step ensures that the number of atoms on each side of the reaction is equal, confirming the law of conservation of mass is followed.
Mastering these steps is essential in chemistry for ensuring calculations and predictions are accurate and reliable.

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Most popular questions from this chapter

Complete and balance the following acid-base reactions. Name the reactants and products. (a) \(\mathrm{H}_{3} \mathrm{PO}_{4}(\mathrm{aq})+\mathrm{KOH}(\mathrm{aq}) \longrightarrow\) (b) \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s}) \longrightarrow\) $$\left(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\right.$$ is oxalic acid, an acid capable of donating two $$\left.\mathrm{H}^{+} \text {ions. }\right)$$

A Two students titrate different samples of the same solution of HCl using \(0.100 \mathrm{M} \mathrm{NaOH}\) solution and phenolphthalein indicator (see Figure 5.23). The first student pipets \(20.0 \mathrm{mL}\) of the HCl solution into a flask, adds 20 mL of distilled water and a few drops of phenolphthalein solution, and titrates until a lasting pink color appears. The second student pipets \(20.0 \mathrm{mL}\), of the HCl solution into a flask, adds 60 mL. of distilled water and a few drops of phenolphthalein solution, and titrates to the first lasting pink color. Each student correctly calculates the molarity of a HCl solution. What will the second student's result be? (a) four times less than the first student's result (b) four times greater than the first student's result (c) two times less than the first student's result (d) two times greater than the first student's result (e) the same as the first student's result

(a) What is the pH of a 0.105 M HCl solution? (b) What is the hydrogen ion concentration in a solution with a pH of \(2.56 ?\) Is the solution acidic or basic? (c) A solution has a pH of 9.67. What is the hydrogen ion concentration in the solution? Is the solution acidic or basic? (d) \(A 10.0\) -mL. sample of \(2.56 \mathrm{M}\) HCl is diluted with water to \(250 .\) mL. What is the pH of the dilute solution?

A One-half liter \((500 . \mathrm{mL})\) of \(2.50 \mathrm{M} \mathrm{HCl}\) is mixed with \(250 .\) mL of \(3.75 \mathrm{M} \mathrm{HCl}\). Assuming the total solution volume after mixing is \(750 . \mathrm{mL}\), what is the concentration of hydrochloric acid in the resulting solution? What is its \(\mathrm{pH} ?\)

Write a balanced equation for the reaction of barium hydroxide with nitric acid.
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