Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
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![**Acid-Base Reaction: Net Ionic Equation**
**Problem Statement:**
Write the net ionic equation for the reaction for the following acid-base reaction:
\[ \text{Ca(OH)}_2 (aq) + 2 \text{HCl} (aq) \rightarrow 2 \text{H}_2\text{O} (l) + \text{CaCl}_2 (aq) \]
**Explanation:**
The given reaction is a neutralization reaction where calcium hydroxide \(\text{Ca(OH)}_2\) reacts with hydrochloric acid (\(\text{HCl}\)) to form water \(\left( \text{H}_2\text{O} \right)\) and aqueous calcium chloride (\(\text{CaCl}_2\)).
**Steps to Find the Net Ionic Equation:**
1. **Write the balanced molecular equation:**
\[ \text{Ca(OH)}_2 (aq) + 2 \text{HCl} (aq) \rightarrow 2 \text{H}_2\text{O} (l) + \text{CaCl}_2 (aq) \]
2. **Write the complete ionic equation by dissociating all strong electrolytes into their ions.**
\[ \text{Ca}^{2+} (aq) + 2 \text{OH}^- (aq) + 2 \text{H}^+ (aq) + 2 \text{Cl}^- (aq) \rightarrow 2 \text{H}_2\text{O} (l) + \text{Ca}^{2+} (aq) + 2 \text{Cl}^- (aq) \]
3. **Identify and cancel the spectator ions (ions that appear on both sides of the equation):**
Spectator ions: \(\text{Ca}^{2+} (aq)\) and \(\text{Cl}^- (aq)\)
4. **Write the net ionic equation by including only those components that undergo a chemical change:**
\[ 2 \text{OH}^- (aq) + 2 \text{H}^+ (aq) \rightarrow 2 \text{H}_2\text{O} (l) \]
5. **Simplify the equation if possible:**
\[ \text{OH}^- (aq) + \text{H}^+ (](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F776f865c-aff7-4060-8b66-2ed96dd6121a%2F4c5161fe-3070-47d9-ac2a-0e1f7fc1ca83%2F38g28k9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Acid-Base Reaction: Net Ionic Equation**
**Problem Statement:**
Write the net ionic equation for the reaction for the following acid-base reaction:
\[ \text{Ca(OH)}_2 (aq) + 2 \text{HCl} (aq) \rightarrow 2 \text{H}_2\text{O} (l) + \text{CaCl}_2 (aq) \]
**Explanation:**
The given reaction is a neutralization reaction where calcium hydroxide \(\text{Ca(OH)}_2\) reacts with hydrochloric acid (\(\text{HCl}\)) to form water \(\left( \text{H}_2\text{O} \right)\) and aqueous calcium chloride (\(\text{CaCl}_2\)).
**Steps to Find the Net Ionic Equation:**
1. **Write the balanced molecular equation:**
\[ \text{Ca(OH)}_2 (aq) + 2 \text{HCl} (aq) \rightarrow 2 \text{H}_2\text{O} (l) + \text{CaCl}_2 (aq) \]
2. **Write the complete ionic equation by dissociating all strong electrolytes into their ions.**
\[ \text{Ca}^{2+} (aq) + 2 \text{OH}^- (aq) + 2 \text{H}^+ (aq) + 2 \text{Cl}^- (aq) \rightarrow 2 \text{H}_2\text{O} (l) + \text{Ca}^{2+} (aq) + 2 \text{Cl}^- (aq) \]
3. **Identify and cancel the spectator ions (ions that appear on both sides of the equation):**
Spectator ions: \(\text{Ca}^{2+} (aq)\) and \(\text{Cl}^- (aq)\)
4. **Write the net ionic equation by including only those components that undergo a chemical change:**
\[ 2 \text{OH}^- (aq) + 2 \text{H}^+ (aq) \rightarrow 2 \text{H}_2\text{O} (l) \]
5. **Simplify the equation if possible:**
\[ \text{OH}^- (aq) + \text{H}^+ (
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