Match List I with List II and select the correct answer using the code given below the Lists: List I (Compound) List II (Nature) A. Sodium hydroxide 1. Strong acid B. Calcium oxide 2. Alkali C. Acetic acid 3. Weak acid D. Hydrochloric acid 4. Base
A - 2, B - 4, C - 3, D - 1
Matching Compounds with their Chemical Nature
This question asks us to match a list of chemical compounds with their corresponding chemical nature from a second list. To solve this, we need to identify whether each compound is an acid, base, alkali, or a specific type like strong acid or weak acid.
Analysis of Each Compound
Let's examine each compound from List I and determine its nature based on general chemical properties:
- A. Sodium hydroxide ($\text{NaOH}$): Sodium hydroxide is an ionic compound and a strong base. It dissolves readily in water to form a solution containing sodium ions ($\text{Na}^+$) and hydroxide ions ($\text{OH}^-$). Bases that are soluble in water are called alkalis. Therefore, Sodium hydroxide is an Alkali.
- B. Calcium oxide ($\text{CaO}$): Calcium oxide is a metal oxide. Metal oxides are generally basic in nature. When Calcium oxide reacts with water, it forms Calcium hydroxide ($\text{Ca(OH)}_2$), which is a base. Although Calcium hydroxide is only sparingly soluble, Calcium oxide itself is considered a basic oxide, leading to a basic solution when it reacts with water. Therefore, Calcium oxide is a Base.
- C. Acetic acid ($\text{CH}_3\text{COOH}$): Acetic acid is an organic acid. It is the main component of vinegar. Unlike strong acids, acetic acid does not completely dissociate in water, meaning only a fraction of its molecules donate protons ($\text{H}^+$). Acids that do not dissociate completely in water are classified as weak acids. Therefore, Acetic acid is a Weak acid.
- D. Hydrochloric acid ($\text{HCl}$): Hydrochloric acid is a solution of hydrogen chloride gas in water. It is a mineral acid. Hydrochloric acid is known to dissociate completely in water, releasing hydrogen ions ($\text{H}^+$) and chloride ions ($\text{Cl}^-$). Acids that dissociate completely in water are classified as strong acids. Therefore, Hydrochloric acid is a Strong acid.
Matching List I with List II
Based on our analysis, we can make the following matches:- A. Sodium hydroxide matches with 2. Alkali
- B. Calcium oxide matches with 4. Base
- C. Acetic acid matches with 3. Weak acid
- D. Hydrochloric acid matches with 1. Strong acid
Summary of Matches
| List I (Compound) | List II (Nature) | Match |
|---|---|---|
| A. Sodium hydroxide | 2. Alkali | A - 2 |
| B. Calcium oxide | 4. Base | B - 4 |
| C. Acetic acid | 3. Weak acid | C - 3 |
| D. Hydrochloric acid | 1. Strong acid | D - 1 |
The correct combination of matches is A - 2, B - 4, C - 3, D - 1.
Revision Table: Compounds and Nature
| Compound | Chemical Formula | Nature | Reason/Classification |
|---|---|---|---|
| Sodium hydroxide | $\text{NaOH}$ | Alkali (Strong Base) | Soluble metal hydroxide |
| Calcium oxide | $\text{CaO}$ | Base (Basic Oxide) | Metal oxide reacts with water to form base |
| Acetic acid | $\text{CH}_3\text{COOH}$ | Weak acid | Organic acid, partial dissociation |
| Hydrochloric acid | $\text{HCl}$ | Strong acid | Mineral acid, complete dissociation |
Additional Information: Acids, Bases, and Alkalis
Understanding the definitions of acids, bases, and alkalis is crucial for classifying compounds:
- Acids: Substances that donate protons ($\text{H}^+$ ions) or accept electron pairs. In water, they increase the concentration of $\text{H}^+$ ions.
- Bases: Substances that accept protons ($\text{H}^+$ ions) or donate electron pairs. Many bases are hydroxides that produce $\text{OH}^-$ ions in water. Metal oxides are also considered basic as they react with water to form bases.
- Alkalis: These are bases that are soluble in water. All alkalis are bases, but not all bases are alkalis (since some bases are insoluble or sparingly soluble in water). Examples include Sodium hydroxide and Potassium hydroxide.
- Strong Acids: Acids that dissociate almost completely in water, releasing a high concentration of $\text{H}^+$ ions. Examples: $\text{HCl}$, $\text{HNO}_3$, $\text{H}_2\text{SO}_4$.
- Weak Acids: Acids that only partially dissociate in water, releasing a lower concentration of $\text{H}^+$ ions. Examples: $\text{CH}_3\text{COOH}$, $\text{H}_2\text{CO}_3$.
- Strong Bases: Bases that dissociate almost completely in water, releasing a high concentration of $\text{OH}^-$ ions. Examples: $\text{NaOH}$, $\text{KOH}$.
- Weak Bases: Bases that only partially dissociate or react with water to produce $\text{OH}^-$ ions. Example: $\text{NH}_3$.
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