Difference Between Acid and Base in Tabular Form (Class 7, 9, 10, 12)
The concept of Difference Between Acid and Base is essential in chemistry and helps students understand various practical and theoretical applications related to this topic.
What is Difference Between Acid and Base in Chemistry?
A difference between acid and base refers to the fundamental distinctions in their chemical nature, definitions, properties, and reactions. This concept appears in chapters related to chemical reactions, acids, bases, and salts, and pH scale, making it a foundational part of your chemistry syllabus.
Acid and Base: Definitions with Examples
Acids are substances that release hydrogen ions (H⁺) in water. They taste sour, turn blue litmus paper red, and usually have a pH value less than 7. Examples include hydrochloric acid (HCl), lemon juice (citric acid), and vinegar (acetic acid).
Bases are substances that release hydroxide ions (OH⁻) in water or accept hydrogen ions. They taste bitter, feel slippery, turn red litmus paper blue, and have a pH value greater than 7. Common base examples are sodium hydroxide (NaOH), milk of magnesia (magnesium hydroxide), and baking soda (sodium bicarbonate).
Difference Between Acid and Base Table
Below is a simple table highlighting the difference between acid and base on key points. This table is useful for quick revision and exam preparation.
| Acid | Base |
|---|---|
| Sour taste | Bitter taste |
| Turns blue litmus paper red | Turns red litmus paper blue |
| pH less than 7 | pH greater than 7 |
| Reacts with metals to produce hydrogen gas | Feels slippery/soapy |
| Corrosive (especially strong acids) | Caustic (especially strong bases) |
| Example: HCl, H2SO4, Lemon juice | Example: NaOH, Soap, Baking soda |
Properties of Acids and Bases in Detail
Properties of Acids
- Produce H⁺ ions in aqueous solutions
- Turn blue litmus red
- React with metals releasing hydrogen gas
- Corrosive and sour
- Conduct electricity
Properties of Bases
- Produce OH⁻ ions in aqueous solutions
- Turn red litmus blue
- Feel slippery, taste bitter
- Can be caustic and damage skin
- Conduct electricity
Theoretical Differences: Arrhenius, Brønsted-Lowry, and Lewis Concepts
| Theory | Acid | Base |
|---|---|---|
| Arrhenius | Produces H⁺ in water | Produces OH⁻ in water |
| Brønsted-Lowry | Proton (H⁺) donor | Proton (H⁺) acceptor |
| Lewis | Electron pair acceptor | Electron pair donor |
Quick Examples: 10 Acids & 10 Bases (Formula & Uses)
| Acid | Formula | Common Use |
|---|---|---|
| Hydrochloric acid | HCl | Stomach acid, cleaning |
| Sulfuric acid | H2SO4 | Car batteries |
| Nitric acid | HNO3 | Fertilizer, explosives |
| Acetic acid | CH3COOH | Vinegar |
| Citric acid | C6H8O7 | Food flavoring |
| Lactic acid | C3H6O3 | Milk, yoghurt |
| Ascorbic acid | C6H8O6 | Vitamin C |
| Phosphoric acid | H3PO4 | Soft drinks |
| Formic acid | HCOOH | Ant and bee stings |
| Oxalic acid | C2H2O4 | Cleaning, bleach |
| Base | Formula | Common Use |
|---|---|---|
| Sodium hydroxide | NaOH | Soap making, drain cleaner |
| Potassium hydroxide | KOH | Soaps, batteries |
| Calcium hydroxide | Ca(OH)2 | Lime water, whitewash |
| Ammonium hydroxide | NH4OH | Household cleaning |
| Magnesium hydroxide | Mg(OH)2 | Milk of magnesia |
| Baking soda (Sodium bicarbonate) | NaHCO3 | Baking, antacid |
| Bleach (Sodium hypochlorite) | NaClO | Disinfectant |
| Limewater | Ca(OH)2 | Test for CO2 |
| Soap | - | Cleaning |
| Ammonia solution | NH3 (aq) | Fertilizers, cleaning |
Practical Importance: Neutralization Reaction
Neutralization occurs when an acid reacts with a base, producing salt and water. For example:
HCl (Acid) + NaOH (Base) → NaCl (Salt) + H2O (Water)
Neutralization is used in treating indigestion (antacids), in cleaning agents, soil treatment, and many industrial processes.
Step-by-Step Reaction Example
1. Write the balanced equation for neutralization.HCl + NaOH → NaCl + H2O
2. Identify the acid and base.
HCl is the acid; NaOH is the base.
3. State the products formed.
Salt (NaCl) and water are produced.
4. Note the reaction conditions.
Happens at room temperature in aqueous solution.
Common Misconceptions or Errors
- Confusing acids and bases based only on taste—never taste chemicals in the lab.
- Assuming all acids and bases are dangerous—many in food are safe in low amounts.
- Mixing up pH values (remember: acids <7, bases >7, neutral = 7).
- Thinking all bases are alkalis—only water-soluble bases are alkalis.
Uses of Difference Between Acid and Base in Real Life
Understanding the difference between acid and base helps in day-to-day activities. Toothpaste neutralizes acids in the mouth, antacids relieve acidity, and cleaning agents often contain bases to remove grease. Farmers use lime (a base) to reduce soil acidity. Food preservatives and flavors involve different acids and bases.
Lab Tip or Classroom Mnemonic
Remember: "Acid turns Blue litmus Red – (A B R – Acid Blue Red)" and "Base turns Red litmus Blue – (B R B – Base Red Blue)". Many Vedantu educators teach this as a classroom hack for quick recall.
Try This Yourself
- List 3 examples of acids and 3 examples of bases from your kitchen.
- Write a balanced equation for neutralization using HNO3 and KOH.
- Test pH of lemon juice and soap solution using a pH strip and record findings.
We explored the difference between acid and base—from fundamental properties and theories, to real-life uses and exam-ready tables. For more in-depth explanations, live classes, and revision notes, check out more resources and study help on Vedantu's chemistry pages.
Related study links:
- Properties of Acids and Bases
- pH of Acids and Bases
- Acid-Base Titration
- Neutralization Reaction
- Examples of Bases
FAQs on Difference Between Acids and Bases: Explained with Examples
1. What is the definition of an acid and a base?
According to the Arrhenius concept, an acid is a substance that increases the concentration of hydrogen ions (H+) in an aqueous solution, while a base increases the concentration of hydroxide ions (OH-). For example, HCl is an acid and NaOH is a base. However, the Brønsted-Lowry theory offers a broader definition: an acid is a proton (H+) donor, and a base is a proton acceptor. The Lewis theory defines acids as electron pair acceptors and bases as electron pair donors.
2. Write any 4 properties that show the difference between acid and base?
Acids typically taste sour, react with metals to produce hydrogen gas (H2), turn blue litmus paper red, and have a pH less than 7. Bases, conversely, taste bitter, feel slippery, turn red litmus paper blue, and have a pH greater than 7. They react with acids to form salts and water in a neutralization reaction.
3. What is the main difference between acid and base?
The fundamental difference lies in their behavior in aqueous solutions: acids release hydrogen ions (H+), while bases release hydroxide ions (OH-) or accept protons (H+). This difference is reflected in their contrasting properties and their effects on indicators, and their pH values (acids have pH < 7, bases have pH > 7).
4. Explain the pH difference between acid and base?
The pH scale measures the acidity or basicity of a solution. A pH of 7 is neutral. Acids have a pH value less than 7, with lower values indicating stronger acidity. Bases have a pH value greater than 7, with higher values indicating stronger basicity. The difference in pH reflects the difference in hydrogen ion (H+) concentration: acids have higher H+ concentration, while bases have lower H+ concentration (or higher OH- concentration).
5. Is water an acid or a base?
Water is amphoteric, meaning it can act as both an acid and a base depending on the reaction. It can donate a proton (H+) to a stronger base (acting as an acid) or accept a proton (H+) from a stronger acid (acting as a base). This is described by the Brønsted-Lowry theory.
6. What are some common examples of acids and bases in everyday life?
Acids are found in many foods like lemons (citric acid), vinegar (acetic acid), and sour milk (lactic acid). Bases include things like soap, baking soda (sodium bicarbonate), and antacids (often containing magnesium hydroxide or calcium hydroxide).
7. What is a neutralization reaction?
A neutralization reaction occurs when an acid reacts with a base. The hydrogen ions (H+) from the acid react with the hydroxide ions (OH-) from the base to form water (H2O) and a salt. The resulting solution is typically closer to neutral (pH 7).
8. How do indicators distinguish acids and bases?
Indicators are substances that change color depending on the pH of a solution. Litmus paper is a common example: it turns red in acids and blue in bases. Other indicators, such as phenolphthalein and methyl orange, exhibit different color changes over specific pH ranges. These changes are caused by the interaction of the indicator molecules with the different concentrations of hydrogen ions (H+) and hydroxide ions (OH-) present.
9. What are strong acids and weak acids?
Strong acids completely dissociate into ions when dissolved in water, while weak acids only partially dissociate. This difference affects their acidity and their reactivity. Examples of strong acids include hydrochloric acid (HCl) and sulfuric acid (H2SO4). Examples of weak acids include acetic acid (CH3COOH) and carbonic acid (H2CO3).
10. What are strong bases and weak bases?
Similar to acids, strong bases completely dissociate into ions in water, while weak bases only partially dissociate. This impacts their basicity and their reactivity. Examples of strong bases include sodium hydroxide (NaOH) and potassium hydroxide (KOH). Examples of weak bases include ammonia (NH3).
11. What is the difference between an alkali and a base?
All alkalis are bases, but not all bases are alkalis. An alkali is a water-soluble base that produces hydroxide ions (OH-) in solution. Bases can be soluble or insoluble in water.
12. Why is understanding acids and bases important?
Understanding acids and bases is crucial because they are involved in countless chemical reactions, both in nature and in industrial processes. They play vital roles in various applications, from digestion in our bodies to manufacturing processes. Knowledge of acid-base chemistry is essential in many scientific fields, including medicine, agriculture, and environmental science.
