6 Questions
What are acids and bases?
Acids are substances that release hydrogen ions when dissolved in water, while bases are substances that release hydroxide ions when dissolved in water.
How do acids and bases differ in terms of their pH?
Acids have a pH less than 7, while bases have a pH greater than 7.
What are some common examples of acids and bases?
Common examples of acids include hydrochloric acid (HCl) and sulfuric acid (H2SO4), while common examples of bases include sodium hydroxide (NaOH) and ammonia (NH3).
What is the Arrhenius definition of acids and bases?
According to the Arrhenius definition, acids are substances that release hydrogen ions (H+) in water, while bases are substances that release hydroxide ions (OH-) in water.
What is the difference between a strong acid and a weak acid?
A strong acid completely ionizes in water, producing a high concentration of hydrogen ions (H+), while a weak acid only partially ionizes, producing a lower concentration of hydrogen ions.
How does the Bronsted-Lowry theory define acids and bases?
According to the Bronsted-Lowry theory, acids are substances that donate protons (H+), while bases are substances that accept protons.
Study Notes
Acids and Bases
- Acids are substances that donate a proton (H+ ion), while bases are substances that accept a proton.
- Acids and bases differ in terms of their pH, with acids having a pH below 7 and bases having a pH above 7.
pH and Acid-Base Classification
- A pH of 7 is neutral, while a pH below 7 is acidic and a pH above 7 is basic.
Examples of Acids and Bases
- Common acids: hydrochloric acid (HCl), sulfuric acid (H2SO4), nitric acid (HNO3), and citric acid (C6H8O7).
- Common bases: sodium hydroxide (NaOH), calcium hydroxide (Ca(OH)2), and ammonia (NH3).
Arrhenius Definition
- The Arrhenius definition states that acids are substances that increase the concentration of H+ ions in a solution, while bases are substances that increase the concentration of OH- ions in a solution.
Strong and Weak Acids
- A strong acid is completely ionized in a solution, releasing all its H+ ions, whereas a weak acid is only partially ionized, releasing only some of its H+ ions.
- Examples of strong acids: hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3).
- Examples of weak acids: citric acid (C6H8O7), acetic acid (CH3COOH), and carbonic acid (H2CO3).
Bronsted-Lowry Theory
- The Bronsted-Lowry theory defines acids as proton (H+ ion) donors and bases as proton acceptors.
- This theory expands the definition of acids and bases to include conjugate acid-base pairs, which are formed when an acid donates a proton and a base accepts it.
Test your knowledge on acids and bases with this quiz! Learn about the definitions of acids and bases, understand the differences in pH levels, and discover some common examples of these substances. Perfect for students studying Chemistry in the Federal Board class 10 curriculum.
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