Bases

• Bases are substances that accept protons (H+) or donate electrons.

• Bases increase the concentration of hydroxide ions (OH-) in water.

Properties of Bases:

• Bitter taste

• Slippery feel

• React with acids to neutralize them

• Turn red litmus paper blue

• Conduct electricity in aqueous solutions

More About Bases:

• Many bases are ionic compounds containing a metal cation and hydroxide anion (OH-).

• Bases can be organic or inorganic.

Solubility in Water of Bases:

• Group 1 hydroxides (e.g., NaOH, KOH) are generally soluble in water.

• Group 2 hydroxides (e.g., Ca(OH)2, Mg(OH)2) are sparingly soluble in water.

• Insoluble bases can still react with acids in neutralization reactions.

Strong and Weak Bases:

• Strong Bases: Dissociate completely in water to produce a high concentration of hydroxide ions (OH-).

  • Examples: NaOH, KOH, Ca(OH)_2. These are typically Group 1 and some Group 2 hydroxides.

• Weak Bases: Do not fully dissociate in water, resulting in a lower concentration of hydroxide ions (OH-).

  • Examples: NH$_3$ (ammonia), amines (organic bases).

• The strength of a base depends on its ability to accept protons or donate electrons.

Uses of Bases:

• Neutralization of Acids:

  • Antacids (e.g., Mg(OH)2, Al(OH)3) neutralize excess stomach acid.

• Cleaning Agents:

  • Soaps and