Key Differences Between Strong and Weak Acids and Bases

1. Dissolving in Water:

   • Strong Acids: These acids break apart completely when mixed with water. This creates a lot of hydronium ions ($\text{H}_3\text{O}^+$). Some examples are hydrochloric acid (HCl) and sulfuric acid (H$_2$SO$_4$).

   • Weak Acids: These acids only break apart a little bit in water, creating fewer hydronium ions. A common example is acetic acid (CH$_3$COOH), which only breaks apart about 1% in a strong solution.

2. pH Values:

   • Strong Acids: These usually have pH values between 0 and 1 when they are in high amounts. For example, a solution of 0.1M HCl has a pH of about 1.

   • Weak Acids: These acids have pH values greater than 1. For instance, a 0.1M acetic acid solution has a pH around 2.9.

3. Strength of Bases:

   • Strong Bases: These bases break apart completely in water to produce hydroxide ions ($\text{OH}^-$). Sodium hydroxide (NaOH) is a good example and has pH values around 14 in strong solutions.

   • Weak Bases: These only partially break apart. Ammonia (NH$_3$) is an example and has a much lower pH compared to strong bases.

4. Neutralization:

   • When an acid and a base react together, they can neutralize each other, forming water and a salt. The strength of the acid or base can change how much they react with each other.