Chapter 4.3: Acid-Base Reactions

Flashcards from Chapter 4.3 of Chemistry: The Molecular Nature of Matter and Change.

Hydronium

The name for the the H₃O⁺ ion formed between an H⁺ ion and a water molecule

Gaseous reactions

Reactions that form a gas and sometimes a water

• Includes reactions with carbonates, sulfites, and bisulfates for an equation resembling CO₂

• Includes reactions with sulfides for H₂S

• Includes reactions with ammonium for NH₃

1. Note the color changes of the indicator in acids and bases

2. Measure out a known volume of acid (or base) with indicator

3. Add drops of base (or acid) to replace H⁺ (or OH^-), observing a temporary change in color that goes away when swirled

4. Stop when the endpoint is reached, where a color is effected even after swirling

How would I perform a titration?

Acid

A substance that increases the concentration of H⁺ when dissolved in water

Base

A substance that increases the concentration of OH^- when dissolved in water

• Can either dissociate to form OH^- (when strong) or remove an H⁺ ion from water (if weak)

Acid-base reaction

A reaction between an acid and a base with water acting as a solvent, product, or reactant

Strong acid

An acid with a strong tendency to dissociate into ions in water, allowing for high electrolytic capacity

• Includes hydrogen and N-ate, S-ate, Cl-+ate, Br, and I, which are soluble

Weak acid

An acid with a low tendency to dissociate into ions in water, creating low electrolytic capcity

• Written as undissociated compound decomposing into ions in ionic equations

Strong base

A base with a strong tendency to dissociate in to OH^- and another substance in water

• Includes OH^- and group 1 and 2 metals, of which ones are soluble

Weak base

A base that does not readily dissociate in water and instead forms OH^- through the attraction of an H⁺ ion from water

• Typically includes nitrogen, like in NH₃⁺ (ammonia)

Electrolytic capacity

This is increased when a salt, strong acid, or strong base dissociates into water

• Allows for the use of molarity as a conversion factor

Metathesis reactions (double-displacement reactions)

Reactions where cation and anion partners switch

Molecular equation

An equation where all compounds are shown as undissociated substances

Total ionic equation

An equation where all compounds are shown as they exist in solution, potentially as ions for a salt, strong base, or weak base

Net ionic equation

An equation where only changed ionic compounds are shown in solution

• Does not include spectator ions

Spectator ions

Ions that do not participate in a reaction and are left out in the net ionic equation

Equivalence point

When the moles of OH^- equal the moles of H⁺ in a solution for complete neutralization

End point

When the moles of either H⁺ or OH^- in a solution are slightly greater than the other, effecting a change in an indicator that does not disappear when swirling

• Sometimes treated as equivalent to the equivalence point due to only slight difference