Question

Sodium hydroxide, \(\mathrm{NaOH}\), is a strong base, which means it readily accepts hydrogen ions. What products are formed when sodium hydroxide accepts a hydrogen ion from a water molecule?

Short answer

NaOH forms water and sodium ions when it reacts with a hydrogen ion from water.

Step-by-step solution

Understanding the Reaction

When sodium hydroxide (\(\mathrm{NaOH}\)) dissolves in water, it dissociates into sodium ions (\(\mathrm{Na^+}\)) and hydroxide ions (\(\mathrm{OH^-}\)). It is a strong base and can accept hydrogen ions from water molecules.

Writing the Ion Formation

In water, the \(\mathrm{NaOH}\) dissociates as follows: \[ \mathrm{NaOH \rightarrow Na^+ + OH^-} \] This equation shows that \(\mathrm{Na^+}\) and \(\mathrm{OH^-}\) ions are formed in solution.

Reaction with Water

The hydroxide ion (\(\mathrm{OH^-}\)) reacts with a hydrogen ion (\(\mathrm{H^+}\)) from a water molecule (\(\mathrm{H_2O}\)) to form water: \[ \mathrm{OH^- + H^+ \rightarrow H_2O} \].

Final Products

The overall reaction when \(\mathrm{OH^-}\) accepts a \(\mathrm{H^+}\) ion involves forming water from the \(\mathrm{OH^-}\) and \(\mathrm{H^+}\). The sodium ion (\(\mathrm{Na^+}\)) remains in solution as a spectator ion.

Key concepts

Sodium Hydroxide

Sodium hydroxide, commonly referred to as lye or caustic soda, is essential in many chemical processes. It is a strong base, meaning it efficiently accepts hydrogen ions in reaction.
When sodium hydroxide is introduced to water, it dissociates entirely into sodium ions (\(\mathrm{Na^+}\)) and hydroxide ions (\(\mathrm{OH^-}\)). This property of sodium hydroxide makes it a key player in various reactions where strong bases are required.

• Useful in neutralizing acids in chemical processes.
• Found in household cleaning agents due to its strong base characteristics.

Understanding sodium hydroxide's role as a strong base gives insight into its extensive applications both in industrial settings and everyday life.

Hydroxide Ions

Hydroxide ions (\(\mathrm{OH^-}\)) are crucial in the discussion of acid-base chemistry. These ions emerge from the dissociation of bases like sodium hydroxide in water.
Hydroxide ions are responsible for the basicity of solutions because they readily accept hydrogen ions (\(\mathrm{H^+}\)).

• They increase the pH of the solution, making it more basic or alkaline.
• React with acids to form water, driving crucial neutralization reactions.

In a reaction, such as with water molecules, hydroxide ions grab a hydrogen ion to construct a water molecule. This acceptance-stability relationship underscores many fundamental chemistry principles.

Water Molecule

Water molecules are more than just the everyday liquid we drink; they play a dynamic role in chemistry. Comprised of two hydrogen atoms and one oxygen atom (\(\mathrm{H_2O}\)), these molecules can dissociate into hydrogen ions (\(\mathrm{H^+}\)) and hydroxide ions (\(\mathrm{OH^-}\)) under certain conditions.
Water serves as a reactant and a product in numerous chemical reactions, including those involving acid-base equilibria.

• Acts as both an acid and a base, showing amphoteric behavior.
• Participates in neutralization reactions by donating a hydrogen ion.

Its ability to provide hydrogen ions and participate in forming a steady product like a water molecule is vital for sustaining chemical processes.

Hydrogen Ions

Hydrogen ions (\(\mathrm{H^+}\)) are central players in acid-base interactions. These ions are essentially protons and carry a positive charge.
When a substance like sodium hydroxide accepts hydrogen ions, it illustrates typical acid-base reactions. The ease with which hydrogen ions can be transferred between reactants and products is key to many biochemical and industrial processes.

• Determine the acidity level of a solution.
• Combine with hydroxide ions to form water; central in neutralization reactions.

Their capacity for transfer between entities contributes to the mechanisms of maintaining balance in solutions, making them indispensable in understanding chemical reactions.