$H _2 SO _4( aq )$ and $KOH ( aq )$
$\\\xrightarrow[\\text { Molecular Equation }]{H_2 SO_4(aq)+KOH(aq) \\rightarrow}$
Complete Ionic Equation
Net Ionic Equation
Spectator Ions
Answer (1)
H + ( a q ) + O H − ( a q ) → H 2 O ( l ) . Spectator ions: K + ( a q ) and S O 4 2 − ( a q ) .
Explanation
Problem Analysis We are given the reactants sulfuric acid ( H 2 S O 4 ) in aqueous solution and potassium hydroxide ( K O H ) in aqueous solution. Our goal is to determine the molecular equation, complete ionic equation, net ionic equation, and spectator ions for the reaction.
Molecular Equation - Unbalanced First, we write the balanced molecular equation for the reaction between H 2 S O 4 ( a q ) and K O H ( a q ) . This is an acid-base neutralization reaction, which produces a salt and water:
H 2 S O 4 ( a q ) + K O H ( a q ) → K 2 S O 4 ( a q ) + H 2 O ( l )
Molecular Equation - Balanced Next, we balance the molecular equation:
H 2 S O 4 ( a q ) + 2 K O H ( a q ) → K 2 S O 4 ( a q ) + 2 H 2 O ( l )
Complete Ionic Equation Now, we write the complete ionic equation by dissociating all aqueous strong electrolytes into their respective ions. Strong electrolytes include strong acids, strong bases, and soluble salts. H 2 S O 4 ( a q ) is a strong acid, K O H ( a q ) is a strong base, and K 2 S O 4 ( a q ) is a soluble salt. Thus, we have:
2 H + ( a q ) + S O 4 2 − ( a q ) + 2 K + ( a q ) + 2 O H − ( a q ) → 2 K + ( a q ) + S O 4 2 − ( a q ) + 2 H 2 O ( l )
Identifying Spectator Ions We identify the spectator ions, which are the ions that appear on both sides of the complete ionic equation. In this case, K + ( a q ) and S O 4 2 − ( a q ) are spectator ions.
Net Ionic Equation - Unsimplified We write the net ionic equation by removing the spectator ions from the complete ionic equation:
2 H + ( a q ) + 2 O H − ( a q ) → 2 H 2 O ( l )
Net Ionic Equation - Simplified Finally, we simplify the net ionic equation by dividing all coefficients by their greatest common divisor:
H + ( a q ) + O H − ( a q ) → H 2 O ( l )
Spectator Ions The spectator ions are K + ( a q ) and S O 4 2 − ( a q ) .
Examples
Acid-base neutralization reactions are fundamental in chemistry and have numerous real-world applications. For instance, they are crucial in titrations, where the concentration of an acid or base is determined. In environmental science, these reactions are used to neutralize acidic pollutants in water or soil. Moreover, our bodies use neutralization reactions to maintain pH balance, such as when antacids neutralize excess stomach acid. Understanding these reactions helps us manage chemical processes and maintain equilibrium in various systems.
