Question

Which acid and base react to give an aqueous solution of \(\mathrm{K}_{2} \mathrm{SO}_{4} ?\) Write a balanced equation for this neutralization reaction.

Short answer

The acid H₂SO₄ (sulfuric acid) and the base KOH (potassium hydroxide) react to give an aqueous solution of K₂SO₄ (potassium sulfate). The balanced equation for the neutralization reaction is given by: \[ H_{2}SO_{4} \: (aq) + 2 \: KOH \: (aq) \rightarrow K_{2}SO_{4} \: (aq) + 2 \: H_{2}O \: (l) \]

Step-by-step solution

Identify the cation and anion in K₂SO₄

In the compound K₂SO₄, we have two ions: the cation K⁺(potassium ion) and the anion SO₄²⁻ (sulfate ion).

Find an acid containing the anion and a base containing the cation

To find an acid containing the sulfate anion (SO₄²⁻) and a base containing the potassium cation (K⁺), we can consider the following: Acid: H₂SO₄ (sulfuric acid) contains the sulfate anion (SO₄²⁻) Base: KOH (potassium hydroxide) contains the potassium cation (K⁺)

Write the balanced equation for the neutralization reaction

Now, we can write the balanced equation for the neutralization reaction between H₂SO₄ and KOH: H₂SO₄ (aq) + 2 KOH (aq) → K₂SO₄ (aq) + 2 H₂O (l) In this reaction, the sulfuric acid (H₂SO₄) neutralizes potassium hydroxide (KOH), forming potassium sulfate (K₂SO₄) and water (H₂O). The equation is balanced since there are an equal number of atoms of each element on both sides of the equation.

Key concepts

Sulfuric Acid

Sulfuric acid, scientifically represented as \( \text{H}_2\text{SO}_4 \), is a dense, oily liquid that is colorless to slightly yellow. It is one of the most important acids used in industry and chemistry.
Sulfuric acid is highly corrosive and can cause burns, so it must be handled with care. It has a strong affinity for water, which means it is excellent for dehydrating processes where water needs to be removed.

• It is a diprotic acid, which means it can donate two hydrogen ions (\( \text{H}^+ \)) in reactions.
• In the neutralization reaction, it donates these hydrogen ions to react with bases like potassium hydroxide (KOH).

Understanding sulfuric acid's properties and behavior is crucial in predicting how it will react in chemical reactions, such as neutralization, where it combines with bases to form salt and water.

Potassium Hydroxide

Potassium hydroxide, denoted as \( \text{KOH} \), is a strong base used in various chemical reactions and industrial applications. It usually appears as a white solid and is highly soluble in water.
When dissolved, it dissociates to form potassium ions (\( \text{K}^+ \)) and hydroxide ions (\( \text{OH}^- \)). This dissociation is key to its reactivity with acids.

• Potassium hydroxide can neutralize acids by providing hydroxide ions to react with hydrogen ions, producing water.
• It is commonly used in soap production, as a pH regulator, and in the synthesis of other potassium compounds.

In a neutralization reaction with sulfuric acid, potassium hydroxide contributes potassium ions that combine with sulfate ions, forming the salt potassium sulfate (\( \text{K}_2\text{SO}_4 \)). This is an essential part of understanding how such reactions occur.

Balanced Chemical Equation

A balanced chemical equation is fundamental in chemistry as it depicts the reactants and products of a reaction accurately, while maintaining the law of conservation of mass. This means that the number of each type of atom must be the same on both sides of the equation.
For the neutralization reaction between sulfuric acid (\( \text{H}_2\text{SO}_4 \)) and potassium hydroxide (\( \text{KOH} \)), the balanced chemical equation is: \[ \text{H}_2\text{SO}_4 (aq) + 2 \text{KOH} (aq) \rightarrow \text{K}_2\text{SO}_4 (aq) + 2 \text{H}_2\text{O} (l) \]

• This equation reveals that two molecules of potassium hydroxide react with one molecule of sulfuric acid.
• The resulting products are one molecule of potassium sulfate and two molecules of water.

Achieving a balanced equation ensures that calculations related to the reaction, such as reactant quantities and product yield, are accurate. Understanding the balance in a reaction is pivotal to mastering chemical equations in any chemical process.