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Chapter 15: Problem 201

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

Expert verified
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

01

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).
02

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⁺)
03

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.

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Most popular questions from this chapter

Based solely on concentrations, when is an aqueous solution judged to be acidic? Give two answers to this question.

When ammonia gas is dissolved in water, is the water behaving as an acid, as a base, or neither? Explain.

If \(0.378 \mathrm{~g}\) of HBr dissolved in enough water to make \(1.25 \mathrm{~L}\) of solution, what is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? What is the \(\mathrm{OH}^{-}\) concentration?

Does a mixture of carbonic acid, \(\mathrm{H}_{2} \mathrm{CO}_{3}\), a weak acid, and sodium bicarbonate, \(\mathrm{NaHCO}_{3}\), in water constitute a buffer? If no, explain why. If yes, explain why and use chemical equations to show what happens when either \(\mathrm{OH}\) or \(\mathrm{H}_{3} \mathrm{O}^{+}\) is added to the solution.

What is the \(\mathrm{OH}^{-}\) concentration of a solution that has a pH of \(9.66\) ? Is this solution acidic or basic?
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