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Chapter 15: Problem 7

What salt forms when sulfuric acid completely neutralizes sodium hydroxide? Give both name and formula for the salt.

Short Answer

Expert verified
The salt formed when sulfuric acid completely neutralizes sodium hydroxide is sodium sulfate (Na₂SO₄).

Step by step solution

01

Write the balanced chemical equation for the neutralization reaction.

The balanced chemical equation for the neutralization reaction between sulfuric acid and sodium hydroxide can be written as: \[ H_2SO_4 + 2 NaOH \rightarrow Na_2SO_4 + 2 H_2O \] In this equation, sulfuric acid (H₂SO₄) reacts with sodium hydroxide (NaOH) to form the salt sodium sulfate (Na₂SO₄) and water (H₂O).
02

Identify the salt in the balanced chemical equation.

In the balanced chemical equation, we can see that the salt formed is Na₂SO₄, which is composed of two sodium ions (Na⁺) and one sulfate ion (SO₄²⁻). Take note that the two sodium ions balance the charge of the sulfate ion, making the compound neutrally charged.
03

Name the salt.

The name for the salt is composed of the cation (positive ion) and the anion (negative ion). In this case, the cation is sodium (Na⁺) and the anion sulfate (SO₄²⁻). Therefore, the name of the salt is sodium sulfate.
04

Write the final answer.

The salt formed when sulfuric acid completely neutralizes sodium hydroxide is sodium sulfate (Na₂SO₄).

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Most popular questions from this chapter

Solid ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl}\), reacts with solid sodium hydroxide to produce ammonia gas, water, and sodium chloride, \(\mathrm{NaCl}\). (a) Write a balanced equation for this reaction. (b) According to the Bronsted-Lowry definition, which species is the acid and which species is the base? Explain.

Does pure liquid water have any buffering ability? Explain.

Without using a calculator, what is the base- 10 logarithm of \(10^{0}\) ? Of 1?

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.

To be a weak base in water, a molecular compound must also be a weak electrolyte. What must be one of the ions it produces in water?
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