Chapter 4: Q4.53P (page 180)

An auto mechanic spills 88 mL of 2.6 M H₂SO₄ solution from a rebuilt auto battery. How many milliliters of 1.6 M NaHCO₃ must be poured on the spill to react completely with the sulfuric acid?

Short Answer

Expert verified

286 ml of1.6 M NaHCO₃ must be poured on the spill to react completely with the sulfuric acid.

Step by step solution

Step 1:first write down the balanced molecular equation:

$2 N a H C O_{3} (a q) + H_{2} S O_{4} (a q) \to N a_{2} S O_{4} (a q) + 2 H_{2} C O_{3} (a q)$

To find out the volume of NaHCO3 poured to react completely with the sulfuric acid, first, we have to calculate the moles of NaHCO3:

Given values are:

$v o l u m e o f s t a n d a r d 2.6 M H_{2} S O_{4} s o l u t i o n = 88 m l v o l u m e o f N a H C O_{3} = 1.6 M$

Moles of NaHCO₃is:

$\begin{array}{rcl} m o l e s o f N a H C O_{3} & = & (88 m l H_{2} S O_{4}) (\frac{1 l i t}{1000 m l}) (\frac{2.6 m o l H_{2} S O_{4}}{1 l i t H_{2} S O_{4} s o l u t i o n}) (\frac{2 m o l N a H C O_{3}}{1 m o l H_{2} S O_{4}}) \\ = & 0.4576 m o l N a H C O_{3} \end{array}$

The volume of NaHCO₃ poured to react completely with the sulfuric acid:

$v o l u m e o f N a H C O_{3} = \frac{m o l e s o f N a H C O_{3}}{m o l a r i t y o f N a H C O_{3}}$

$= \frac{0.4576 m o l N a H C O_{3}}{(\frac{1.6 m o l N a H C O_{3}}{1 l i t N a H C O_{3}})}$

$= 0.286 l i t N a H C O_{3} = 286 m l N a H C O_{3}$

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An auto mechanic spills 88 mL of 2.6 M H₂SO₄ solution from a rebuilt auto battery. How many milliliters of 1.6 M NaHCO₃ must be poured on the spill to react completely with the sulfuric acid?

Short Answer

Step by step solution

Step 1:first write down the balanced molecular equation:

To find out the volume of NaHCO3 poured to react completely with the sulfuric acid, first, we have to calculate the moles of NaHCO3:

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An auto mechanic spills 88 mL of 2.6 M H2SO4 solution from a rebuilt auto battery. How many milliliters of 1.6 M NaHCO3 must be poured on the spill to react completely with the sulfuric acid?

Short Answer

Step by step solution

Step 1:first write down the balanced molecular equation:

To find out the volume of NaHCO3 poured to react completely with the sulfuric acid, first, we have to calculate the moles of NaHCO3:

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Chemical Analysis

Chemistry Branches

Kinetics

Inorganic Chemistry

Ionic and Molecular Compounds

Study anywhere. Anytime. Across all devices.

An auto mechanic spills 88 mL of 2.6 M H₂SO₄ solution from a rebuilt auto battery. How many milliliters of 1.6 M NaHCO₃ must be poured on the spill to react completely with the sulfuric acid?