A Chemist Uses 0.25 L Of $200 \, M \, H_2SO_4$ To Completely Neutralize 2.00 L Of A Solution Of NaOH. The Balanced Chemical Equation Of The Reaction Is Given Below:$\[2 \, \text{NaOH} + \text{H}_2\text{SO}_4 \rightarrow

A Chemist's Dilemma: Balancing the Neutralization Reaction of H2SO4 and NaOH

In the world of chemistry, balancing chemical equations is a crucial skill that every chemist must possess. It not only helps in understanding the stoichiometry of a reaction but also in predicting the amount of reactants and products involved. In this article, we will delve into the world of acid-base chemistry and explore the neutralization reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH). We will use the given information to balance the chemical equation and determine the limiting reactant.

The balanced chemical equation for the neutralization reaction between H2SO4 and NaOH is given as:

${2 \, \text{NaOH} + \text{H}_2\text{SO}_4 \rightarrow \text{Na}_2\text{SO}_4 + 2 \, \text{H}_2\text{O}}$

This equation shows that 2 moles of NaOH react with 1 mole of H2SO4 to produce 1 mole of Na2SO4 and 2 moles of H2O.

We are given that a chemist uses 0.25 L of 200 M H2SO4 to completely neutralize 2.00 L of a solution of NaOH. We need to use this information to determine the limiting reactant and the amount of products formed.

Calculating the Number of Moles of H2SO4

To calculate the number of moles of H2SO4, we can use the formula:

${ \text{Number of moles} = \text{Molarity} \times \text{Volume (in liters)} }$

Substituting the given values, we get:

${ \text{Number of moles of H}_2\text{SO}_4 = 200 \, \text{M} \times 0.25 \, \text{L} = 50 \, \text{moles} }$

Calculating the Number of Moles of NaOH

To calculate the number of moles of NaOH, we need to know the molarity of the NaOH solution. However, the molarity of the NaOH solution is not given. We can use the given information to calculate the number of moles of NaOH.

Since 2 moles of NaOH react with 1 mole of H2SO4, the number of moles of NaOH required to neutralize 50 moles of H2SO4 is:

${ \text{Number of moles of NaOH} = 2 \times 50 \, \text{moles} = 100 \, \text{moles} }$

Calculating the Molarity of the NaOH Solution

Now that we know the number of moles of NaOH required to neutralize 50 moles of H2SO4, we can calculate the molarity of the NaOH solution.

The volume of the NaOH solution is given as 2.00 L. We can use the formula:

${ \text{Molarity} = \frac{\text{Number of moles}}{\text{Volume (in liters)}} }$

Substituting the values, we get:

${ \text{Molarity of NaOH} = \frac{100 \, \text{moles}}{2.00 \, \text{L}} = 50 \, \text{M} }$

Determining the Limiting Reactant

Now that we have calculated the number of moles of H2SO4 and NaOH, we can determine the limiting reactant.

Since 50 moles of H2SO4 are required to neutralize 100 moles of NaOH, and we have 50 moles of H2SO4, the H2SO4 is the limiting reactant.

Calculating the Amount of Products Formed

Since H2SO4 is the limiting reactant, we can calculate the amount of products formed using the balanced chemical equation.

The balanced chemical equation shows that 1 mole of H2SO4 produces 1 mole of Na2SO4 and 2 moles of H2O.

Therefore, the amount of Na2SO4 formed is:

${ \text{Amount of Na}_2\text{SO}_4 = 50 \, \text{moles} }$

And the amount of H2O formed is:

${ \text{Amount of H}_2\text{O} = 2 \times 50 \, \text{moles} = 100 \, \text{moles} }$

In this article, we used the given information to balance the chemical equation for the neutralization reaction between H2SO4 and NaOH. We calculated the number of moles of H2SO4 and NaOH required to neutralize each other and determined the limiting reactant. We also calculated the amount of products formed using the balanced chemical equation. This example demonstrates the importance of balancing chemical equations in understanding the stoichiometry of a reaction and predicting the amount of reactants and products involved.

• Chemical Equations and Stoichiometry by OpenStax College
• Acid-Base Chemistry by Chemistry LibreTexts

• Balancing Chemical Equations by Chemistry LibreTexts
• Stoichiometry by OpenStax College
  A Chemist's Dilemma: Balancing the Neutralization Reaction of H2SO4 and NaOH - Q&A

In our previous article, we explored the neutralization reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH). We balanced the chemical equation, calculated the number of moles of H2SO4 and NaOH required to neutralize each other, and determined the limiting reactant. In this article, we will answer some frequently asked questions related to the neutralization reaction between H2SO4 and NaOH.

Q: What is the balanced chemical equation for the neutralization reaction between H2SO4 and NaOH?

A: The balanced chemical equation for the neutralization reaction between H2SO4 and NaOH is:

${2 \, \text{NaOH} + \text{H}_2\text{SO}_4 \rightarrow \text{Na}_2\text{SO}_4 + 2 \, \text{H}_2\text{O}}$

Q: What is the molarity of the H2SO4 solution?

A: The molarity of the H2SO4 solution is given as 200 M.

Q: What is the volume of the H2SO4 solution?

A: The volume of the H2SO4 solution is given as 0.25 L.

Q: What is the volume of the NaOH solution?

A: The volume of the NaOH solution is given as 2.00 L.

Q: What is the molarity of the NaOH solution?

A: The molarity of the NaOH solution is calculated to be 50 M.

Q: Which reactant is the limiting reactant?

A: H2SO4 is the limiting reactant.

Q: How many moles of Na2SO4 are formed?

A: 50 moles of Na2SO4 are formed.

Q: How many moles of H2O are formed?

A: 100 moles of H2O are formed.

Q: What is the purpose of balancing chemical equations?

A: Balancing chemical equations is essential to understand the stoichiometry of a reaction and predict the amount of reactants and products involved.

Q: How can I determine the limiting reactant in a reaction?

A: To determine the limiting reactant, you need to calculate the number of moles of each reactant required to complete the reaction. The reactant with the smaller number of moles is the limiting reactant.

Q: What is the importance of understanding acid-base chemistry?

A: Understanding acid-base chemistry is crucial in various fields such as chemistry, biology, and medicine. It helps in predicting the behavior of acids and bases, which is essential in understanding various chemical reactions.

In this article, we answered some frequently asked questions related to the neutralization reaction between H2SO4 and NaOH. We hope that this article has provided you with a better understanding of the neutralization reaction and its importance in chemistry.

• Chemical Equations and Stoichiometry by OpenStax College
• Acid-Base Chemistry by Chemistry LibreTexts

• Balancing Chemical Equations by Chemistry LibreTexts
• Stoichiometry by OpenStax College