A flask containing 450 mL of 0.50 M H2 SO4 was accidentally knocked to the floor. How many gram

Name: Problem 59, Chapter 9: Fundamentals of General, Organic, and Biological Chemistry
Uploaded: 2022-01-12T20:17:16-08:00
Duration: 2 min 18 s
Channel: John Nicolle
Description: A flask containing 450 mL of 0.50 M H2 SO4 was accidentally knocked to the floor. How many grams of NaHCO3 do you need to put on the spill to neutralize the acid according to the following equation? H2 SO4(a q)+2 NaHCO3(a q) ⟶ Na2 SO4(a q)+2 H2 O(l)+2 CO2(g)

step 1 Hi so in this question the given molarity of H2 S -o4 is 0 .50 mole volume is 0 .450 liter moles

Question

A flask containing $450 \mathrm{~mL}$ of $0.50 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ was accidentally knocked to the floor. How many grams of $\mathrm{NaHCO}_{3}$ do you need to put on the spill to neutralize the acid according to the following equation? $$ \begin{aligned} \mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaHCO}_{3}(a q) & \longrightarrow \\ \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g) \end{aligned} $$

   A flask containing $450 \mathrm{~mL}$ of $0.50 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ was accidentally knocked to the floor. How many grams of $\mathrm{NaHCO}_{3}$ do you need to put on the spill to neutralize the acid according to the following equation?
$$
\begin{aligned}
\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaHCO}_{3}(a q) & \longrightarrow \\
\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)
\end{aligned}
$$

Fundamentals of General, Organic, and Biological Chemistry

John McMurry, David… 1st Edition

Chapter 9, Problem 59

Instant Answer

Solved by Expert John Nicolle

01/12/2022

Step 1

We can do this using the formula for molarity, which is moles of solute divided by volume of solution in liters. In this case, the molarity of $\mathrm{H}_{2} \mathrm{SO}_{4}$ is 0.50 M and the volume of the solution is 450 mL or 0.450 L. So, the number of moles Show more…

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A flask containing $450 \mathrm{~mL}$ of $0.50 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ was accidentally knocked to the floor. How many grams of $\mathrm{NaHCO}_{3}$ do you need to put on the spill to neutralize the acid according to the following equation? $$ \begin{aligned} \mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NaHCO}_{3}(a q) & \longrightarrow \\ \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g) \end{aligned} $$

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Key Concepts

Molarity and Volume

Molarity is a measure of concentration representing the number of moles of solute per liter of solution. When combined with the volume of the solution, this allows one to determine the total moles of a substance present, which is critical for stoichiometric calculations in reactions.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to determine the mole-to-mole relationships between reactants and products. This enables the calculation of the necessary amount of one reactant based on the amount of another, ensuring complete reaction without excess.

Mole-to-Mass Conversion

Mole-to-mass conversion is the process of converting the number of moles of a substance into a corresponding mass using its molar mass. This conversion is essential for translating theoretical amounts from stoichiometric calculations into practical, measurable quantities for laboratory use.

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