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Chapter 4: Problem 83

Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resulting solution. The sodium bicarbonate reacts with sulfuric acid according to: $$ \begin{aligned} 2 \mathrm{NaHCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+& \\ & 2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g) \end{aligned} $$ Sodium bicarbonate is added until the fizzing due to the formation of \(\mathrm{CO}_{2}(g)\) stops. If \(27 \mathrm{~mL}\) of $6.0 \mathrm{MH}_{2} \mathrm{SO}_{4}\( was spilled, what is the minimum mass of \)\mathrm{NaHCO}_{3}$ that must be added to the spill to neutralize the acid?

Short Answer

Expert verified
The minimum mass of NaHCO3 required for neutralizing the acid spill can be calculated using the following steps: 1. Calculate moles of H2SO4 spilled: \(Moles\: of\: H_{2}SO_{4} = 0.027 L \times 6.0 M = 0.162\: moles\) 2. Calculate moles of NaHCO3 required: \(Moles\: of\: NaHCO_{3} = 2 \times Moles\: of\: H_{2}SO_{4} = 2 \times 0.162\: moles = 0.324\: moles\) 3. Convert moles of NaHCO3 to grams: \(Mass\: of\: NaHCO_{3} = 0.324\: moles \times 84 \frac{g}{mol} = 27.216 g\) Therefore, the minimum mass of NaHCO3 required to neutralize the acid spill is 27.216 g.

Step by step solution

01

Find moles of sulfuric acid (H2SO4) spilled on the bench

To calculate the moles of H2SO4, we need to multiply the volume of the spilled acid (27 mL) by its concentration (6.0 M): Moles of H2SO4 = Volume × Concentration First, convert the volume of H2SO4 from mL to L: 27 mL = 0.027 L Now, multiply the volume (in L) by the concentration: Moles of H2SO4: \(= 0.027 L \times 6.0 M\)
02

Use stoichiometry to find moles of sodium bicarbonate (NaHCO3) required

The balanced equation shows the stoichiometric ratio between the reactants: \(2 \mathrm{NaHCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)\) As per the equation, 2 moles of NaHCO3 are required to neutralize 1 mole of H2SO4. So we can find the amount of NaHCO3 required: Moles of NaHCO3 = 2 × Moles of H2SO4
03

Convert moles of sodium bicarbonate (NaHCO3) to grams

To find the mass of NaHCO3, we need to multiply the number of moles of NaHCO3 with its molar mass. The molar mass of NaHCO3 = 23 (Na) + 1 (H) + 12 (C) + 16 x 3 (O) = 84 g/mol Mass of NaHCO3 = Moles of NaHCO3 × Molar Mass of NaHCO3 Calculate the minimum mass of NaHCO3 required for neutralizing the acid spill.

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Most popular questions from this chapter

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