Some sulfuric acid spilled on a lab bench. It can be neutralized by sprinkling s

Question

Some sulfuric acid spilled on a lab bench. It can be neutralized by sprinkling sodium is bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid as follows: 2 NaHCO_3(s) + H_2SO_4 (aq) rightarrow Na_2SO_4(aq) + 2H_2O(I) + 2CO_2 (g) sodium bicarbonate is added until the fizzing due to the formation of Co_2(g) stops. If 27 mL of 6.0 M H_2SO_4 was spilled, what is the minimum mass of NaHCO_3 that must be added to the spill to neutralize the acid?

Explanation / Answer

Moles of H2SO4 given = 6.0 * 27 / 1000 = 0.162 mol

From the balanced equation provided,

1 mol H2SO4 requires 2 mol NaHCO3

Then, 0.162 mol H2SO4 requires 2 * 0.162 = 0.324 mol NaHCO3

Mass of NaHCO3 required = moles * molar mass = 0.324 * 84.0 = 27.2 g.

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