Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by spr

Question

Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium hydrogen carbonate on it and then mopping up the resultant solution. The sodium hydrogen carbonate reacts with sulfuric acid producing sodium sulfate, water, and carbon dioxide. Sodium hydrogen carbonate is added until the fizzing due to the formation of carbon dioxide stops. If 22.0mL of 6.4 M sulfuric acid was spilled, what is the minimum mass of sodium hydrogen carbonate that must be added to the spill to neutralize the acid?

Explanation / Answer

H?SO? + NaHCO? --> NaHSO? + H?O + CO?

In order to find the mass of sodium bicarbonate required, we must find its number of moles, which can be found from its mole ratio with sulfuric acid.

Moles of sulfuric acid = Concentration x Volume = 6.4 x 0.022 = 0.1408 mol

Since the mole ratio of H?SO? to NaHCO? is 1:1 ;

Moles of sodium bicarbonate = Moles of sulfuric acid = 0.1408mol
Mass of sodium bicarbonate = Molar mass x Moles = 84 x 0.1408 = 11.827g

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