Suppose that a student spills a solution containing 10.0 g of hydrochloric acid

Question

Suppose that a student spills a solution containing 10.0 g of hydrochloric acid (HCI) onto a laboratory bench. a. How many moles of HCI was spilled? b. The student is instructed to neutralize the spill by adding sodium hydrogen carbonate (baking soda, NaHCO_3). The neutralization reaction is: NaHCO_3(s) + HCI(aq) rightarrow H_2 O(I) + CO_2 (g) + NaCI(aq) How many moles of NaHCO3 must be added to completely react with the HCI that was spilled? c. Starting with your answer to part (b), calculate the grams of baking soda required to neutralize the acid spill.

Explanation / Answer

(a)

Moles of HCl = mass of HCl / Molar mass of HCl

n = 10.0 / 36.5

n = 0.274 mol

(b) From the balanced equation .

1 mol HCl requires 1 mol NaHCO3

then, 0.274 mol HCl needs 0.274 mol NaHCO3

(c) Mass of NaHCO3 = moles * molar mass of NaHCO3

m = 0.274 * 84

m = 22.8 g. of NaHCO3 is needed to neutralise the spill.

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