A 0.50 M solution of H Br is to be poured into a beaker that initially contains 50 g of solid CaCO3. Determine the volume of H Br that will be needed to completely react with the 50 g of solid CaCO3.

2 liters of HBr is needed to completely react with the 50 g of salt.

Explanation:

First of all, we determine the reaction:

2HBr + CaCO₃ →  CaBr₂  +  CO₂  + H₂O

We need to calculate, moles of carbonate in order to state the stoichiometry (1:2)

50 g . 1mol / 100.08g = 0.499 mol

1 mol of salt need 2 moles of acid to react, according to stoichiometry

Then, 0.499 moles of salt, will react with (0.499 . 2)/1 = 0.999 moles

As we have the [HBr], we can calculate the volume.

M = mol/L → we replace → 0.50 mol/L = 0.999 mol /L

L = 0.999 mol/0.50 mol → 1.99 L ≅ 2L

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error