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

the dependant variable is spilled water

the independent is the heat

i'm wiling to try and you : )