Question

How many grams of calcium chloride would form if 1.25 liters of a 2.50 molar hydrochloric acid (HCl) solution reacts with 1.10 liters of a 2.25 molar calcium hydroxide Ca(OH)2 solution? (2 points) 2HCl (aq) + Ca(OH)2 (aq) yields CaCl2 (aq) + H2O (l)

Answer 1

Hello!

The chemical equation for this reaction is the following:

2HCl (aq) + Ca(OH)₂(aq) → CaCl₂(aq) + H₂O(l)

To determine the grams of Calcium Chloride formed, we will need to determine the moles of each reactant and divide by the reaction coefficient to know which is the limiting reactant (the one that is in the lowest amount):

$moles HCl= \frac{vHCl*cHCl}{2} = \frac{1,25L*2,50M}{2} =1,5625 molesHCl \\ \\ molesCa(OH)_2=vCa(OH)_2*cCa(OH)_2=1,10L*2,25M \\ moles Ca(OH)_2=2,475 moles Ca(OH)_2$

So, the limiting reactant is HCl, so we'll use the following conversion factor to determine the mass of CaCl₂ produced:

$1,25 L HCl* \frac{2,50 mol HCl}{1 L}* \frac{1 mol CaCl_2}{2 mol HCl}* \frac{110,98 g CaCl_2}{1 mol CaCl_2}= 173,41 g CaCl_2$

So, 173,41 grams of CaCl₂ are produced.

Have a nice day!