CaCO3 (s) + HCl(aq) --------------> CO2 (g) + CaCl2 (aq) + H2O (l)
Suppose a chemist mixed 2.00g of CaCO3 (s) with 100ml of 0.250 M HCl. What mass of each of the three products would form?
In the question above, what is the concentration of CaCl2 in solution after that reaction has been completed?
Please put in terms I can understand.
First of all, balance the reaction before you start to solve anything (put a 2 in front of the HCl)...
CaCO3 (s) + 2 HCl(aq) --------------> CO2 (g) + CaCl2 (aq) + H2O (l)
50 mL is 0.050 L
moles of HCl = (0.050 L)(0.1 M) = 0.005 mol HCl
For every 2 mol of HCl you need one mole of CaCO3, therefore
moles of CaCO3 = (1 mol CaCO3/ ...
The solution is completed step-by-step.