To react with a #5.00g# mass of calcium hydroxide, what volume of #0.100mol*L^-1# #HCl# is required?

Question

1625 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2016-10-03T09:28:02

Approx. #1.4*L# hydrochloric acid are required.

We need (i) a chemical reaction:

#Ca(OH)_2(s) + 2HCl(aq)rarr CaCl_2(aq) + 2H_2O(l)#*

And (ii), the molar quantity of calcium hydroxide:

#=# #(5.00*g)/(74.09*g*mol^-1)# #=# #0.0675*mol#.

Given the rxn stoichiometry, clearly, we need #2xx0.0675*mol=0.135*mol# #HCl(aq)#.

And given our concentration of #HCl#, #(0.135*mol)/(0.100*mol*L^-1)xx10^3*mL*L^-1# #=# #??mL#

To react with a #5.00*g# mass of calcium hydroxide, what volume of #0.100*mol*L^-1# #HCl# is required?