If I combine 15.0 grams of calcium hydroxide with 75.0 mL of 0.500M HCl, how many grams of calcium chloride would be formed?

Question

Peyton Adams · Accepted Answer

Approx...#2*g#...

We adhere to the equation of stoichiometry. #Ca(OH)_2(s) + 2HCl(aq) rarr CaCl_2(aq) + 2H_2O# #n_(Ca(OH)_2)=(15.0*g)/(74.09*g*mol^-1)=0.203*mol# And we got with respect to #HCl# a molar quantity of... #75.0*mLxx0.500*mol*L^-1xx10^-3*L*mL^-1=0.0375*mol# Clearly the calcium hydroxide is present in molar excess....and at most we can form #(0.0375*mol)/2# of calcium chloride...a mass of #110.98*g*mol^-1xx(0.0375*mol)/2=??*g#.. The question operates under a faulty premise...because the species in solution after addition of the acid would be #Ca(OH)Cl#

Mateo Aguilar · Answer

undefined The balanced chemical equation for the reaction between calcium hydroxide (Ca(OH)₂) and hydrochloric acid (HCl) is:

Ca(OH)₂ + 2HCl → CaCl₂ + 2H₂O

Using the given amounts of calcium hydroxide and hydrochloric acid, calculate the moles of each reactant. Then, determine the limiting reactant. Once you have the limiting reactant, use stoichiometry to find the moles of calcium chloride formed. Finally, convert moles of calcium chloride to grams using its molar mass.