How many grams of Ca(OH)2 are there if a sample is titrated to the complete endpoint with 38.0 mL of 0.120N HCl?
for HCl, normality and molarity is same since HCl has only 1 H+
we have the Balanced chemical equation as:
2 HCl + Ca(OH)2 ---> CaCl2 + 2 H2O
lets calculate the mol of HCl
volume , V = 38.0 mL
= 3.8*10^-2 L
we have below equation to be used:
number of mol,
n = Molarity * Volume
= 0.12*0.038
= 4.56*10^-3 mol
From balanced chemical reaction, we see that
when 2 mol of HCl reacts, 1 mol of Ca(OH)2 reacts
mol of Ca(OH)2 reacted = (1/2)* moles of HCl
= (1/2)*4.56*10^-3
= 2.28*10^-3 mol
This is number of moles of Ca(OH)2
Molar mass of Ca(OH)2 = 1*MM(Ca) + 2*MM(O) + 2*MM(H)
= 1*40.08 + 2*16.0 + 2*1.008
= 74.096 g/mol
we have below equation to be used:
mass of Ca(OH)2,
m = number of mol * molar mass
= 2.28*10^-3 mol * 74.096 g/mol
= 0.169 g
Answer: 0.169 g
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