An aqueous solution of hydroiodic acid is
standardized by titration with a 0.116 M solution
of calcium hydroxide.
If 11.2 mL of base are required to neutralize
24.4 mL of the acid, what is the molarity of the
hydroiodic acid solution?
M hydroiodic acid
Balanced chemical equation is:
Ca(OH)2 + 2 HI ---> CaI2 + 2 H2O
Here:
M(Ca(OH)2)=0.116 M
V(Ca(OH)2)=11.2 mL
V(HI)=24.4 mL
According to balanced reaction:
2*number of mol of Ca(OH)2 =1*number of mol of HI
2*M(Ca(OH)2)*V(Ca(OH)2) =1*M(HI)*V(HI)
2*0.116*11.2 = 1*M(HI)*24.4
M(HI) = 0.1065 M
Answer: 0.106 M
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