An aqueous solution of hydroiodic acid is standardized by titration with a 0.138 M solution of potassium hydroxide. If 10.6 mL of base are required to neutralize 10.4 mL of the acid, what is the molarity of the hydroiodic acid solution?

The molarity of hydroiodic acid solution is 0.141 M

Explanation:

To calculate the concentration of acid, we use the equation given by neutralization reaction:

where,

are the n-factor, molarity and volume of acid which is HI

are the n-factor, molarity and volume of base which is KOH.

We are given:

Putting values in above equation, we get:

Hence, the molarity of hydroiodic acid solution is 0.141 M

the formula mass of a molecule or a compound is the sum of the atomic weights of the atoms in its empirical formula

(that's what i know about formula mass)

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2