On a lab exam, you have to find the concentrations of the monoprotic (one proton per molecule) acids ha and hb. you are given 43.5 ml of ha solution in one flask. you titrate this flask of ha solution with 87.3 ml of 0.0906 m naoh. calculate the molarity of the ha solution

0.1818 M

Explanation:

For the process of titration , the formula we use is -

M₁V₁ = M₂V₂

Where ,

M₁ = initial concentration of the acid

V₁ = initial volume of the acid

M₂ = final concentration of the base

V₂ = final volume of the base

Hence , from the question ,

The given data is ,

M₁ = ?

V₁ = 43.5 mL

M₂ = 0.0906 M

V₂ = 87.3 mL

Now, to determine the unknown quantity , the formula can be applied ,

Hence ,

M₁V₁ = M₂V₂

Putting the respective values ,

? *  43.5 mL =  0.0906 M * 87.3 mL

solving the above equation ,

M₁ = ? = 0.1818 M

what is the question?