What volume in ml of a 0.121 m sodium hydroxide solution is required to reach the equivalence point in the complete titration of a 10.0 ml sample of a 0.102 m sulfuric acid? (hint: write the equation out)

8.42 mL

Explanation:

For the equivalence point for the reaction of an acid and base , is given by the following formula -

M₁V₁ = M₂V₂

where ,

M₁ = acid's concentration ,

V₁ = acid's volume ,

M₂ = base's concentration ,

V₂ = base's volume .

from , the question ,

M₁  = 0.102 M ( acid )

V₁ = 10.0 mL  ( acid )

M₂ = 0.121 M ( base )

V₂ = ?

To calculate the volume of the base , the above formula is used and the respective values are substituted , as follow -

M₁V₁ = M₂V₂

0.102 M *  10.0 mL = 0.121 M * V₂  

V₂  = 1.02 / 0.121 = 8.42 mL

i belive it is water