What volume of 2.148 H2SO4 would be required to react to the equivalence point with 85.16g of KOH(s)?

Answer 1

I will assume that you mean 2.148 M H2SO4.

The reaction to reach the equivalence point is
H2SO4 + 2KOH -> 2H2O + K2SO4.
First find the moles of KOH= 85.16/57 appx= 1.5 molar.

From the equation, we need 0.75 moles of H2SO4. From the definition of molarity,
moles = volume(in L) x molarity
0.75 = 2.148 M x Volume = 0.36 moles approximately.,