Suppose 0.09886 m koh is titrated into 15.00 ml h2so4 of unknown concentration until the equivalence point is reached. it takes a total volume of 29.25 ml koh to neutralize the h2so4. what is the concentration of the acid? express the result to the proper number of significant figures based on the limits of data from the problem.

The chemical reaction between KOH and H2SO4 is:
2KOH + H2SO4 ⇒K2SO4 + 2H2O

According to the formula, at the end point where equivalence point is reached, the molar ratio between the reacted KOH and H2SO4 is 2:1. Based on this ratio, the concentration of the H2SO4 can be calculated.  Because all the measurement has 4 significant figures, we need to keep 5 significant figures during the calculation and 4 significant figures for the final answer.

The moles of KOH reacted is: 0.02925 L * 0.09886 M = 0.0028917 mole.
Based on the 2:1 ratio, the moles of H2SO4 in the solution is 0.0028917mole/2 = 0.0014458 mole.
So, the concentration of H2SO4 is: 0.0014458mole/0.01500L = 0.09639 mole/L, or 0.09639M.