A student titrated 10.00 mL of 0.131 M H2SO4, this is the analyte which was pipetted into the Erlenmeyer flask and five drops of the indicator was added. The titrant, a solution of NaOH with an unknown concentration, was in the burette. The NaOH, titrant, was added to the Erlenmeyer flask until the indicator in the analyte solution changed color which indicates neutralization of the acid – analyte. This titration used 17.34 mL of NaOH to reach the end point – the color change of the indicator. Step 1: Fill in the calculation to determine how many moles of H2SO4 reacted in this titration to reach the end point. ( A )H2SO4 !!! ( B )H2SO4 / 1 L H2SO4 = mol H2SO4 A: Choose... B: Choose... Step 2: Fill in the calculation. Use the previous answer to determine how many moles of NaOH reacted in this titration to reach the end point. mol H2SO4 !!! ( C ) mol NaOH / ( D ) mol H2SO4 = mol NaOH C: Choose... D: Choose... Step 3: Fill in the calculation. Use the previous answer to determine the concentration of NaOH that was in the burette, the titrant, in this titration. mol NaOH !!! 1 / ( E )NaOH = M NaOH E: Choose...