(Solved): Create an ICE table to determine the concentration of mystery H2SO4. Introduction: Adding a drop of ...

Introduction: Adding a drop of strong acid or base into a neutralized solution is similar to adding a drop of strong acid or base to water-it causes an abrupt change in $$\mathrm{pH}$$. By using an appropriate indicator, a chemist can tell when a solution is neutralized by monitoring its color. Question: How is titration used to determine an unknown concentration? 1. Measure: Titrate the sulfuric acid analyte $$\left({\mathrm{H}}_2{\mathrm{SO}}_4\right)$$ with the sodium hydroxide titrant $$(\mathrm{NaOH})$$. How much $$1.00\mathrm{M}\mathrm{NaOH}$$ is needed to neutralize the $${\mathrm{H}}_2{\mathrm{SO}}_4$$ solution (how many $$\mathrm{mL}$$ of titrant needed for the solution in the flask to turns blue/purple)? $$21.6\mathrm{mL}\mathrm{mL}$$ 2. Interpret: The balanced equation for the reaction of $${\mathrm{H}}_2{\mathrm{SO}}_4$$ and $$\mathrm{NaOH}$$ is given at bottom right. 3. Recall: that molarity is equal to the number of moles of a substance dissolved in one liter of solution: concentration $$=$$ moles $$+$$ volume. $$(c=n/V)$$ Use a stoichiometric table (just like we practiced in class) and determine the concentration of the Mystery $${\mathrm{H}}_2{\mathrm{SO}}_4$$. Show your work below (don't worry about editing formulas and subscripts, as I know this takes a lot of time). If you have extra time, view: Titration Curves and Titration Curves and Acid Base Indicators Burette: $$1.00\mathrm{M}\mathrm{NaOH}$$ is a strong base. Flask: Mystery $${\mathrm{H}}_2{\mathrm{SO}}_4$$ is a strong acid. The initial $$\mathbf{pH}$$ of the solution is $$0.9$$. Indicator: Bromothymol blue is yellow when $$\mathrm{pH}$$ is below $$6.0$$ and blue when $$\mathrm{pH}$$ is above $$7.6$$. Balanced chemical equation: $${\mathrm{H}}_2{\mathrm{SO}}_4+2\mathrm{NaOH}?{\mathrm{Na}}_2{\mathrm{SO}}_4+2{\mathrm{H}}_2\mathrm{O}$$