We’re being asked to find the **concentration of H _{2}SO**

**Let’s first write the balanced reaction between H _{2}SO_{4} and NaOH:**

**Reactants:**

• **H _{2}SO_{4}**

▪ oxyacid → 2 more oxygens than hydrogens → *strong oxyacid*

▪ a strong acid → will completely dissociate in solution

▪ **H _{2}SO_{4(aq)} → 2 H^{+}_{(aq)} + SO_{4}^{2-}_{(aq)} **

**•**** Na****OH**

The titration of 42.35 mL of H_{2}SO_{4} requires 21.17 mL of 0.5000 *M* NaOH for *complete* neutralization. Calculate the concentration of H_{2}SO_{4}.

(A) 0.2499 *M* H_{2}SO_{4}

(B) 0.1250 *M* H_{2}SO_{4}

(C) 0.4998 *M* H_{2}SO_{4}

(D) 1.000 *M* H_{2}SO_{4}

(E) 0.36 *M* H_{2}SO_{4}

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Strong Acid Strong Base Titrations concept. You can view video lessons to learn Strong Acid Strong Base Titrations. Or if you need more Strong Acid Strong Base Titrations practice, you can also practice Strong Acid Strong Base Titrations practice problems.

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