Problem: The titration of 42.35 mL of H2SO4 requires 21.17 mL of 0.5000 M NaOH for complete neutralization. Calculate the concentration of H2SO4.(A) 0.2499 M H2SO4 (B) 0.1250 M H2SO4 (C) 0.4998 M H2SO4 (D) 1.000 M H2SO4 (E) 0.36 M H2SO4

FREE Expert Solution

We’re being asked to find the concentration of H2SOafter enough NaOH is added to the solution to neutralize.


Let’s first write the balanced reaction between H2SO4 and NaOH:

Reactants:

2SO4

▪ oxyacid → 2 more oxygens than hydrogens → strong oxyacid
▪ a strong acid → will completely dissociate in solution
H2SO4(aq) → 2 H+(aq) + SO42-(aq) 

 NaOH


View Complete Written Solution
Problem Details

The titration of 42.35 mL of H2SO4 requires 21.17 mL of 0.5000 M NaOH for complete neutralization. Calculate the concentration of H2SO4.

(A) 0.2499 M H2SO4 

(B) 0.1250 M H2SO4 

(C) 0.4998 M H2SO4 

(D) 1.000 M H2SO4 

(E) 0.36 M H2SO4

Frequently Asked Questions

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Schurmeier's class at UCSD.