Chemistry Practice Problems Equivalence Point Practice Problems Solution: Titration of a strong acid with a strong base. The...

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Solution: Titration of a strong acid with a strong base. The pH curve for titration of 50.0 mL of a 0.100 M solution of hydrochloric acid with a 0.100 M solution of NaOH(aq). For clarity, water molecules have been omitted from the molecular art.What volume of NaOH(aq) would be needed to reach the equivalence point if the concentration of the added base were 0.280 M?

Problem

Titration of a strong acid with a strong base. The pH curve for titration of 50.0 mL of a 0.100 M solution of hydrochloric acid with a 0.100 M solution of NaOH(aq). For clarity, water molecules have been omitted from the molecular art.

The graph shows pH changes throughout titration. Only HCl is present before the titration (pH equals 1). H plus is consumed as OH minus is added, forming H2O (pH less than 7.0). A line beginning at pH 1 at 0 milliliters of NaOH increases linearly up to pH 2 at 45 milliliters of NaOH. H plus is completely neutralized by OH minus (pH equals 7.0). The equivalence point (pH 7, NaCl salt solution) occurs when moles of the base are equal to moles of the acid. The pH jumps suddenly at 50 milliliters of NaOH. No H plus is left to react with the excess of OH minus (pH greater than 7). After the drastic increase of pH near the equivalence point, the pH line increases linearly and slowly at the pH of around 12.

What volume of NaOH(aq) would be needed to reach the equivalence point if the concentration of the added base were 0.280 M?

Solution

We’re being asked to calculate the volume (in mL) of 0.280 M NaOH (strong base) required to reach the equivalence point in a titration of 50.00 mL of 0.100 M HCl (strong acid)


Recall that at the equivalence point of a titration:


moles acid=moles base


Also, recall that moles = molarity × volume

This means:


MVacid=MVbase


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