Problem: Calculate the pH of the resulting solution if 32.0 mL of 0.320 M HCl(aq) is added to 37.0 mL of 0.320 M NaOH (aq).

FREE Expert Solution

Given: 32.0 mL of 0.320 M HCl(aq) + 37.0 mL of 0.320 M NaOH(aq)


Reaction: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)


Calculating moles of each:

32.0 mL×1 L10-3 mL×0.320 mol HCl1 L = 0.01024 mol HCl


37.0 mL×1 L10-3 mL×0.320 mol NaOH1 L = 0.01184 mol NaOH


Since mol HCl < mol NaOH

0.01184 mol NaOH – 0.01024 mol HCl = 1.6 × 10–3 mol NaOH

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Problem Details

Calculate the pH of the resulting solution if 32.0 mL of 0.320 M HCl(aq) is added to 37.0 mL of 0.320 M NaOH (aq).

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