What is the pH of a solution obtained by mixing 30.00 ml of 0.500 M HCl and 30.00 mL of 0.250 M NaOH?
convert to mols for both the HCl and NaOH
mols HCl = 0.03000L * 0.500 M = 0.0150 mols
mols NaOH = 0.03000L * 0.250 M = 0.00750 mols
Neutralization occurs, whereby all of the NaOH is used up.
Calculating the mols of HCl remaining...
0.0150 - 0.00750 = 0.00750 mols HCl
All of the HCl dissociates, meaning we have 0.00750 mols of H+
The pH is given by taking the -log of [H+]
= 2.125 (with sigfigs in mind
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