Two beakers each initially contain 1.00 L of liquid at 25 °C
CHEMISTRY · Multi-part · A Level · Chemistry · Acids and bases · Acids and bases
Problem
Two beakers each initially contain 1.00 L of liquid at 25 °C.
• Beaker X: 0.10 M acetic acid (CH₃COOH) and 0.10 M sodium acetate (CH₃COONa)
• Beaker Y: pure distilled water
Into each beaker, 0.0020 mol of gaseous HCl is bubbled with no appreciable change in volume.
(a) For the solution in beaker X, write the balanced net ionic equation that shows the predominant chemical reaction occurring when the HCl dissolves.
(b) Qualitatively compare the amount (in moles) of free hydronium ion produced in beaker X with that produced in beaker Y after the addition of HCl. Justify your comparison.
(c) Explain, in terms of chemical species present and their interactions, why the final pH of beaker X is expected to be significantly higher than the final pH of beaker Y.
(d) Describe one additional experimental observation (other than pH measurement) that would provide evidence that the buffered solution in beaker X resists the acid addition more effectively than the water in beaker Y.