10A.Complete the table below for the potassium hydrogen phthalate buffer followi

Question

10A.Complete the table below for the potassium hydrogen phthalate buffer following the addition of 1.00 mL of 0.60M HCI Assume you started with only moles of the hydrogen phthalate ion. HCgH404 (aq) + Moles in 50.0 mL before addition of acid Moles of acid added to this volume of buffer Moles in 50.0 mL after addition of acid (equilibrium will be established between the species that remain after the addition of this strong acid) Approx 0 Submit Answer Tries 0/99 10B. Using the information from the table you completed in 10A, calculate the pH of 50.0 mL of the potassium hydrogen phthalate buffer, following the addition of 1.00 mL of 0.60M HC Note: enter all pH values to 3 significant figures.

Explanation / Answer

we know that

for buffers

pH = pKa + log [base / acid]

in this case

base ---> HC8H404-

acid---> H2C8H404

so

pH = pKa + log [HC8H404-/ H2C8H404]

now

pKa for H2C8H404 is 289

so

pH = 2.89 + log [0.00136 / 0.0006]

pH = 3.2454

so

pH of the solution after addition of HCl is 3.2454

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