7A.Complete the table below for the addition of 1.00 mL of 0.60M HCI to 50.0 mL

Question

7A.Complete the table below for the addition of 1.00 mL of 0.60M HCI to 50.0 mL of the acetate buffer. CH3Coo (ag)+ 0.00080 0.00120 Ok Moles in 50.0 mL before addition of acid Ok 0.00060 Moles of acid added to this volume of buffer Ok 0.0014 0.00065 Ok Moles in 50.0 mL after addition of acid Approx 0 (equilibrium will be established between the species that remain after the addition of this strong acid) Ok You are correct. Your receipt no. is 161-3839 Previous Tries ) 7B. Using the information from the table you completed in 7A, calculate the pH of 50.0 mL of the acetate buffer following the addition of 1.00 mL of 0.60M HCI Note: enter all pH values to 3 significant figures.

Explanation / Answer

Using the values from Table 7A ,

[acid] = 0.0014

[acetate] = 0.00065

and pKa of acetic acid = 4.75

Thus the solution is a buffer whose pH is calculated using Hendersen equation.

pH = pKa + log [acetate]/[acid]

= 4.75 + log [0.00065/0.0014]

= 4.416

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