A buffer is prepared by mixing 0.10 mol of Na2A and 0.050 mol of NaHA in 1.0 L. For A2, pKb1 is 4.00 and pKb2 is 8.00. Find the buffer's pH (assume all activity coefficients are 1).

Please show your work.

Given that pKb1 is 4.00 and pKb2 is 8.00, we can convert them to pKa values using the equation pKa + pKb = 14.00. Therefore, pKa1 = 14.00 - 4.00 = 10.00 and pKa2 = 14.00 - 8.00 = 6.00.

Now, we can substitute the values into the Henderson-Hasselbalch equation:

pH = 10.00 + log([Na2A]/[NaHA])

Since the concentrations of Na2A and NaHA are given as 0.10 mol and 0.050 mol, respectively, in a 1.0 L solution, we can calculate the ratio [Na2A]/[NaHA] as 0.10/0.050 = 2.00.

Substituting this ratio into the equation, we get:

pH = 10.00 + log(2.00)

Using logarithm properties, we can simplify the equation to:

pH = 10.00 + 0.3010

Calculating the sum, we find:

pH = 10.3010

Therefore, the buffer's pH is approximately 10.3010.

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A buffer is prepared by mixing 0.10 mol of Na2A and 0.050 mol of NaHA in 1.0 L. For A2, pKb1 is 4.00 and pKb2 is 8.00. Find the buffer's pH (assume all activity coefficients are 1).Please show your work.

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A buffer is prepared by mixing 0.10 mol of Na2A and 0.050 mol of NaHA in 1.0 L. For A2, pKb1 is 4.00 and pKb2 is 8.00. Find the buffer's pH (assume all activity coefficients are 1).

Please show your work.