Calculating pH using Ka: Equal Concentrations of HB and B-

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To calculate the pH of a solution with equal concentrations of the weak acid HB and its conjugate base B-, the Henderson-Hasselbalch equation is applicable. Given the acid dissociation constant (Ka) of 5.293 x 10^-6, the pH can be determined by using the relationship pH = pKa + log([B-]/[HB]). Since the concentrations of HB and B- are equal, the log term becomes zero, simplifying the calculation to pH = pKa. The pKa can be calculated as -log(5.293 x 10^-6), leading to the final pH value.
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Homework Statement



ka= 5.293 x 10^-6

using Ka, calculate the ph of a solution that contains equal concentrations of HB and B-.


Homework Equations



ph = -log[H+]

The Attempt at a Solution



im guessing that HB is the acid and B- is the base
 
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thanks
 

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