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We’re being asked to calculate the pH of buffer composed of H2PO4-(aq) and HPO42-(aq). To calculate for pH, we’re going to use the Henderson-Hasselbalch equation:
We know that
So first have to figure out which Ka value we’re going to use for our calculation. Phosphoric acid (H3PO4) is a weak triprotic acid, meaning it can donate three protons (H+) and it will have three equilibrium reactions.
Removing one H+ per step in H3PO4:
Phosphoric acid is a triprotic acid (Ka1 = 6.9 x 10-3, Ka2 = 6.2x 10-8, and Ka3 = 4.8 x10-13). To find the pH of a buffer composed of H2PO4- (aq) and HPO42- (aq), which pKa value would you use in the Henderson-Hasselbalch equation?
Calculate the pH of a buffer solution obtained by dissolving 13.0 g of KH2PO4(s) and 26.0 g of Na2HPO4(s) in water and then diluting to 1.00 L.
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Our tutors have indicated that to solve this problem you will need to apply the Polyprotic Acid concept. You can view video lessons to learn Polyprotic Acid. Or if you need more Polyprotic Acid practice, you can also practice Polyprotic Acid practice problems.
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Based on our data, we think this problem is relevant for Professor Bindell's class at UCF.