Problem for the group: Determine the weight in grams of sodium dihydrogen phosphate (NaH2PO4.H2O; FW = 138.01) and sodium hydrogen phosphate (Na2HPO4; FW = 141.98) needed to prepare 1L of a standard buffer at pH 7.0 with a total phosphate concentration of 0.1M. (pKa =6.86)
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An aqueous solution is made by dissolving 11.24 g of sodium phosphate (tribasic) anhydrous salt in water to make 250 mL of solution. What is the expected pH of this solution? The pKa values for phosphoric acid are 2.15, 7.2, and 12.38.
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You are asked to make up a pH=6.86, 0.1M phosphate buffer. The pKa for sodium phosphate monobasic (pKa=6.86). Using the Henderson-Hasselbalch equation, what molar concentration of Sodium phosphate monobasic do we need?
Calculate and weigh out the correct amounts (g) of Na2HPO4 (Sodium phosphate dibasic) and NaH2PO4 (Sodium phosphate monobasic) to make a 0.1 M solution in 50 mL. Solution 1: Na2HPO4 = 141.95 g/mol Solution 2: NaH2PO4 = 120.00 g/mol (corrected) b) Determine the amount (in milliliters) of 0.1M NaH2PO4 and 0.1M Na2HPO4 solutions required to prepare 50 mL of Sodium phosphate buffer at pH 7.4. Sodium phosphate buffer has a pKa of 7.21. Henderson-Hasselbalch equation:
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