We want to prepare 1.00 L of a buffer solution with a pH of 7.77. The following acid/base pairs are available. Which is appropriate to use for preparing this buffer? H3PO4/NaH2PO4 Ka = 7.5 × 10-3 pKa = 2.12 CH3CO2H/NaCH3CO2 Ka = 1.8 × 10-5 pKa = 4.74 NaH2PO4/Na2HPO4 Ka = 6.2 × 10-8 pKa = 7.21 NH4Cl/NH3 Ka = 5.6 × 10-10 pKa = 9.25 what mass of Na2HPO4 is required? Assume a 1.00 L volume buffer solution. Target pH = 7.77 Acid/Base pair: NaH2PO4/Na2HPO4 pKa = 7.21 [Na2HPO4] > [NaH2PO4] [NaH2PO4] = 0.100 M 12.0 g NaH2PO4 required [base]/[acid] = 3.63 [Na2HPO4] = 0.363 M

Q: Part 1: Calculate the concentration of each species present in a 0.050-M solution of H2S. (Ka1 = 1.1…

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A: Pkb =  -log(kb)     = - log(7.4×10-10 )  Pkb  = 9.13

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Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

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Q: a Calculate the pH of a solution that is 0.20 M HOCI and 0.88 M KOCI. Ka = 3.5x10-8 pH = 8.1 b In…

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Q: 9. Calculate the pH of 0.250 L of 0.36 M formic acid (CH2O2) – 0.30 M sodium formate (CHOżNa)…

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Q: Calculate the pH of a solution that is 0.20 M HOC1 and 0.92 M KOCI. Ka = 3.5x10-8 pH = 8.16 b In…

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Q: the pH calculated using the Henderson-Hasselbalch equation

A:

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A: Correct answer is option d. 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl

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Q: The buffer was made by combining 0.220 M lactic acid (HC3H5O3) and 0.200 M sodium lactate (…

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Q: Study guide answer is 4.77 for part 2 please show steps thanks

A: