pH Calculations of Polyprotic Systems b.)What is the pH of 0.1000 M NaH2PO4? (Ka1 = 6.9x10-3, Ka2=6.2x10-8) c.)What is the pH of 0.1000 M Na2HPO4? (Ka2=6.2x10-8, Ka3=4.8x10-13) d.)What is the pH of 0.1000 M Na3PO4? (Ka3=4.8x10-13)
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- 2,What is the pH of the solution with hydronium ion concentration of 6.3 x 10-12 M? Group of answer choices 10.80 12.60 11.20 11.80 10.20 3,Calculate the pH of 0.50 L of the solution containing 5.61.0g KOH dissolved at 25oC. Group of answer choices 13.30 13.00 0.33 13.70 1.33 4. Calculate the [H3O+]of the solution with pH=9.2. Group of answer choices 2.0 x 10-10 3.6 x 10-9 6.3 x 10-10 9.2 x 10-9 2.0 x 10-9Calculate the pKa of hydrofluoric acid (HF(aq)) and hydrogen cyanide (HCN). What would be the pH of a solution containing 5 mM HF? What would be the pH of a solution containing 5 mM HCN?You do not need concentrations. Standard Gribbs Free energy for HF is -296.8 and for HCN is 124.7 This calculation assumes the acid is completely dissociated. You need the pKa to figure out how much of the H+ is free. This was all I was given. I do not know where to start, what I need, or what I need to calculate first. There are no other instructions or parts to this question. I'm at a loss, where do I begin?When calculating the PH for a .023 mole solution of HBrO2. My Ki is 2.1x10-4 and PH is 2.6. However Calculate the PH for a solution that is .023 M in HBrO2 and .03M in Ca(BrO2)2? Ki for HBrO2 = 2.1x10-4 Will that increase my PH?
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