Phosphoric acid is triprotic with the step-wise dissociation shown below. A 0.92 M phosphoric acid solution is prepared. Calculate the equilibrium concentrations of the species indicated. Report all answers in scientific notation using 2 sig figs. Rather than use the quadratic equation, you can make assumptions like we do in class (ie if K<<1, then 0.1-x ~ 0.1) H3PO4H3PO4 + H2OH2O ↔↔ H2PO−4H2PO4- + H3O+H3O+ Ka1=7.5x10−3Ka1=7.5x10-3 H2PO−4H2PO4- + H2OH2O ↔↔ HPO2−4HPO42- + H3O+H3O+ Ka2=6.2x10−8Ka2=6.2x10-8 HPO2−4HPO42- + H2OH2O ↔↔ PO3−4PO43- + H3O+H3O+ Ka3=4.8x10−13Ka3=4.8x10-13 What is the pH of this solution? Report pH as a number and not in scientific notation.
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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Phosphoric acid is triprotic with the step-wise dissociation shown below. A 0.92 M phosphoric acid solution is prepared. Calculate the equilibrium concentrations of the species indicated. Report all answers in scientific notation using 2 sig figs. Rather than use the quadratic equation, you can make assumptions like we do in class (ie if K<<1, then 0.1-x ~ 0.1)
| H3PO4H3PO4 | + | H2OH2O | ↔↔ | H2PO−4H2PO4- | + | H3O+H3O+ | Ka1=7.5x10−3Ka1=7.5x10-3 |
| H2PO−4H2PO4- | + | H2OH2O | ↔↔ | HPO2−4HPO42- | + | H3O+H3O+ | Ka2=6.2x10−8Ka2=6.2x10-8 |
| HPO2−4HPO42- | + | H2OH2O | ↔↔ | PO3−4PO43- | + | H3O+H3O+ | Ka3=4.8x10−13Ka3=4.8x10-13 |
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What is the pH of this solution? Report pH as a number and not in scientific notation. |
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