Part B. After addition 25.0 mL of KOH
Write the chemical equation for the reaction between H3PO3 and NaOH.
H3PO3(aq) + NaOH(aq) ⇌ F-(aq) + H2O(l)
*Main group metals should have a +3 charge or higher to be considered acidic. Na+ has only a +1 charge and is a neutral ion so it will not contribute to the pH of the solution
Calculate the initial amounts of H3PO3 and NaOH in moles before the reaction happens.
molarity (volume) → moles
*convert volumes from mL to L → 1 mL = 10-3 L
Phosphorous acid, H3PO4(aq), is a diprotic oxyacid that is an important compound in industry and agriculture.
pKa1 = 1.30
pKa2 = 6.70
Calculate the pH for each of the following points in the titration of 50.0 mL of a 1.5 M H3PO3(aq) with 1.5 M KOH(aq).
Part C. after addition of 50.0 mL of KOH
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