The previous problem demonstrated how to find the total or \"initial\" concentra

Question

The previous problem demonstrated how to find the total or "initial" concentration of phosphoric acid ([H3PO4 in Cola from data at the first equivalence point. Together with the pH of the Cola before titration is begun, a1 In one trial, the pH of the Cola before titration was 2.41 and [H3Po1,was 0.00584 mol/L. Complete the ICE table below to reveal the equilibrium concentrations of H3PO4 H2PO . and H3o . Use three significant figures in each concentration and do not include units H2PO 0.005840 -X + X +X

Explanation / Answer

The ICE table ( initial, change, equilbirium ) table has been aready filled up partially

so

th eequilbirum conditions is the final amount due to I and C

E = I + C

for H3PO4:

E = 0.0084 - x

for H2PO4-

E = 0 + x

for H3O+

E = 0 + x

Then

Ka = x*x/(0.00584-x)

x^2 + Ka*x - (0.00584)*Ka = 0

Assign Ka for the ionization and solve via quadratic equation

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