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Consider the titration of 25.0 mL of 0.210 MHCO2H with 0.250 MNaOH. (Ka of HCO2H is...

Consider the titration of 25.0 mL of 0.210 MHCO2H with 0.250 MNaOH. (Ka of HCO2H is 1.8×10^−4) How many milliliters of base are required to reach the equivalence point? Calculate the pH after the addition of 8.0 mL of base. Calculate the pH at halfway to the equivalence point. Calculate the pH at the equivalence point. Calculate the pH after the addition of 30.0 mL of base

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Expert Solution

Answer = 21.0 ml

b.

c.

d.

e.

queen_honey_blossom answered 2 years ago
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