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Chemistry
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27 Jun 2020

A   container has    of formic acid that was dissociated in water. After it reaches equilibrium, it has    of formate. What are the concentrations of formic acid and its product at equilibrium?

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AP Chemistry
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Solve problems involving acid-base equilibria
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Related questions

A buffer is composed of formic acid and its conjugate base, the formate ion.  

  1. What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M?  
  2. What must the ratio of acid to conjugate base be to have a pH value of 0.50 units higher than the value calculated in part (a)?

Ka for formic acid is 1.8x10-4

 

A solution is prepared by dilating .10 mol formic acid (HCO2H) withwater to a volume of 1.0L. At equilibrium, the H3O^+^ concentrationis 4.2x10^-3 M. What is the equilibrium constant for thedissociation of formic acid in water?

HCO2H + h2) -> HCO2 + H3O^+^

A buffer is composed of formic acid and its conjugate base, the formate ion.

(a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035M? 

(b) What must the ratio of conjugate base to acid be to have a pH value that is 0.50 units higher than the value calculated in part (a)? 

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