formic acid  =  HCOOH acetic acid  =  CH3COOH HCOOH is a stronger acid than CH3COOH (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.056 M aqueous formic acid and sodiumacetate are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO- as the formula for the formate ion Which is the strongest base, HCOO- or CH3COO- At equilibrium will the (reactants or products) be favored. ÂÂ
formic acid  =  HCOOH
acetic acid  =  CH3COOH
HCOOH is a stronger acid than CH3COOH
(1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.056 M aqueous formic acid and sodiumacetate are mixed. It is not necessary to include states such as (aq) or (s). Use HCOO- as the formula for the formate ion
Which is the strongest base, HCOO- or CH3COO-
At equilibrium will the (reactants or products) be favored.
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The Correct Answer and Explanation is:
Answer:
(1) Net ionic equation: HCOOH+CH3COO−⇌CH3COOH+HCOO−\text{HCOOH} + \text{CH}_3\text{COO}^- \rightleftharpoons \text{CH}_3\text{COOH} + \text{HCOO}^-
Strongest base:
CH₃COO⁻ (acetate ion)
At equilibrium, the:
Reactants will be favored.
Explanation
The reaction involves mixing formic acid (HCOOH), a weak acid, with sodium acetate (CH₃COONa), a salt that dissociates to produce acetate ions (CH₃COO⁻), the conjugate base of acetic acid. The key process here is an acid-base reaction between formic acid (an acid) and acetate (a base).
The net ionic equation focuses only on the species that change in the reaction: HCOOH+CH3COO−⇌CH3COOH+HCOO−\text{HCOOH} + \text{CH}_3\text{COO}^- \rightleftharpoons \text{CH}_3\text{COOH} + \text{HCOO}^-
This represents a proton transfer: formic acid donates a proton (H⁺) to acetate, forming acetic acid and formate ion.
To understand equilibrium direction, we compare acid strengths using their conjugate bases. It’s stated that formic acid is stronger than acetic acid. That means:
- HCOOH ⇌ H⁺ + HCOO⁻ has a greater tendency to donate protons than
- CH₃COOH ⇌ H⁺ + CH₃COO⁻
Thus, HCOO⁻ is a weaker base than CH₃COO⁻. A stronger acid has a weaker conjugate base.
Since the stronger acid (HCOOH) reacts with the stronger base (CH₃COO⁻), the system shifts toward the weaker acid-base pair: CH₃COOH and HCOO⁻.
In acid-base equilibria, the position favors the side with the weaker acid and base, i.e., the side that is less reactive.
Conclusion:
- CH₃COO⁻ is the stronger base.
- Since the stronger acid and stronger base are on the left, the reactants are favored at equilibrium.
- This means only a small amount of product (CH₃COOH and HCOO⁻) will form.
