Which one is the correct equation?

[lkh1986]

The molecular equation for the reaction between HCHO2 and K2CO3 is
2HCHO3 +K2CO3 --> H2CO3 + 2KCHO2.

H2CO3 will undergo further reaction to become H2O and CO2, so maybe the molelar equation can be written as 2HCHO3 +K2CO3 --> H2O + CO2 + 2KCHO2. Which of the molecular equation is the correct one?

Then, for ionic equation, which one of the following is the correct one?
2HCHO2 + 2K+ + CO32- --> H2CO3 + 2K+ + 2CHO2-
or
2HCHO2 + 2K+ + CO32- --> H2O + CO2 + 2K+ + 2CHO2-
or
2H+ + 2CHO2- + 2K+ + CO32- --> H2CO3 + 2K+ + 2CHO2-
or
2H+ + 2CHO2- + 2K+ + CO32- --> H2O + CO2 + 2K+ + 2CHO2-

Do we need to separate the acid? But then again it is a weak acid.
However, since this reaction is a neutralization reaction between an acid and a base, it would be weird if we don't separate the acid into ions. Technically, small percene of the acid do ionize.

 

[sdekivit]

The molecular equation for the reaction between HCHO2 and K2CO3 is
2HCHO3 +K2CO3 --> H2CO3 + 2KCHO2.

H2CO3 will undergo further reaction to become H2O and CO2, so maybe the molelar equation can be written as 2HCHO3 +K2CO3 --> H2O + CO2 + 2KCHO2. Which of the molecular equation is the correct one?

The second is correct, because H2CO3 doesn't exist in a solution and always dissociates in H2O and CO2.

Then, for ionic equation, which one of the following is the correct one?
2HCHO2 + 2K+ + CO32- --> H2CO3 + 2K+ + 2CHO2-
or
2HCHO2 + 2K+ + CO32- --> H2O + CO2 + 2K+ + 2CHO2-
or
2H+ + 2CHO2- + 2K+ + CO32- --> H2CO3 + 2K+ + 2CHO2-
or
2H+ + 2CHO2- + 2K+ + CO32- --> H2O + CO2 + 2K+ + 2CHO2-

none are correct, since you have equal amount K+ on both sides of the arrow so they cancel each other out. But apart from that i would go for the second one.

Do we need to separate the acid? But then again it is a weak acid.
However, since this reaction is a neutralization reaction between an acid and a base, it would be weird if we don't separate the acid into ions. Technically, small percene of the acid do ionize.

assume the reaction takes place completely all HCOOH will form HCOO-

 

[Blueshift5]

I cannot definitively say which equation is correct without more information about the reaction conditions. However, it is important to note that molecular equations and ionic equations serve different purposes and may be used in different contexts.

The molecular equation provided, 2HCHO3 + K2CO3 --> H2CO3 + 2KCHO2, is a balanced equation that shows the reactants and products in their molecular form. This equation is useful for predicting the products of a reaction and determining the stoichiometry (mole ratios) of the reactants and products.

The second set of equations provided are ionic equations, which show the dissociation of the reactants into their respective ions. These equations are useful for understanding the actual species present in a solution and can help determine the net ionic equation, which only includes the species that actually participate in the reaction. The correct ionic equation would depend on the solubility of the reactants and products in the given reaction conditions.

In terms of separating the acid into ions, it is important to note that even weak acids do ionize to some extent, and this should be reflected in the ionic equation. However, the extent of ionization may vary depending on the strength of the acid and the concentration of the solution. Therefore, it is important to consider the specific conditions of the reaction when determining the correct ionic equation.

In summary, both the molecular and ionic equations are correct in their own contexts and serve different purposes. The correct equation would depend on the specific reaction conditions and the purpose for which it is being used.