15 Facts on HF + Na2CO3: What, How To Balance & FAQs

Na₂CO₃ is often known as soda ash or washing soda. It is a non-volatile base. HF is an ionic, polar weak acid with a dipole moment of 1.86 D. Let us see how Na₂CO₃ reacts with HF.

Na₂CO₃ is a water – soluble white solid and a sodium salt of carbonic acid. Its major source is trona ore. It is used in soaps, paper, water glass, and acts as a water softener and base. HF is linear with a point group C∞v. Its 60 % is used to make the refrigerants. French chemist Edmond Frémy is credited with the HF.

In this article, we will discuss important facts about HF + Na₂CO₃ chemical reactions such as reaction enthalpy, the heat required, the product formed, the type of reaction, the type of intermolecular forces between their compounds, etc.

What is the product of HF and Na₂CO₃

Sodium fluoride (NaF), carbon dioxide (CO₂), and water (H₂O) is produced during the reaction of HF and Na₂CO₃ where Sodium fluoride is dissolved in water.

2 HF (aq) + Na₂CO₃ (s) = 2 NaF (aq) + H₂O (l) + CO₂ (g)

What type of reaction is HF +Na₂CO₃

HF + Na₂CO₃ is double displacement (salt metathesis), acid – base (neutralization), and an exothermic reaction.

How to balance HF +Na₂CO₃

The unbalanced molecular equation for HF + Na₂CO₃ is.

HF (aq) + Na₂CO₃ (s) = NaF (aq) + H₂O (l) + CO₂ (g)

To balance this equation, we should follow the steps given below:

• Here, the number of H and Na atoms is not the same on both sides of the reaction. So we will multiply these atoms with some coefficients so that they become equal.
• The total number of H atoms on the reactant side is 1 while on the product side it is 2.
• So, we multiply the HF with a coefficient of 2 on the reactant side so that the number of H atoms becomes 2 on both sides of the reaction.
• 2 HF (aq) + Na₂CO₃ (s) = NaF (aq) + H₂O (l) + CO₂ (g)
• Similarly, 2 Na atoms are present on the reactant side while it is 1 on the product side of the reaction.
• So, we multiply the NaF with a coefficient of 2 on the product side so that the number of Na atoms becomes 2 on both sides of the reaction.
• HF (aq) + Na₂CO₃ (s) = 2 NaF (aq) + H₂O (l) + CO₂ (g)
• Finally, the balanced equation is:
• 2 HF (aq) + Na₂CO₃ (s) = 2 NaF (aq) + H₂O (l) + CO₂ (g)

HF + Na₂CO₃ titration

Quantitative estimation of hydrogen fluoride is estimated by performing the titration of HF against a standard solution of Sodium Carbonate.

Apparatus used

A burette, Pipette, measuring flask, glass funnel, clamp stand, measuring cylinder, volumetric flask, and beakers are required for this titration.

Indicator

The methyl orange indicator is used for this titration.

Procedure

• A standard amount of Na₂CO₃ is filled into the burette and noted the initial reading on the burette.
• At the same time, the aqueous solution of HF with the respective indicator methyl orange is taken in a conical flask.
• Then Na₂CO₃ is added dropwise into the conical flask very carefully till the color changes to light pink.
• The constant shaking of the conical flask provides an accurate endpoint. Now note the final reading at the burette.
• The procedure is repeated at least three times until a constant endpoint comes where the indicator changes its color. 
• After the successful titration, the strength of hydrogen fluoride is measured by the formula V₁N₁ = V₂N₂.

HF +Na₂CO₃ net ionic equation

The net ionic equation of HF + Na₂CO₃ is as follows:

2H⁺(aq) + Na₂CO₃ (s) = 2 Na²⁺ (aq) +H₂O (l) + CO₂ (g)

To get the net ionic equation for HF +Na₂CO₃, we should follow the steps given below:

• Write the general balanced molecular equation.
• 2 HF + Na₂CO₃ = 2 NaF + H₂O + CO₂
• Now the solubility equation for HF + Na₂CO₃ is written by labeling the state or phase (s, l, g or aq) of each substance in the balanced molecular equation of HF + Na₂CO₃.
• 2 HF (aq) + Na₂CO₃ (s) = 2 NaF (aq) + H₂O (l) + CO₂ (g)
• Break all aquatic soluble ionic substances into their corresponding ions to get the balanced ionic equation.
• 2H⁺ (aq) +2F^– (aq) + Na₂CO₃ (s) = 2 Na²⁺ (aq) + 2F⁻ (aq) +H₂O (l) + CO₂ (g)
• To get the net ionic equation, remove spectator ions (F^– ) from the reactant and product side of the balanced ionic equation.
• Finally, the net ionic equation for HF + Na₂CO₃ is:
• 2H⁺(aq) + Na₂CO₃ (s) = 2 Na²⁺ (aq) +H₂O (l) + CO₂ (g)

HF + Na₂CO₃ conjugate pairs

The conjugate pairs (compounds differ by one proton in their respective pair) in HF + Na₂CO₃ are:

• The conjugate base of HF acid is F^–.
• The conjugate base of H₂O is OH^–.
• Na₂CO₃, NaF, and CO₂ do not have their conjugate pairs because these compounds do not contain hydrogen atoms that can remove as proton ions.

HF and Na₂CO₃ intermolecular forces

The intermolecular forces that work on HF and Na₂CO₃ are-

• Dipole-dipole force, London dispersion force, and hydrogen bonding are present in HF molecules.
• The electrostatic force of attraction and Coulomb force is present in Na₂CO₃ molecules that held Na⁺ ion to CO₃^2- ions.
• The electrostatic force of attraction and Coulomb force is present in NaF as it is a strong ionic compound.
• Hydrogen bonds, dipole-induced dipole forces, and London dispersion forces exist in water due to their strong polar and ionic nature.
• London dispersion force is the only intermolecular force that is found in the CO₂ molecules because of its extremely low boiling point ( -78.46 °C).

HF + Na₂CO₃ reaction enthalpy

The net enthalpy change of the reaction HF + Na₂CO₃ is -28.60 kJ/mol. The value is gained from the following mathematical calculation.

• ΔH°_f = ΣΔH°_f (products) – ΣΔH°_f (reactants) (kJ/mol)
• ΔH_f = [2*( -495.74) +(-285.83) +(-393.51) -(2* (-255.64) +(-1130.94)] kJ/mol
• ΔH_f = -28.60 kJ/mol

Is HF +Na₂CO₃ a buffer solution

HF + Na₂CO₃ is not a buffer solution because this mixture does not contain the corresponding weak acid (i.e. H₂CO₃) of Na₂CO₃ salt.

Is HF + Na₂CO₃ a complete reaction

HF + Na₂CO₃ is a complete reaction because in this reaction HF and Na₂CO₃ are completely consumed and converted into the final product (NaF) successfully.

Is HF + Na₂CO₃ an exothermic or endothermic reaction

HF+Na₂CO₃ reaction is an exothermic reaction because the net change of enthalpy is negative (i.e., ΔH_f < 0, -28.60 kJ/mol) where the -ve sign interprets the following facts about the reaction:

• 28.60 kJ/mol heat is released by the reactants HF and Na₂CO₃ due to the formation of less energetic salt NaF. 
• Heat emission by HF and Na₂CO₃ rises the energy of surroundings and makes the products stable.

Is HF +Na₂CO₃ a redox reaction

HF +Na₂CO₃ is not a redox reaction as we see the oxidation number of all atoms H, F, Na, C, and O are all the same in reactants and products as well.

Is HF + Na₂CO₃ a precipitation reaction

HF+ Na₂CO₃ is not a precipitation reaction because the completion of the reaction provides the NaF as the main product that is dissolved in reaction media. 

Is HF + Na₂CO₃ reversible or irreversible reaction

HF + Na₂CO₃ is an irreversible reaction because the product NaF and CO₂ are stable so they do not need to react with each other to form reactants back.

Is HF +Na₂CO₃ displacement reaction

HF + Na₂CO₃ is a double displacement reaction because, in this reaction, fluoride ion (F^–) and carbonate ion (CO₃^2- ) exchange their places with each other to form new products, NaF, H₂O, and CO₂.

Conclusion

HF + Na₂CO₃ reaction is carried out through a double displacement reaction in which sodium fluoride and carbonic acid (H₂CO₃) are formed and because carbonic acid is less stable it breaks down into H₂O and carbon dioxide (CO₂). During the whole reaction, net 28. 60 kJ/mol energy is released by reactants.

Kavita Singhal

Hi, I am Kavita Singhal, Ph.D. in Chemical Sciences. My subject area of interest is Physical and Inorganic Chemistry with special emphasis on Electrochemistry, Polymer Chemistry, Nano Chemistry, Corrosion Study, Cyclic voltammetry, Supercapacitance, and Organometallic Chemistry.
I love to bring to my readers the foundational aspects of the subject and my articles are focused on the major areas of chemical sciences in an easy yet informative approach. Looking forward to getting connected through LinkedIn: