15 Facts on HF + K2CO3: What, How To Balance & FAQs

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The HF + K2CO3 is a chemical reaction between a weak acid and a salt. Let us discuss more brief details on HF + K2CO3 reaction.

HF is a weak acid known as hydrofluoric acid or hydrogen fluoride. It is composed of 1 H and 1 F atom. K2CO3 is a chemical formula of potassium carbonate, an inorganic white salt. It is composed of 2 K, 1 C, and 3 O atoms. K2CO3 is a potassium salt of carbonic acid used as a base in various reactions.

Let us learn more details on HF + K2CO3 reaction including the type of reaction, product formation, net ionic equation, balanced equation, titration process, conjugate base, buffer solution, etc. with more various facts and FAQs on it.

What is the product of HF and K2CO3?

The product of the HF + K2CO3 reaction is Carobbiite or potassium fluoride (KF), with the formation of water (H2O) and liberation of carbon dioxide (CO2) gas.

2 HF + K2CO3 → 2 KF + H2O + CO2

What type of reaction is HF + K2CO3?

The HF + K2CO3 reaction is an acid-base neutralization reaction and confirms due to the formation of salt and water.

How to balance HF + K2CO3?

The HF + K2CO3 reaction is balanced with the help of the following steps:

  • The HF + K2CO3 unbalanced reaction is as follows
  • HF + K2CO3 = KF + H2O + CO2
  • In the above equation, both LHS and RHS do not contain the same number of elements
  • First, multiply the HF by 2 on LHS we get
  • 2 HF + K2CO3 = KF + H2O + CO2
  • Second, multiply the KF by 2 on RHS we get
  • 2 HF + K2CO3 = 2 KF + H2O + CO2
  • Now, the above equation contains an equal number of elements on the reactant LHS side and product RHS side of the reaction.

HF + K2CO3 titration

The HF + K2CO3 titration is a weak acid and weak base titration and the Conductometric titration procedure is explained below points.

Apparatus and chemicals:

  • Burette- 10 ml
  • Pipette- 5 ml
  • Stirrer or glass rod
  • Conical flask- 100 ml
  • Burette stand and clamp
  • Beakers- 100 ml
  • Conductometer
  • Conductance cell
  • Hydrofluoric acid (HF)
  • Potassium carbonate (K2CO3)

Principle:

On titration, the ions of acid and base get replaced each other. The ionic conductivity difference of such ions has a direct impact on the electrolytic conductivity of a solution. The values of ionic conductance get vary within cations and anions and also depends on the reaction that occurs in the solution.

Theory:

The end-point of the titration is determined by measuring the conductivity of a solution. As the base is added, the conductivity gets decreases in the solution due to the replacement of H+ ions with the positive part of the base. At the equivalence point, the ion concentration and conductance get increase.

Procedure:

  • Add 10 ml of HF acid in 100 ml of distilled water.
  • Wash the burette with K2CO3 solution and make up the volume of the burette up to the mark with K2CO3 solution.
  • Switch on the conductometer and also the conductance cell.
  • Insert the conductivity cell in the beaker containing the acid solution.
  • Calibrate the conductometer by moving the selector button till the meter screen shows a 1.0 value.
  • First, read the conductance of the blank solution on the conductometer.
  • Add the K2CO3 solution from the burette dropwise to the beaker containing HF acid.
  • Record the K2CO3 volume which is added to the acid solution every time.
  • Record the change in conductance after every addition of K2CO3 solution.
  • A sharp or rapid increase in conductance value confirms the endpoint of the reaction solution, but still, some more readings should be taken and recorded.
  • Finally, the observed values are used to plot a graph. The graph gets plotted against conductance versus the volume of K2CO3.
HF K2CO3
Graph of a weak acid and weak base titration

HF + K2CO3 net ionic equation

The net ionic equation for HF + K2CO3 chemical reaction is 2 H+ (aq) + CO32- (aq) = H2O (l) + CO2 (g).

  • 2 HF (aq) + FeCl2 (aq)  = FeF2 (aq) + 2 HCl (aq)
  • 2 H+ (aq) + 2 F– (aq) + 2 K+ (aq) + CO32- (aq) = 2 K+ (aq) + 2 F– (aq) + H2O (l) + CO2 (g)
  • Here, the K+ and F- ions are spectator ions in this reaction, so cancel out both the ions from RHS and LHS of the reaction we get.
  • 2 H+ (aq) + CO32- (aq) = H2O (l) + CO2 (g)
  • The above reaction is the net ionic equation for the chemical reaction HF + K2CO3.

HF + K2CO3 conjugate pairs

The HF + K2CO3 is a conjugate pair.

  • HF is can act as conjugate acid and F– can act as a conjugate base.
  • The conjugate acid of K2CO3 is KHCO3.

HF + K2CO3 intermolecular forces

The intermolecular force between the HF + K2CO3 is discussed below:

  • HF acid consists of the hydrogen bond intermolecular force as it can donate its proton which is attached with F– by a hydrogen bond.
  • K2CO3 is an ionic moiety, so it has ion-ion interaction between two oppositely charged K+ and CO32- ions.

HF + K2CO3 reaction enthalpy

The reaction enthalpy for HF + K2CO3 chemical reaction is -181.546 kJ/mol.

  • The enthalpy of formation for HF is -272.72 kJ/mol.
  • The enthalpy of formation for K2CO3 is -1151.0 kJ/mol.
  • The enthalpy of formation for KF is -563 kJ/mol.
  • The enthalpy of formation for H2O is -285.7 kJ/mol.
  • The enthalpy of formation for CO2 is -393.474 kJ/mol.
  • The Reaction enthalpy (∆H) of HF + K2CO3 = Enthalpy of product – enthalpy of reactant, we get,
  • (∆H) of HF + K2CO3 is = -1423.72 kJ/mol – (-1242.174) kJ/mol
  • (∆H) of HF + K2CO3 is = -181.546 kJ/mol.

Is HF + K2CO3 a buffer solution?

The HF + K2CO3 is a buffer solution. HF is a weak acid and K2CO3 is a salt of carbonic acid which acts as a weak base in most organic reactions.

Is HF + K2CO3 a complete reaction?

The HF + K2CO3 is a complete reaction because, at the equivalence point in the graph, it shows equilibrium and further reaction is not possible and shows a straight line of the graph. The sharp increase in conductance shows an equivalence point and equilibrium at the reaction.

Is HF + K2CO3 an exothermic or endothermic reaction?

The HF + K2CO3 is an exothermic reaction. There is heat produced during the reaction as HF is a weak acid and K2CO3 is a salt that acts as a weak base. The enthalpy change value for HF + K2CO3 reaction is negative which confirms that it is an exothermic reaction.

Is HF + K2CO3 a redox reaction?

The HF + K2CO3 is not a redox reaction due to the following points.

  • The oxidation number of H and F in HF is +1 and -1.
  • The oxidation number of K, C, and O in K2CO3 is +1, +4, and -2.
  • The oxidation number in K and F in KF is +1 and -1.
  • The oxidation number of H and O in H2O is +1 and -2.
  • The oxidation number of H and O in CO2 is +4 and -2.
  • From the above values of oxidation numbers of reactants and products of HF + K2CO3 reaction, it is clear that there is no change in oxidation number.
  • The oxidation number of the reactant and product is the same in HF + K2CO3 reaction, so it is not a redox reaction.

Is HF + K2CO3 a precipitation reaction?

The HF + K2CO3 is a precipitation reaction. In this reaction, when HF is reacted with K2CO3, there is a formation of precipitates of a white color crystalline solid compound known as KF. The KF is a fluoride salt formed as a white solid precipitate in this reaction.

Is HF + K2CO3 reversible or irreversible reaction?

The HF + K2CO3 shows an irreversible reaction because in this reaction, the reactants HF and K2CO3 can form products KF, H2O, and CO2 but these products are not able to form the same reactants as a product again when gets reacted with each other.

Is HF + K2CO3 displacement reaction?

The HF + K2CO3 reaction is not a displacement reaction. It is an acid-base neutralization reaction. In this reaction, the oppositely charged ion of HF and K2CO3 does not get displaced with each other during the product formation.

Conclusion:

The HF + K2CO3 reaction has products KF, H2O, and CO2. It is an acid-base neutralization reaction. The reaction enthalpy for HF + K2CO3 reaction is -181.546 kJ/mol. It can form a buffer solution. It is a complete, precipitation, exothermic, and irreversible reaction.