15 Facts on HBr + BaCO3: What, How To Balance & FAQs

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HBr is an inorganic acid, whereas BaCO3 is an alkali metal carbonate. Let us analyze the interactions between these two substances.

BaCO3, a white powdered solid basic salt, and HBr, a colorless, powerful mineral acid, interact to generate a salt and acid first. The acid product instantly breaks down into a liquid and a gas.

This article will provide some insight into all the critical aspects of the reaction between HBr and BaCO3.

What is the product of HBr and BaCO3?

The end products of the reaction of HBr and BaCO3 are barium bromide (BaBr2), carbon dioxide (CO2), and water (H2O). Unstable carbonic acid (H2CO3) easily breaks down into water and carbon dioxide. The outcome is depicted below. 

HBr + BaCO3 → BaBr2 +H2CO3 → H2O + CO2

What type of reaction is HBr + BaCO3?

HBr and BaCO3 react with each other to form salt and lie under a double displacement reaction.

How to balance HBr + BaCO3?

The imbalanced equation for the HBr + BaCO3 is given below

HBr + BaCO3 → BaBr2 + CO2 + H2O

1.On the product and reactant sides, the total number of atoms in each element must be matched.

2. In this specified equation, Ba, C, and O atoms on the equation’s reactant- side should be equal to the product- side.

3. HBr + BaCO3 → BaBr2 + CO2 + H2O

4. H and Br atom numbers should also be matched on both sides of the equation, as they are not equal. H= 1, Br= 2

5. HBr+ BaCO3 → BaBr2 + CO2 + H2O

6. To match the H and Br atom numbers, HBr will be multiplied by the number 2.

7. The balanced equation is, finally, as follows.

2HBr + BaCO3 → BaBr2 + CO2 + H2O

HBr + BaCO3 titration

Back titration is required to calculate the concentration of the insoluble salt BaCO3 in HBr.

Apparatus

Burette, pipette, distilled water, conical flask, burette holder, volumetric flask, beakers, stirrer, and wash bottle.

Indicator

Acid-base indicator phenolphthalein is used to identify the titration’s end point.

Procedure

  • Using a pipette, HBr (determined volume and concentration) was introduced to a conical flask containing a solution of BaCO3.
  • Add a few indicator drops after thoroughly mixing the mixture.
  • Titrate the extra HBr until the color turns light pink by adding known concentrations of NaOH solution from a burette.
  • To confirm the precision and record the burette analysis, repeat the procedure 2 to 3 times.
  • The quantity of unreacted HBr can then be calculated using the equation S1V1 = S2V2.
  • It is possible to calculate the amount of BaCO3 from the amount of HBr that interacted with it.

HBr + BaCO3 net ionic equation

HBr + BaCO3‘s net ionic equation is -.

CO32− (aq) + 2H+ (aq) → H2O (l) + CO2 (g)

  • Ionic substances that are soluble can separate into cations and anions.
  • Ionic substances like HBr, BaCO3, and BaBr2 can be represented as cations and anions.
  • 2H+ (aq) + 2Br− (aq) + Ba2+ (aq) + CO32− (aq) → Ba2+ (aq) + 2Br− (aq) + H2O (l) + CO2 (g)
  • Finally, we can obtain the net ionic equation by canceling the spectator ions through both ends.

HBr + BaCO3 conjugate pairs

HBr+ BaCO3 has the following conjugate pairs,

  • No conjugate pair is possible for the BaCO3 base.

HBr + BaCO3 intermolecular forces

HBr+ BaCO3 has the following intermolecular forces,

  • Dipole-dipole and London dispersion forces are the two intermolecular interactions present in the HBr molecule. Due to its polar nature, dipole-dipole interaction is more significant.
  • Ionic in nature, BaCO3 exhibits electrostatic attraction.

HBr + BaCO3 reaction enthalpy

For the reaction of HBr and BaCO3, the reaction enthalpy value is -2.4 kJ/mole. The calculation is listed below.

  • Reaction Enthalpy = (enthalpies of formation of all products) – (enthalpies of formation of all reactants)
  • Reaction enthalpy = (ΔHf of BaBr2 + ΔHf of CO2 + ΔHf of H2O)- (ΔHf of 2HBr + ΔHf of BaCO3)
CompoundsΔHf
HBr (aq)-125.6 kJ/mol
BaCO3 (aq)-1202.2 kJ/mol
H2O (aq)-285.8 kJ/mol
CO2 (g)-393.5 kJ/mol
BaBr2 (aq)-364.9 kJ/mol
Reaction Enthalpy
  • Reaction enthalpy = [(-364.9) + (-393.5) +(-285.8)] – [2*(-125.6) -1202.2) = -2.4 kJ/mol

Is HBr + BaCO3 a buffer solution?

HBr is a potent acid and BaCO3 lacks the conjugate base of HBr, the combination of HBr and BaCO3 cannot result in a buffer solution.

Is HBr + BaCO3 a complete reaction?

HBr + BaCO3 is a complete reaction because the acid HBr and salt BaCO3 totally react with one another.

Is HBr + BaCO3 an exothermic or endothermic reaction?

HBr + BaCO3 is exothermic in nature as the computation of the reaction’s enthalpy, which came out to be -2.4 kJ/mole is negative.

Is HBr + BaCO3 a redox reaction?

HBr + BaCO3 cannot be referred to as a redox process since the oxidation states of the atoms in the reactant and product molecules are unaltered.

Is HBr + BaCO3 a precipitation reaction?

HBr + BaCO3 cannot be referred to as a precipitation reaction since the resultant BaBr2 is a solid that dissolves in water while CO2 and H2O are gas and liquid respectively.

Is HBr + BaCO3 reversible or irreversible reaction?

HBr + BaCO3 can be referred to as an irreversible reaction as the reaction does not shift back to the left after the formation of the products.

Is HBr + BaCO3 a displacement reaction?

HBr + BaCO3 can be referred to as a displacement reaction since ions are exchanged between the two reactants, BaCO3 and HBr.

Conclusion

To conclude interaction between a mineral acid HBr and a white powdered basic salt BaCO3 is a double displacement, an irreversible reaction which on interaction forms water-soluble solid BaBr2, CO2 gas, and H2O. It gives a negative reaction enthalpy and hence is exothermic in nature.

     

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