15 Facts on HBr+Na2CO3: What, How to Balance & FAQs

Hydrobromide acid reacts with washing soda evolves formation of gas, and forms bromide salt of sodium. Let us study the reaction of HBr + Na2CO3 in detail.

Sodium bicarbonate is a white, water soluble, odorless salts which yields moderate alkaline solutions in water. It is produced via Solvay process, from sodium chloride and limestone. Hydrobromic acid is a strong colorless acid, usually used as a catalyst, in the production of bromide compounds.

The following article studies the various fact of HBr + Na2CO3 reactions like the , product, enthalpy of the reaction, exothermic and endothermic behavior, conjugate pairs, reaction type, ionic equation, etc.

What is the product of HBr + Na2CO3?

Hydrobromic acid (HBr) reacts with sodium bicarbonate (Na2CO3) to form sulphuric sodium bromide (NaBr), water (H2O) and carbon dioxide (CO2).

Na2CO3 + HBr → NaBr + H2O + CO2       

What type of reaction is HBr + Na2CO3?

HBr + Na2CO3 is an acid base, precipitate reaction, and exothermic reaction.

How to balance HBr + Na2CO3?

The given HBr + Na2CO3 chemical reaction can be balanced by following steps:

  • Write down the unbalanced chemical reaction as show below:
  • Na2CO3 + HBr → NaBr + H2O + CO2
  • Tabulate down the number of moles of each element present in the reactant and product side as shown below:
ElementsReactant SideProduct Side
Na21
Br11
C11
O33
H12
Number of moles on the reactant and product side
  • The given HBr + Na2CO3 chemical reaction is balanced when the number of moles of each element on the reactant side is equal to the number of moles of each element on the product side.
  • Here moles of Na and H are unbalanced on either side.
  • To balance the reaction, multiply 2 each with HBr on the reactant side and NaBr on the product side.
  • The Balanced chemical reaction is
  • Na2CO3 + 2HBr → 2NaBr + H2O + CO2
Capture 3
Balanced Chemical Reaction

HBr + Na2CO3 Titration

HBr + Na2CO3 is an acid base titration.

Apparatus

Burette, Pipette, Conical flask, Burette stand, Funnel, Stirrer, White glazed tile, Measuring flask, Watch glass.

Indicator

Methyl orange

Procedure

  1. Thoroughly wash, rinse and clean the burette and fill it with M/10 Na2CO3 solution. Note down the initial reading.
  2. Using a pipette, transfer 10 cm3 of HBr solution into a thoroughly cleaned and washed titration flask.
  3. Add 2 to 3 drops of titrating indicator: Methyl orange
  4. Slowly drop by drop add the M/10 sodium carbonate to the titration flask, until the color changes to light pink.
  5. Note down the final reading.
  6. Calculate the amount of sodium carbonate solution used to neutralize the HBr solution
  7. (Na2CO3) a1M1V1 = (HBr) a2M2V2
  8. Strength (g/L) = M2 * 36.5   

HBr + Na2CO3 Net ionic equation

The net ionic equation for HBr + Na2CO3 is: CO32-(aq) + 2H+(aq) = H2O(l) + CO2(g)

  1. Determine each substance’s state or phase (gas = g, liquid = l, solid/non-soluble = s, and aqueous/soluble = aq).
  2. The complete ionic equation is written by separating each ionic compounds into respective ion, as shown below:
  3. 2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Br(aq) = 2Na+(aq) + 2Br(aq) + H2O(l) + CO2(g).
  4. The net ionic equation is written by cancelling out the ions which occurs in both reactant and product side of the complete ionic equation.
  5. 2Na+(aq) + CO32-(aq) + 2H+(aq) + 2Br(aq) = 2Na+(aq) + 2Br(aq) + H2O(l) + CO2(g).
  6. The net ionic equation is: CO32-(aq) + 2H+(aq) = H2O(l) + CO2(g)

HBr + Na2CO3 conjugate pairs

The conjugate acid-base pairs for HBr + Na2CO3 are

  • Conjugate acid of HBr =  HBr+
  • Conjugate base of HBr  = Br 
  • Conjugate acid of the base Na2CO= HCO3

HBr + Na2CO3 intermolecular forces

The intermolecular forces on HBr and Na2CO3 are-

HBr + Na2CO3 reaction enthalpy

The change in reaction enthalpy for HBr + Na2CO3 is: -154.06 kJ/mol

To calculate the change in reaction enthalpy follow the below steps –

  • The enthalpy of formation of each compound on reactant and product side is tabulated down as:
CompoundsEnthalpy (kJ/mol)
Na2CO3-1130.9
HBr72.46
NaBr-722.12
H2O-241.8
CO2-393.5
Enthalpies of each compounds in the reaction
  • Change in reaction enthalpy = Summation of enthalpies on the product side – the summation of enthalpies on the reactant side.
  • Change in Enthalpy  =  (-722.12-241.8-393.5) – (-1130.9-75.46)  = -154.06 kJ/mol

Is HBr + Na2CO3 a buffer solution?

HBr + Na2CO3 reaction is not a buffer solution since presence of strong HBracid taking place during the reaction.

Is HBr + Na2CO3 a complete reaction?

HBr + Na2CO3 is described as a complete reaction as complete moles of reactant are consumed and converted to form respective products at equilibrium, and no further reaction is possible.

Is HBr + Na2CO3 an exothermic or endothermic reaction?

HBr + Na2CO3 is an exothermic reaction because the change in reaction enthalpy is -154.06 kJ/mol, which is negative, which decreases the temperature.

Is HBr + Na2CO3 a redox reaction?

HBr + Na2CO3 is not a redox reaction since the oxidation state of elements remains unchanged throughout the reaction.

Is HBr + Na2CO3 a precipitation reaction?

HBr + Na2CO3 is a precipitation reaction since the formation of inorganic sodium salt NaBr takes place in the reaction.

Is HBr + Na2CO3 irreversible or irreversible reaction?

HBr + Na2CO3 is an irreversible reaction, and can only be reversed when there is a drastic change in experiment pressure or experiment temperature.

Is HBr + Na2CO3 displacement reaction?

HBr + Na2CO3 is not a displacement reaction as both the reactant reacts to from three new products, not by displacing elements with each other.

Conclusion

The reaction of sodium bicarbonate with Hydrobromic acid involves the formation of inorganic sodium salt along with liquid water and carbon dioxide gas. This is an exothermic, precipitate reaction. Sodium bromide is an important industrial chemical, and is mostly used as catalyst in TEMPO-mediated oxidation reactions.