Table of contents


What Solutions Neutralize Barium Hydroxide?


An acid-base reaction that forms salt and water as products is called a neutralization reaction. The acids and bases that are involved in the reaction may be strong or weak. Depending on the strength of reactants, the reaction can be classified as a strong acid-strong base, weak acid-strong base, strong acid-weak base, and weak acid-weak base. The pH of the resultant salt also varies on the strength of the parent acid and base.

If you are looking for different neutralization reactions of barium hydroxide, then you are on the right page.

What Solutions Neutralize Barium Hydroxide?

Usually, the mineral acids are used to neutralize barium hydroxide. We know that barium hydroxide is a strong base so we can prepare the desired salt by using different acids. In the laboratory, the neutralization reaction is carried out by titration techniques. Titration techniques are used to determine the unknown concentration of an acid or a base. Now let us see how different acids neutralize barium hydroxide.

1. Neutralization with Hydrochloric Acid

HCl is the most commonly used acid for neutralization reactions. Barium hydroxide gives two moles of hydroxide ions in the solution so we use two moles of hydrochloric acid to carry out the reaction.

Ba(OH)2 + 2HCl➞BaCl2 + H2O

Both the barium hydroxide and hydrochloric acid are strong so the pH of the resulting salt is seven (neutral). Barium chloride is commercially prepared using this method. It is an industrially important salt.

2. Neutralization with Phosphoric Acid

The phosphoric acid also neutralizes the barium hydroxide. Phosphoric acid is a weak acid so the pH of the resulting salt would be less than seven (acidic). The neutralization reaction involves three moles of barium hydroxide and two moles of phosphoric acid.

3Ba(OH)2 + 2H3 PO4➞Ba3 (PO4 )2 + 6H2 O

Barium phosphate is also an important salt that is prepared by this method. Barium phosphate is an insoluble salt so it is precipitated out at the end of the reaction.

3. Neutralization with Carbonic Acid

Carbonic acid is also a weak acid and it neutralizes the barium hydroxide to form barium carbonate. The pH of barium carbonate is also less than seven (acidic). One mole of barium hydroxide reacts with one mole of carbonic acid. Following is the reaction equation

Ba(OH)2 + H2CO3➞BaCO3 + 2H2 O

One mole of barium carbonate and two moles of water are formed as the product. Barium carbonate is insoluble in the solution so it can easily be precipitated out of the solution.

4. Neutralization with Acetic Acid

Acetic acid is a weak organic acid and it forms an acidic salt with barium hydroxide. Two moles of acetic acid are used to neutralize one mole of barium hydroxide. The resulting salt is barium acetate.

Ba(OH)2 + 2CH3 COOH➞Ba(CH3 COO-) + 2H2 O

5. Neutralization with Nitric Acid

Nitric acid is a strong acid and it forms the neutral salt upon reacting with barium hydroxide. Two moles of nitric acid neutralize the one mole of barium hydroxide. The resulting salt is barium nitrate which is soluble in an aqueous solution. Thus, the neutralization solution of barium hydroxide and nitric acid is the clear solution. The reaction equation is given below

Ba(OH)2 + 2HNO3➞Ba(NO3)2 + 2H2O

Barium nitrate is used in the making of signal lights, ceramics, paints, and as an oxidizing agent.

Frequently asked questions

Q 1: What are the uses of Barium Carbonate?

Ans: Barium carbonate is used in the manufacturing of glass, photographic films, brick, and oil drilling.

Q 2: Which is the Best Acid to Neutralize Barium Hydroxide?

Ans:According to literature, weak acids are best for the neutralization of strong bases. So weak mineral acids are best to neutralize the barium hydroxide. But in the laboratory, HCl is easily available so HCl may also be used commonly to neutralize barium hydroxide.

Q 3: What are the Applications of a Neutralization Reaction?

Ans:Following are the common applications of neutralization reaction

  • Acid-base titrations
  • Wastewater treatment
  • Maintaining the pH of soil
  • Treatment of acidity in the human body
  • Treatment of mouth cavities