Solution of Barium Hydroxide Preparation, Formula, and Molar Mass

Barium hydroxide is a chemical compound with the chemical formula Ba(OH)2. It is solid with a white color and crystalline structure. This substance easily dissolves in water, creating a powerful alkaline solution. Known for its strong base properties, barium hydroxide readily reacts with acids to produce barium salts.

Molar Mass

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The molar mass of barium hydroxide is calculated by adding the atomic masses of its constituent atoms. The atomic masses of barium (Ba), oxygen (O), and hydrogen (H) are 137.33 g/mol, 15.99 g/mol, and 1.01 g/mol, respectively. 

Barium Hydroxide Chemical Formula and Molar Mass

Ba(OH)2 = 1(BA) + 2(O) + 2(H)

\[= 137.33 g/mol + 2(15.99 g/mol) + 2(1.01 g/mol)\]

\[= 171.34 g/mol\]

The molar mass of barium hydroxide is 171.34 g/mol.

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Preparation of 0.2N Barium Hydroxide Solution

Take 63gm of Ba(OH)2.8H2O to make a 0.2 M solution. 

Take a clean and dry volumetric flask add barium hydroxide, add a small amount of distilled water, and mix proper dissolved barium hydroxide.

Add more distilled water to the flask to bring the volume up to the mark on the flask.

Cover the flask with a stopper fitted with a guard tube. So that the guard fills the tube with soda lime or ascarid to remove the air and carbon dioxide entering the flask.

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The solution is filtered through a filter paper to remove any insoluble impurities, such as BaCO3.

Transfer the molar solution to a bottle and the solution bottle is tightly sealed to prevent exposure to carbon dioxide in the air.

NOTE: Please ensure that you handle barium hydroxide with caution, as it is a potent base that can lead to burns and is harmful if ingested or inhaled. Remember to wear appropriate protective gear like gloves and goggles, and always work in a well-ventilated space.

Calculate the pH of a 0.10 m solution of barium hydroxide, Ba(OH)2.

Barium hydroxide (Ba(OH)2) is a strong base that readily dissociates in water to form Ba2+ and OH- ions. 

To calculate the pH of a 0.10 M solution of Ba(OH)2, we need to determine the concentration of hydroxide ions (OH-) in the solution.

Ba(OH)2 → Ba2+ + 2OH-

Ba(OH)2 dissociates completely, and the concentration of OH- ions is twice the concentration of Ba(OH)2:

[OH-] = 2 × [Ba(OH)2]

= 2 × 0.10 m

= 0.20m

Use this formula to know pH:

pH = -log [H+]

pOH is calculated as follows:

pOH = -log [OH-]

= -log(0.20)

= 0.70

Since pH + pOH = 14, 

pH = 14 - pOH

= 14 - 0.70

= 13.3

Therefore, the pH of a 0.10 M solution of barium hydroxide is 13.3.

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