Barium hydroxide is a chemical compound with the chemical formula Ba(OH)2. It is a white colored crystalline solid which is highly soluble in water and forms a strong alkaline solution. Barium hydroxide is a strong base and reacts with acids to form barium salts.
It is commonly used in the production of chemicals containing barium, such as barium titanate and barium carbonate, and is also used in the manufacture of soaps and lubricants. Barium hydroxide is toxic, so it must be handled with care and protective equipment must be worn when working with it.
Barium Hydroxide Chemical Formula and Molar Mass
The chemical formula for barium hydroxide is Ba(OH)2. The 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. Therefore, the mass of barium hydroxide is.
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
So the molar mass of barium hydroxide is 171.34 g/mol.
Preparation of 0.2N Barium Hydroxide Solution
Weigh the accurate 63gm of Ba(OH)2.8H2O to make a 0.2 M solution.
Take clean and dry volumetric flask add barium Hydroxide and littel ammount of distilled water and mix proper dissolved of 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.
The solution is filtered through a filter paper to remove any insoluble impurities, such as BaCO3.
Solution bottle the solution bottle is tightly sealed to prevent exposure to carbon dioxide in the air.
NOTE: Barium hydroxide must be handled with care, as it is a strong base that can cause burns and is toxic if swallowed or inhaled. Use proper protective equipment, such as gloves and goggles, and work in a well-ventilated area.
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-
Since Ba(OH)2 dissociates completely, 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 for 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.
