Barium hydroxide

Description

Barium Hydroxide occurs as an anhydrate whose prismatic, colorless crystals are very deliquescent. Barium hydroxide can be prepared by dissolving barium oxide (BaO) in water:
BaO＋ 9H2O→Ba(OH)2·8H2O
It crystallizes as the octahydrate, which converts to the monohydrate upon heating in air. Barium oxide has been found to react with water vapor at temperatures from 1443 to 1593 K to form gaseous Ba(OH)2 according to the reaction:
BaO(solid)＋H2O(gas)→Ba(OH)2(gas)
A better method of preparation involves addition of NaOH to the nitrate. Since barium hydroxide is fairly soluble, it is necessary to evaporate the solution to crystallize Ba(OH)2·8H2O. Ethanol is added to aid in this crystallization. The crystals are washed in cold ethanol to remove sodium ions and then dried.

Description

The octahydrate of barium hydroxide is freely soluble in water and MeOH, whereas the monohydrate is only slightly soluble in water. For this reason the octahydrate is the most common form.

Chemical properties

Barium hydroxide,Ba(OH)2·8H20, is a white crystalline powder, colorless solid composed of monoclinic crystals. It has a melting point of 78°C and is soluble in water and insoluble in acetone. It is used in the fusion of silicates and fat saponification.

Physical properties

Monohydrate, Ba(OH)₂?H₂O is a white powder; density 3.743 g/cm³; slightly soluble in water; soluble in dilute mineral acids. Octahydrate, Ba(OH)₂?8H₂O is a colorless monoclinic crystal; density 2.18 g/cm³ at 16°C; refractive index 1.50; melts at 78°C; vapor pressure 227 torr; loses seven molecules of water of crystallization when its solution is boiled in the absence of atmospheric CO₂ forming solid monohydrate; further heating produces anhydrous Ba(OH)₂ melting at 407°C; readily dissolves in water (3.76 g/100 g at 20°C and 11.7 g/100 g at 50°C); aqueous solution highly alkaline; also soluble in methanol; slightly soluble in ethanol; insoluble in acetone.

The Uses of Barium hydroxide

Barium hydroxide is used in analytical chemistry to titrate weak acids, particularly organic acids. It forms clear aqueous solutions that are free from carbonate, unlike those of the alkali hydroxides, since barium carbonate is insoluble in water. This allows the use of indicators such as phenolphthalein or thymophthalein (with alkaline color changes) without the risk of titration errors due to the presence of weakly basic CO3^2- ions.Barium hydroxide is used in organic synthesis as a strong base, for example for the hydrolysis of esters and nitriles.It has been used to hydrolyze one of the two equivalent ester groups in dimethyl endecanedioate. It is also used in the preparation of cyclopentanone, diacetone alcohol and d-Gluonic g-lactone.
Barium hydroxide is used as an additive in thermoplastics (such as phenolic resins), rayon and PVC stabilizers to improve plastic properties. This material is used as a general-purpose additive for lubricants and greases. Other industrial applications for barium hydroxide include sugar fabrication, manufacturing soaps, fat saponification, fusing of silicates and chemical synthesis of other barium compounds and organic compounds.
Barium hydroxide is offered for sale both as the octahydrate and the monohydrate. It is available in large quantities commercially.

The Uses of Barium hydroxide

To a solution of KOH (10 g, 178 mmol) in H2O (15 mL) and EtOH (15 mL) at RT was added the SM (3.92 g, 42 mmol) over 10 min. The reaction mixture was stirred at 90 C for 3.5 h, after which time it was concentrated in vacuo. The resulting residue was dissolved in H2O (10 mL) and acidified at 0 C with 6M HCl to pH 1. The mixture was extracted with DCM. The org layer was dried (MgSO4) and concentrated to provide the product as a colorless oil which was taken forward without further purification. [4.65 g, 98%]

The Uses of Barium hydroxide

Carbon dioxide absorbant.

The Uses of Barium hydroxide

Bariium hydroxide is used as a precursor to other barium compounds. It is used in analytical chemistry for titration of weak acids, particularly organic acids. It removes the carbonate in water. It is a strong base, and is used as catalyst in many organic reactions, such as hydrolysis of esters and nitriles, decarboxylation of amino acids, selective hydrolysis of one of the ester groups in dimethyl hendecanedioate, and preparation of cyclopentanone, diacetone alcohol and D-Gulonic gamma-lactone.

Preparation

Barium hydroxide is made by dissolving barium oxide in hot water. The octahydrate, Ba(OH)₂?8H₂O, crystallizes upon cooling. It also is prepared by precipitation with caustic soda from an aqueous solution of barium sulfide:
BaS + 2NaOH → Ba(OH)₂ + Na₂S.

Hazard

An acute poison; toxic symptoms are similar to other soluble salts of barium (see Barium).

Flammability and Explosibility

Not classified

Safety Profile

A poison by ingestion andintraperitoneal routes. Incompatible with chlorinated rubber.