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Caesium hydroxide is a strong base (pK a = 15.76) containing the highly reactive alkali metal caesium, much like the other alkali metal hydroxides such as sodium hydroxide and potassium hydroxide. It is the strongest of the five alkali metal hydroxides. [7]
A strong base is a basic chemical compound that can remove a proton (H +) from (or deprotonate) a molecule of even a very weak acid (such as water) in an acid–base reaction. Common examples of strong bases include hydroxides of alkali metals and alkaline earth metals, like NaOH and Ca(OH) 2, respectively. Due to their low solubility, some ...
All alkali metal hydroxides are strong bases, meaning that they dissociate completely in solution to give OH − ions. As strong bases, alkali hydroxides are highly corrosive and are used in cleaning products. Sodium hydroxide is readily available in most hardware stores in products such as a drain cleaner. Similarly, potassium hydroxide is ...
In chemistry, metal hydroxides are a family of compounds of the form M n+ (OH) n, where M is a metal.They consist of hydroxide (OH −) anions and metallic cations, [1] and are often strong bases.
In chemistry, a strong electrolyte is a solute that completely, or almost completely, ionizes or dissociates in a solution. These ions are good conductors of electric current in the solution. Originally, a "strong electrolyte" was defined as a chemical compound that, when in aqueous solution , is a good conductor of electricity.
Caesium hydroxide is a very strong base, and will rapidly corrode glass. [18] The isotopes 134 and 137 are present in the biosphere in small amounts from human activities, differing by location. Radiocaesium does not accumulate in the body as readily as other fission products (such as radioiodine and radiostrontium).
Its conjugate base is the acetate ion with K b = 10 −14 /K a = 5.7 x 10 −10 (from the relationship K a × K b = 10 −14), which certainly does not correspond to a strong base. The conjugate of a weak acid is often a weak base and vice versa.
csoh + hf → csf + h 2 o Using the same reaction, another way to create caesium fluoride is to treat caesium carbonate (Cs 2 CO 3 ) with hydrofluoric acid and again, the resulting salt can then be purified by recrystallization.