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Does silver hydroxide dissociate fully in an aqueous solution?
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Michael Naunton
Does silver hydroxide dissociate fully in an aqueous solution?
I’m not aware that ferric hydroxide will dissolve in strong base, but if it does, my guess would be that a charged coordination complex of some sort is formed in the strong base. I’m sure that the complex would have an overall negative charge and the corresponding cations would be the alkali cation, whatever that may be, eg. Li, Na, K.
I’m not aware that ferric hydroxide will dissolve in strong base, but if it does, my guess would be that a charged coordination complex of some sort is formed in the strong base. I’m sure that the complex would have an overall negative charge and the corresponding cations would be the alkali cation, whatever that may be, eg. Li, Na, K.
Silver hydroxide, AgOH, is formed by dropwise addition of aqueous OH¯ to a solution of Ag⁺ ions;
Ag⁺(aq) + OH¯(aq) → AgOH(s)
However, it quickly dehydrates to form black-brown silver oxide, Ag₂O:
2AgOH(s) → Ag₂O(s) + H₂O(l)
It should be pointed out that the Ag(I) cation is a weak Brønsted acid: this means that AgOH precipitates at relatively high pH and does not dissolve in excess of OH¯ ions. Moreover, owing to the noble character of the metal, AgOH readily forms Ag₂O (rather than dissociating), which is thermodynamically more stable.
Silver hydroxide, AgOH, is formed by dropwise addition of aqueous OH¯ to a solution of Ag⁺ ions;
Ag⁺(aq) + OH¯(aq) → AgOH(s)
However, it quickly dehydrates to form black-brown silver oxide, Ag₂O:
2AgOH(s) → Ag₂O(s) + H₂O(l)
It should be pointed out that the Ag(I) cation is a weak Brønsted acid: this means that AgOH precipitates at relatively high pH and does not dissolve in excess of OH¯ ions. Moreover, owing to the noble character of the metal, AgOH readily forms Ag₂O (rather than dissociating), which is thermodynamically more stable.
I’m not aware that ferric hydroxide will dissolve in strong base, but if it does, my guess would be that a charged coordination complex of some sort is formed in the strong base. I’m sure that the complex would have an overall negative charge and the corresponding cations would be the alkali cation, whatever that may be, eg. Li, Na, K.
I’m not aware that ferric hydroxide will dissolve in strong base, but if it does, my guess would be that a charged coordination complex of some sort is formed in the strong base. I’m sure that the complex would have an overall negative charge and the corresponding cations would be the alkali cation, whatever that may be, eg. Li, Na, K.
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Silver hydroxide, AgOH, is formed by dropwise addition of aqueous OH¯ to a solution of Ag⁺ ions;
Ag⁺(aq) + OH¯(aq) → AgOH(s)
However, it quickly dehydrates to form black-brown silver oxide, Ag₂O:
2AgOH(s) → Ag₂O(s) + H₂O(l)
It should be pointed out that the Ag(I) cation is a weak Brønsted acid: this means that AgOH precipitates at relatively high pH and does not dissolve in excess of OH¯ ions. Moreover, owing to the noble character of the metal, AgOH readily forms Ag₂O (rather than dissociating), which is thermodynamically more stable.
Silver hydroxide, AgOH, is formed by dropwise addition of aqueous OH¯ to a solution of Ag⁺ ions;
Ag⁺(aq) + OH¯(aq) → AgOH(s)
However, it quickly dehydrates to form black-brown silver oxide, Ag₂O:
2AgOH(s) → Ag₂O(s) + H₂O(l)
It should be pointed out that the Ag(I) cation is a weak Brønsted acid: this means that AgOH precipitates at relatively high pH and does not dissolve in excess of OH¯ ions. Moreover, owing to the noble character of the metal, AgOH readily forms Ag₂O (rather than dissociating), which is thermodynamically more stable.
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