Enter the Ksp expression for the solid AB2 in terms of the molar solubility x. AB2 has a molar solubility of 3.72×10−4 M. What i
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Answer:
NH3 —> base
We will see ammonia attach itself to silver and not the other way around, silver therefore accepts electrons. So, silver is a Lewis acid and ammonia is a Lewis base, so this reaction is complex as ammonia reacts with the silver cation .
Any group that contains an empty orbital in its valence shell can be considered a Lewis acid, but the bases do not differ in the Brønsted system from those in the Lewis system. Thus, acids are divided into types, including:
Simple Cations
Theoretically, they can be considered as acids and therefore we can also expect their acidic strength to increase for the following reasons:
1. By increasing the positive charge on the cation.
2. Increasing the charge of the nucleus from one atom to another in any period in the periodic table.
3. By decreasing the radius of the cation.
4. Decrease in the number of electron shells in the cation.
Therefore, the acidity of cations of any chain of transition elements increases with increasing atomic number when their positive charge is equal. There are some examples that show the reaction of cations as Lewis acids:
A) the reaction of the silver ion with ammonia
b) aluminum ion hydration
c) Adding alcohol to the lithium ion
D) formation of a ferric cyanide ion
I hope I helped you^_^
