Diagonal relationship - Wikipedia
By definition, a common ion is an ion that enters the solution from two different The Inverse Relationship Between the Equilibrium Concentrations of the Cr3+. Solubility is defined as the maximum amount of solute that can be is important when describing the solubility of slightly ionic compounds. Explain solid/solution equilibria using Ksp and Qsp. Formations of precipitates are chemical equilibria phenomena, and we usually write these heterogeneous Thus, the relationship among Qsp, Ksp and saturation is given below.
With lithium salts there is evidence to show that both inner-sphere and outer-sphere complexes exist in liquid-ammonia solutions. In this solvent ion association is the rule rather than the exception. Indeed, higher associates such as tetramers are often formed. In this case it also helps that the surface of the cation is hydrophobic.
In SN1 reactions the carbocation intermediate may form an ion pair with an anion, particularly in solvents of low dielectric constant, such as diethylether. Characterization[ edit ] Vibrational spectroscopy provides the most widely used means for characterizing ion associates.
Both infrared spectroscopy and Raman spectroscopy have been used. The anion vibration frequency is "shifted" on formation of ion pairs and other associates, and the extent of the shift gives information about the nature of the species. Other monovalent anions that have been studied include nitratenitrite and azide. Ion pairs of monatomic anions, such as halide ions, cannot be studied by this technique.
Ka is equal to 2.
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That's our answer, 2. Let's go a little further. Let's take our equation here, Ka times Kb is equal to Kw. Let's take the log of both sides. That would be the log of Ka times Kb is equal to the log of Kw. If we take the negative of everything, let's go ahead and do that, the negative of everything, negative log of Ka.What's an Ion?
I'll put that in parenthesis, plus the negative log of Kb is equal to the negative log of Kw. The negative log of Ka, we know that this is equal to the pKa.
The negative log of Ka was our definition for our pKa, and the negative log of Kb was our definition for pKb. That would give you The negative log of 1.
Now we have something else that we can work with, so let me go ahead and box this right here. Let's take the Ka value that we just found. Let's find the pKa. The pKa would be equal to the negative log of 2. Let's do that on our calculator here. Let's get some room. The negative log of 2. We have to round that.
These are our two significant figures because we have two significant figures here. Let's go back up to our problem here, so that's the pKa for the methylammonium ion. Let's say you're given the pKa for the methylammonium ion and asked for the pKb for methylamine. What is the pKb for methylamine?
All we have to do is plug in to our equation. Let's go ahead and write that in here. When we solve for the pKb that would give us 3.
So the pKb is equal to 3. We could double-check that. Let's go back up here and we could double-check that, because if we took the negative log of this number that's what we should get. Let's take the negative log of 3. That's what we just calculated down here.
The pKb is equal to 3. That's the relationship between Ka and Kb, and you can also talk about the relationship between pKa and pKb.
These are called diagonal relationships. It is not as noticeable after B and Si. The reasons for the existence of diagonal relationships are not fully understood, but charge density is a factor.
Using the Li—Mg pair: Li is the only Group 1 element which forms a stable nitride, Li3N. The corresponding Group 2 salts are insoluble. Think lattice and solvation energies. Both Li and Mg form covalent organometallic compounds.