Why does solubility increases down the group?
Since the lattice enthalpy decreases much more rapidly than the hydration enthalpy with increasing ionic size , the solubility of the metal hydroxides increases as we move down the group .
Why does solubility of alkaline earth metal hydroxides increases down the group?
Solution : Among alkaline earth metal hydroxides, the anion being common, the cationic radius will influence the lattice enthalpy. Since lattice enthalpy decreases much more than the hydration enthalpy with increasing ionic size, the solubility increases as we go down the group.
Why does solubility of group 2 carbonates decrease down the group?
Since the hydration enthalpies decrease as the size of the cation increases down the group , the solubility of carbonates and sulphates of alkaline earth metals decreases down the group .
What determines the solubility of hydroxides?
Since the hydroxide concentration, [OH−], is an integrated property of the solution, the solubility of metal hydroxide depends on pH, pOH or [OH−]. Alkali metal hydroxides LiOH, NaOH, KOH, CsOH are soluble, and their solutions are basic. Hydroxides of alkali earth metals are much less soluble.
Why does the thermal stability of hydroxides increase down the group?
In the periodic table, as we go down in the group the lattice enthalpy increases, which leads to an increase in thermal stability of the hydroxide.
Why does solubility of alkaline earth metal hydroxides increases down the group while the solubility of alkaline earth metal carbonates decreases down the group?
Among alkaline earth metal hydroxides, the anion being common, the cationic radius will influence the lattice enthalpy. Since lattice enthalpy decreases much more than the hydration enthalpy with increasing ionic size, the solubility increases down the group `(darr)`.
Why some hydroxides are insoluble in water?
The insolubility of the hydroxides of the transition metals can be explained both by the increasingly large ionization energies that result from successively removing electrons (or negatively charged hydroxide molecules in this case) from the metal cation, and the greater effective nuclear charge on the electrons …
What can be said about the solubility of hydroxides?
The hydroxides of sodium, potassium, and ammonium are very soluble in water. The hydroxides of calcium and barium are moderately soluble. The oxides and hydroxides of all other metals are insoluble.
How thermal stability increases down the group?
Detailed Solution
All the alkaline earth metals form carbonates. All these carbonates decompose on heating CO3 and metal oxides. Therefore, the thermal stability of these carbonates increases down the group. In the 2nd group carbonates, thermal stability increases down the group due to increases in lattice energy.
What is the decreasing order of basicity of hydroxides of the alkaline earth metals?
th eorder is Cs > Rb > Na > Li.
Why is Koh more soluble than NaOH?
KOH has a greater ionic character than NaOH and hence needs a more polar solvent to get dissolved as compared to the equivalent amount of NaOH needs to be.
Why does thermal stability increase down Group 2 hydroxides?
As you go down the group the O-H is less polarised by the larger group 2 cations with a lower charge density so the thermal stability increases.
Why does thermal stability increase down Group 2?
The thermal stability increases as you go down Group 2. This is because the Group 2 ion has lower charge density, and thus distorts the carbonate ion less. The less distorted the carbonate ion is, the more stable it is, and so a higher temperature is required to decompose the carbonate.
Why does the basic strength of hydroxide increase down the group?
1 Answer. Basic strength of alkaline earth metal hydroxides increases down the group because ionization energy of metal decreases and electropositive character increases down the group.
What is the trend of solubility in group 2?
Group II metal hydroxides become more soluble in water as you go down the column. This trend can be explained by the decrease in the lattice energy of the hydroxide salt and by the increase in the coordination number of the metal ion as you go down the column.
Why is NaOH the strongest base?
NaOH dissociates completely in water to give Na+ and OH− . It is considered as a strong base because all the available [OH] in NaOH is present in solution as [OH−] and available to accept protons.
Why potassium hydroxide is more soluble in water?
KOH is hygroscopic and very easily soluble in water. The aqueous solution reacts strongly alkaline and is called potassium hydroxide solution (KOH). Due to the exothermic reaction of the hydrate formation, the dissolution in water takes place with strong generation of heat. Was this answer helpful?
Which Group 2 hydroxide is the most soluble in water?
In alkaline earth metal hydroxides, Ksp increases down the group. So, Ba(OH)2 is the most soluble in water.
Why basic strength decreases down the group?
Solution : The basic strength of the hydrides of group 15 elements down the group decreases because down the group as electronegativity decreases `p`-orbital take part in the bond and lone pair present in `s`-orbital : `s`-orbital is larger and non directional hence it has less effective tendency of bond formation.
Why KOH is more basic than NaOH?
Solution : Among NaOH and KOH, KOH is a stronger base. Due to large size of K,K-O bond is weaker than Na-O bond. Hence it is a stronger base than NaOH.
Why NaOH is a strong but NH4OH is weak electrolyte?
Because NaoH is a strong alkali which it dissociates almost completely into its ions when electricity is passed. Hence it’s a strong electrolyte. NH4OH is weak base and doesn’t dissociate completely into ions hence it’s a weak electrolyte.
Why is KOH more soluble than NaOH?
Why is KOH preferred over NaOH?
Potassium hydroxide is slightly smaller than sodium hydroxide which means it cuts through oil molecules faster than sodium hydroxide. This makes potassium hydroxide a great choice for soaps that need to remove caked-on oil. Their reactions are slightly different as well.
Why does acidity increase down a group?
Going down a group the acid strength increases because the bond strength decreases as a function of increasing size of the nonmetal, and this has a larger effect than the electronegativity. In fact HF is a weak acid because it is so small that the hydrogen-fluorine bond is so strong that it is hard to break.
Why does basicity decrease from left to right?
On moving from left to right in the lanthanoid series, size of the elements decreases thereby increasing the polarising power of the cation and hence the basicity of lanthanoid hydroxides decreases.