Hydration Enthalpy and Lattice Enthalpy (Group 2)

Q.

The solubility of metal halides depends on their nature, lattice enthalpy and hydration enthalpy of the individual ions. Amongst flurides of alkali metals, the lowest solubility of LiF in water is due to
(a) Ionic nature fo lithium fluoride
(b) high lattice enthalpy
(c) high hydration enthalpy for lithium ion
(d) low ionisation enthalpy of lithium atom

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

Compounds of alkaline earth metals are less soluble than alkali metals, due to:

1. Their high hydration enthalpy
2. Their high lattice enthalpy
3. Their increased covalent character
4. Their high ionisation enthalpy

Q. The solubilities of carbonates decrease down the Mg group due to a decrease in

1. interionic interaction
2. lattice energies of solids
3. hydration energies of cations
4. entropy of solution formation

Q.

If NaCl is doped with 10⁻³ mol % of SrCl₂, what is the concentration of cation vacancies?

Q.

What are the common physical and chemical features of alkali metals?

Q.

Why Is hydration enthalpy of lithium highest?

Q.

Amploteric hydroxides react with both alkalies and acids. Which of the following Group 2 metal hydroxides is soluble in sodium hydroxide?
(a) $Be(OH{)}_2$ (b) $Mg(OH{)}_2$ (c) $Ca(OH{)}_2$ (d) $Ba(OH{)}_2$

Q.

Molar ionic conductivity of a bivalent electrolyte are 57 and 73. The molar conductivity of the solution will be

Q. 11. Which has maximum molal depression constants? 1) 0.1M aq KCl 2)0.1M aq sodium sulphate 3)0.2M aq barium phosphate 4)same for all

Q.

What does the solubility of s block halides in water depend upon?

Q.

Calculate the depression in the freezing point of water when 10 g of CH₃CH₂CHClCOOH is added to 250 g of water. K_a = 1.4 × 10⁻³, K_f = 1.86

K kg mol⁻¹.

Q.

The halogen with the highest first ionization energy is ___________

Q.

$SnC{l}_4$ is liquid while $SnC{l}_2$ is solid. Explain.

Q. Which of the following is least soluble in water?

1. 
2. 
3. 
4. 

Q.

Which of the following alkaline earth metal sulphates has hydration enthalpy higher than the lattice enthalpy?

1. $CaS{O}_4$

2. $BaS{O}_4$

3. $BeS{O}_4$

4. $SrS{O}_4$

Q. What are the chemical properties of Lanthanoids ?

Q.

How do the hydrides of s-block elements act as powerful reducing agents?

Q. A liquid system containning two immiscible liquids water and n- butyl bromide distils at 90^° C . Their vapour pressure at this temperature are in the ratio of 5:1 respectively. The ratio of their masses distilled is

Q.

Which of the following phenomena occurs when a chalk stick is dipped in ink?

1. absorption & adsorption both of solvent

2. adsorption of coloured substance

3. adsorption of solvent

4. absorption of solvent

Q. What is molality of an aqueous solution whose relative lowering in vapor pressure is 0.1?

Q. The elements which exist in the liquid state at room temperature are:

1. $Na$
2. $Br$
3. $Hg$
4. $Ga$

Q. What will be the mole percentage of CH3OH and H2O resectively in 60% (by mass) aqueous solution of CH3OH??

Q. "The solubility of carbonates and bicarbonates of alkali metals increases down the group."
Answer whether the above statement is true or false.
If true enter 1, else enter 0.

Q. Acetic acid is titrated with $NaOH$ solution. Which of the following statements is correct for this titration?

1. Conductance slowly decreases upto the equivalence point, then it decreases rapidly
2. Conductance decreases upto equivalence point, then it increases
3. First conductance increases slowly up to the equivalence point and then increases rapidly
4. First conductance increases slowly up to the equivalence point and then drops rapidly

Q. The freezing point of an aqueous solution having 6%urea and18%glucose by weight is if kf water is 1.86K kg/mole

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

$Be{F}_2$ is soluble in water while fluorides of other alkaline earth metals are insoluble because of:

1. Covalent nature of $Be{F}_2$
2. Ionic nature of $Be{F}_2$
3. Greater hydration enthalpy of $B{e}^{2+}$ ion
4. Greater lattice enthalpy of $B{e}^{2+}$ ion

Q. Solubility of an ionic compound in water is mainly dependent on:
a. Lattice enthalpy
b. Hydration enthalpy
Both these factors oppose each other, and the resultant of these factors determines the solubility of an ionic compound in water. If the lattice enthalpy has a larger value, the compound is less soluble. If the hydration enthalpy has larger value, the compound is highly soluble in water.

A compound is soluble in water if the hydration enthalpy is:

1. Greater than the lattice enthalpy
2. Less than the lattice enthalpy
3. Same as the lattice enthalpy
4. None of the above

Q. 1. Assuming salts to be 90percent dissociated which of the following will have highest osmotic pressure? 1)decimolar aluminium sulphate 2)decimolar barium chloride 3)decimolar sodium sulphate

Q. The following compounds have been arranged in order of their increasing thermal stabilities. Identify the correct order.
$K_{2}C{O}_3\left(I\right),MgC{O}_3\left(II\right),CaC{O}_3\left(III\right),BeC{O}_3\left(IV\right)$

1. $IV<II<I<III$
2. $II<IV<III<I$
3. $IV<II<III<I$
4. $I<II<III<IV$

Q.

Which of the following compunds are readily soluble in water.?

(a) $BeS{O}_4$ (b) $MgS{O}_4$ (c) $BaS{O}_4$ (d) $SrS{O}_4$