315841
Statement A : \(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water. Statement B : Carbonate is a strong base and reacts with \(\mathrm{H}^{+}\)from the strong acid, causing the barium salt to dissociate.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
\(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water because carbonate is a weak base and reacts with \(\mathrm{H}^{+}\)ion of \(\mathrm{HNO}_{3}\) causing barium salt to dissociate. The reaction involved is as follows: \(\mathrm{BaCO}_{3}+2 \mathrm{HNO}_{3} \rightarrow \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\) So, the option (1) is correct.
CHXI10:THE S-BLOCK ELEMENTS
315842
The correct order of the solubility of alkaline-earth metal sulphates in water is :
The solubility of sulphates of alkaline earth metals decreases as we move down the group from \(\mathrm{Be}\) to \(\mathrm{Ba}\) due to the reason that ionic size increases down the group. The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference. Thus, the order will be \(\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}\)
JEE - 2016
CHXI10:THE S-BLOCK ELEMENTS
315843
The solubilities of \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{BeSO}_{4}, \mathrm{MgSO}_{4}\) and \(\mathrm{BaSO}_{4}\) will follow the order
Alkali metal sulphates are more soluble as compared to alkaline earth metal sulphates. Thus, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is most soluble. Among alkaline earth metal sulphates, \(\mathrm{BeSO}_{4}\) is most soluble. This is because on moving downward, the magnitude of lattice energy remains almost constant (due to large sized sulphate ion) but hydration energy decreases.Hence, the order of solubility is \(\mathrm{Na}_{2} \mathrm{SO}_{4}>\mathrm{BeSO}_{4}>\mathrm{MgSO}_{4}>\mathrm{BaSO}_{4}\)
CHXI10:THE S-BLOCK ELEMENTS
315844
Which of the following decomposes at highest temperature?
1 \(\mathrm{CaCO}_{3}\)
2 \(\mathrm{SrCO}_{3}\)
3 \(\mathrm{BaCO}_{3}\)
4 \(\mathrm{MgCO}_{3}\)
Explanation:
\(\mathrm{BaCO}_{3}\) decomposes at highest temp. All the carbonates decompose on heating to give \(\mathrm{CO}_{2}\) and metal oxide. \(\mathrm{MCO}_{3} \stackrel{\Delta}{\longrightarrow} \mathrm{MO}+\mathrm{CO}_{2}\) The stability of carbonate towards heat depends upon the stability of the resulting metal oxide. More is the stability of the resulting metal oxide lesser is the stability of the carbonate towards heat and vice versa.
CHXI10:THE S-BLOCK ELEMENTS
315845
The alkaline earth metal nitrate that does not crystallise with water molecules is
Smaller the size of alkaline earth metals, greater is the tendency of their nitrate to crystallise with water molecule. Since \(\mathrm{Ba}\) is the biggest among alkaline earth metal so its nitrate does not crystallise with water molecule.
315841
Statement A : \(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water. Statement B : Carbonate is a strong base and reacts with \(\mathrm{H}^{+}\)from the strong acid, causing the barium salt to dissociate.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
\(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water because carbonate is a weak base and reacts with \(\mathrm{H}^{+}\)ion of \(\mathrm{HNO}_{3}\) causing barium salt to dissociate. The reaction involved is as follows: \(\mathrm{BaCO}_{3}+2 \mathrm{HNO}_{3} \rightarrow \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\) So, the option (1) is correct.
CHXI10:THE S-BLOCK ELEMENTS
315842
The correct order of the solubility of alkaline-earth metal sulphates in water is :
The solubility of sulphates of alkaline earth metals decreases as we move down the group from \(\mathrm{Be}\) to \(\mathrm{Ba}\) due to the reason that ionic size increases down the group. The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference. Thus, the order will be \(\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}\)
JEE - 2016
CHXI10:THE S-BLOCK ELEMENTS
315843
The solubilities of \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{BeSO}_{4}, \mathrm{MgSO}_{4}\) and \(\mathrm{BaSO}_{4}\) will follow the order
Alkali metal sulphates are more soluble as compared to alkaline earth metal sulphates. Thus, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is most soluble. Among alkaline earth metal sulphates, \(\mathrm{BeSO}_{4}\) is most soluble. This is because on moving downward, the magnitude of lattice energy remains almost constant (due to large sized sulphate ion) but hydration energy decreases.Hence, the order of solubility is \(\mathrm{Na}_{2} \mathrm{SO}_{4}>\mathrm{BeSO}_{4}>\mathrm{MgSO}_{4}>\mathrm{BaSO}_{4}\)
CHXI10:THE S-BLOCK ELEMENTS
315844
Which of the following decomposes at highest temperature?
1 \(\mathrm{CaCO}_{3}\)
2 \(\mathrm{SrCO}_{3}\)
3 \(\mathrm{BaCO}_{3}\)
4 \(\mathrm{MgCO}_{3}\)
Explanation:
\(\mathrm{BaCO}_{3}\) decomposes at highest temp. All the carbonates decompose on heating to give \(\mathrm{CO}_{2}\) and metal oxide. \(\mathrm{MCO}_{3} \stackrel{\Delta}{\longrightarrow} \mathrm{MO}+\mathrm{CO}_{2}\) The stability of carbonate towards heat depends upon the stability of the resulting metal oxide. More is the stability of the resulting metal oxide lesser is the stability of the carbonate towards heat and vice versa.
CHXI10:THE S-BLOCK ELEMENTS
315845
The alkaline earth metal nitrate that does not crystallise with water molecules is
Smaller the size of alkaline earth metals, greater is the tendency of their nitrate to crystallise with water molecule. Since \(\mathrm{Ba}\) is the biggest among alkaline earth metal so its nitrate does not crystallise with water molecule.
315841
Statement A : \(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water. Statement B : Carbonate is a strong base and reacts with \(\mathrm{H}^{+}\)from the strong acid, causing the barium salt to dissociate.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
\(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water because carbonate is a weak base and reacts with \(\mathrm{H}^{+}\)ion of \(\mathrm{HNO}_{3}\) causing barium salt to dissociate. The reaction involved is as follows: \(\mathrm{BaCO}_{3}+2 \mathrm{HNO}_{3} \rightarrow \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\) So, the option (1) is correct.
CHXI10:THE S-BLOCK ELEMENTS
315842
The correct order of the solubility of alkaline-earth metal sulphates in water is :
The solubility of sulphates of alkaline earth metals decreases as we move down the group from \(\mathrm{Be}\) to \(\mathrm{Ba}\) due to the reason that ionic size increases down the group. The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference. Thus, the order will be \(\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}\)
JEE - 2016
CHXI10:THE S-BLOCK ELEMENTS
315843
The solubilities of \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{BeSO}_{4}, \mathrm{MgSO}_{4}\) and \(\mathrm{BaSO}_{4}\) will follow the order
Alkali metal sulphates are more soluble as compared to alkaline earth metal sulphates. Thus, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is most soluble. Among alkaline earth metal sulphates, \(\mathrm{BeSO}_{4}\) is most soluble. This is because on moving downward, the magnitude of lattice energy remains almost constant (due to large sized sulphate ion) but hydration energy decreases.Hence, the order of solubility is \(\mathrm{Na}_{2} \mathrm{SO}_{4}>\mathrm{BeSO}_{4}>\mathrm{MgSO}_{4}>\mathrm{BaSO}_{4}\)
CHXI10:THE S-BLOCK ELEMENTS
315844
Which of the following decomposes at highest temperature?
1 \(\mathrm{CaCO}_{3}\)
2 \(\mathrm{SrCO}_{3}\)
3 \(\mathrm{BaCO}_{3}\)
4 \(\mathrm{MgCO}_{3}\)
Explanation:
\(\mathrm{BaCO}_{3}\) decomposes at highest temp. All the carbonates decompose on heating to give \(\mathrm{CO}_{2}\) and metal oxide. \(\mathrm{MCO}_{3} \stackrel{\Delta}{\longrightarrow} \mathrm{MO}+\mathrm{CO}_{2}\) The stability of carbonate towards heat depends upon the stability of the resulting metal oxide. More is the stability of the resulting metal oxide lesser is the stability of the carbonate towards heat and vice versa.
CHXI10:THE S-BLOCK ELEMENTS
315845
The alkaline earth metal nitrate that does not crystallise with water molecules is
Smaller the size of alkaline earth metals, greater is the tendency of their nitrate to crystallise with water molecule. Since \(\mathrm{Ba}\) is the biggest among alkaline earth metal so its nitrate does not crystallise with water molecule.
315841
Statement A : \(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water. Statement B : Carbonate is a strong base and reacts with \(\mathrm{H}^{+}\)from the strong acid, causing the barium salt to dissociate.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
\(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water because carbonate is a weak base and reacts with \(\mathrm{H}^{+}\)ion of \(\mathrm{HNO}_{3}\) causing barium salt to dissociate. The reaction involved is as follows: \(\mathrm{BaCO}_{3}+2 \mathrm{HNO}_{3} \rightarrow \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\) So, the option (1) is correct.
CHXI10:THE S-BLOCK ELEMENTS
315842
The correct order of the solubility of alkaline-earth metal sulphates in water is :
The solubility of sulphates of alkaline earth metals decreases as we move down the group from \(\mathrm{Be}\) to \(\mathrm{Ba}\) due to the reason that ionic size increases down the group. The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference. Thus, the order will be \(\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}\)
JEE - 2016
CHXI10:THE S-BLOCK ELEMENTS
315843
The solubilities of \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{BeSO}_{4}, \mathrm{MgSO}_{4}\) and \(\mathrm{BaSO}_{4}\) will follow the order
Alkali metal sulphates are more soluble as compared to alkaline earth metal sulphates. Thus, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is most soluble. Among alkaline earth metal sulphates, \(\mathrm{BeSO}_{4}\) is most soluble. This is because on moving downward, the magnitude of lattice energy remains almost constant (due to large sized sulphate ion) but hydration energy decreases.Hence, the order of solubility is \(\mathrm{Na}_{2} \mathrm{SO}_{4}>\mathrm{BeSO}_{4}>\mathrm{MgSO}_{4}>\mathrm{BaSO}_{4}\)
CHXI10:THE S-BLOCK ELEMENTS
315844
Which of the following decomposes at highest temperature?
1 \(\mathrm{CaCO}_{3}\)
2 \(\mathrm{SrCO}_{3}\)
3 \(\mathrm{BaCO}_{3}\)
4 \(\mathrm{MgCO}_{3}\)
Explanation:
\(\mathrm{BaCO}_{3}\) decomposes at highest temp. All the carbonates decompose on heating to give \(\mathrm{CO}_{2}\) and metal oxide. \(\mathrm{MCO}_{3} \stackrel{\Delta}{\longrightarrow} \mathrm{MO}+\mathrm{CO}_{2}\) The stability of carbonate towards heat depends upon the stability of the resulting metal oxide. More is the stability of the resulting metal oxide lesser is the stability of the carbonate towards heat and vice versa.
CHXI10:THE S-BLOCK ELEMENTS
315845
The alkaline earth metal nitrate that does not crystallise with water molecules is
Smaller the size of alkaline earth metals, greater is the tendency of their nitrate to crystallise with water molecule. Since \(\mathrm{Ba}\) is the biggest among alkaline earth metal so its nitrate does not crystallise with water molecule.
315841
Statement A : \(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water. Statement B : Carbonate is a strong base and reacts with \(\mathrm{H}^{+}\)from the strong acid, causing the barium salt to dissociate.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
\(\mathrm{BaCO}_{3}\) is more soluble in \(\mathrm{HNO}_{3}\) than in water because carbonate is a weak base and reacts with \(\mathrm{H}^{+}\)ion of \(\mathrm{HNO}_{3}\) causing barium salt to dissociate. The reaction involved is as follows: \(\mathrm{BaCO}_{3}+2 \mathrm{HNO}_{3} \rightarrow \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\) So, the option (1) is correct.
CHXI10:THE S-BLOCK ELEMENTS
315842
The correct order of the solubility of alkaline-earth metal sulphates in water is :
The solubility of sulphates of alkaline earth metals decreases as we move down the group from \(\mathrm{Be}\) to \(\mathrm{Ba}\) due to the reason that ionic size increases down the group. The lattice energy remains constant because sulphate ion is so large, so that small change in cationic sizes do not make any difference. Thus, the order will be \(\mathrm{Mg}>\mathrm{Ca}>\mathrm{Sr}>\mathrm{Ba}\)
JEE - 2016
CHXI10:THE S-BLOCK ELEMENTS
315843
The solubilities of \(\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{BeSO}_{4}, \mathrm{MgSO}_{4}\) and \(\mathrm{BaSO}_{4}\) will follow the order
Alkali metal sulphates are more soluble as compared to alkaline earth metal sulphates. Thus, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) is most soluble. Among alkaline earth metal sulphates, \(\mathrm{BeSO}_{4}\) is most soluble. This is because on moving downward, the magnitude of lattice energy remains almost constant (due to large sized sulphate ion) but hydration energy decreases.Hence, the order of solubility is \(\mathrm{Na}_{2} \mathrm{SO}_{4}>\mathrm{BeSO}_{4}>\mathrm{MgSO}_{4}>\mathrm{BaSO}_{4}\)
CHXI10:THE S-BLOCK ELEMENTS
315844
Which of the following decomposes at highest temperature?
1 \(\mathrm{CaCO}_{3}\)
2 \(\mathrm{SrCO}_{3}\)
3 \(\mathrm{BaCO}_{3}\)
4 \(\mathrm{MgCO}_{3}\)
Explanation:
\(\mathrm{BaCO}_{3}\) decomposes at highest temp. All the carbonates decompose on heating to give \(\mathrm{CO}_{2}\) and metal oxide. \(\mathrm{MCO}_{3} \stackrel{\Delta}{\longrightarrow} \mathrm{MO}+\mathrm{CO}_{2}\) The stability of carbonate towards heat depends upon the stability of the resulting metal oxide. More is the stability of the resulting metal oxide lesser is the stability of the carbonate towards heat and vice versa.
CHXI10:THE S-BLOCK ELEMENTS
315845
The alkaline earth metal nitrate that does not crystallise with water molecules is
Smaller the size of alkaline earth metals, greater is the tendency of their nitrate to crystallise with water molecule. Since \(\mathrm{Ba}\) is the biggest among alkaline earth metal so its nitrate does not crystallise with water molecule.
