229530
Which one of the following salts gives an acidic solution in water?
1 $\mathrm{CH}_3 \mathrm{COONa}$
2 $\mathrm{NH}_4 \mathrm{Cl}$
3 $\mathrm{NaCl}$
4 $\mathrm{CH}_3 \mathrm{COONH}_4$
Explanation:
Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $\mathrm{HCl}$ is a strong acid. $\mathrm{NH}_4 \mathrm{Cl}$ ? $\mathrm{NH}_4^{+}+\mathrm{Cl}^{-}$ $2 \mathrm{H}_2 \mathrm{OG}$ ? $\mathrm{OH}^{-}+\mathrm{H}_3 \mathrm{O}^{+}$ $\mathrm{NH}_4^{+}+\mathrm{OH}^{-}$?? $\mathrm{NH}_4 \mathrm{OH}$
AP-EAMCET-2007
Ionic Equilibrium
229534
When a particular aqueous solution is diluted by a factor of ten with $\mathrm{K}_2 \mathbf{O}$, the $\mathrm{pH}$ increases by one unit. the solution most likely contains a
1 Weak acid
2 Strong base
3 Strong acid
4 Buffer
Explanation:
The increasing of $\mathrm{pH}$ by one unit, that means the solution is more acidic because the $\mathrm{pH}$ scale show the acidic character from 1 to 7 . Less the value in $\mathrm{pH}$ scale, higher acidity of the solution will be. Weak acid $\rightarrow$ Acid that don't completely dissociated in solution. Strong acid $\rightarrow$ Completely dissociated in solution ExaChloric acid hydrobromic acid. Buffer $\rightarrow$ A buffer Solution are resist a change in $\mathrm{pH}$ when small acid or alkali are added.
**SCRA-2014**
Ionic Equilibrium
229535
Consider the following regarding potash alum: 1.It has 24 water molecules. 2.It swells on heating. 3.Its aqueous solution is basic. 4.It is white in colour. Which of the above statements are correct?
1 1 and 2 only
2 1,3 and 4
3 2,3 and 4
4 1,2 and 4
Explanation:
The formula of potash alum is $\mathrm{K}_2 \mathrm{SO}_4 \mathrm{Al}_2\left(\mathrm{SO}_4\right)_3 .24 \mathrm{H}_2 \mathrm{O}$. It is white in colour. It has 24 water molecules and it swells on heating.
SCRA 2010
Ionic Equilibrium
229537
In the reaction $\mathrm{H}_2 \mathrm{O}+\mathrm{HCl} \rightarrow \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$, the species that acts as Bronsted base is :
1 $\mathrm{H}_2 \mathrm{O}$
2 $\mathrm{HCl}$
3 $\mathrm{H}_3 \mathrm{O}^{+}$
4 $\mathrm{Cl}^{-}$
Explanation:
A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $\mathrm{H}^{+}$. Ex. $\mathrm{H}_2 \mathrm{O}$. $\underset{\text { Acid }}{\mathrm{HCl}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { base }}}{\mathrm{Cl}^{-}}+\underset{\substack{\text { Conjugate } \\ \text { acid }}}{\mathrm{H}_3 \mathrm{O}^{+}}$ - Bronsted-Lowry acids are proton/ $/ \mathrm{H}^{+}$doners (Lose $\left.\mathrm{H}^{+}\right)$
229530
Which one of the following salts gives an acidic solution in water?
1 $\mathrm{CH}_3 \mathrm{COONa}$
2 $\mathrm{NH}_4 \mathrm{Cl}$
3 $\mathrm{NaCl}$
4 $\mathrm{CH}_3 \mathrm{COONH}_4$
Explanation:
Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $\mathrm{HCl}$ is a strong acid. $\mathrm{NH}_4 \mathrm{Cl}$ ? $\mathrm{NH}_4^{+}+\mathrm{Cl}^{-}$ $2 \mathrm{H}_2 \mathrm{OG}$ ? $\mathrm{OH}^{-}+\mathrm{H}_3 \mathrm{O}^{+}$ $\mathrm{NH}_4^{+}+\mathrm{OH}^{-}$?? $\mathrm{NH}_4 \mathrm{OH}$
AP-EAMCET-2007
Ionic Equilibrium
229534
When a particular aqueous solution is diluted by a factor of ten with $\mathrm{K}_2 \mathbf{O}$, the $\mathrm{pH}$ increases by one unit. the solution most likely contains a
1 Weak acid
2 Strong base
3 Strong acid
4 Buffer
Explanation:
The increasing of $\mathrm{pH}$ by one unit, that means the solution is more acidic because the $\mathrm{pH}$ scale show the acidic character from 1 to 7 . Less the value in $\mathrm{pH}$ scale, higher acidity of the solution will be. Weak acid $\rightarrow$ Acid that don't completely dissociated in solution. Strong acid $\rightarrow$ Completely dissociated in solution ExaChloric acid hydrobromic acid. Buffer $\rightarrow$ A buffer Solution are resist a change in $\mathrm{pH}$ when small acid or alkali are added.
**SCRA-2014**
Ionic Equilibrium
229535
Consider the following regarding potash alum: 1.It has 24 water molecules. 2.It swells on heating. 3.Its aqueous solution is basic. 4.It is white in colour. Which of the above statements are correct?
1 1 and 2 only
2 1,3 and 4
3 2,3 and 4
4 1,2 and 4
Explanation:
The formula of potash alum is $\mathrm{K}_2 \mathrm{SO}_4 \mathrm{Al}_2\left(\mathrm{SO}_4\right)_3 .24 \mathrm{H}_2 \mathrm{O}$. It is white in colour. It has 24 water molecules and it swells on heating.
SCRA 2010
Ionic Equilibrium
229537
In the reaction $\mathrm{H}_2 \mathrm{O}+\mathrm{HCl} \rightarrow \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$, the species that acts as Bronsted base is :
1 $\mathrm{H}_2 \mathrm{O}$
2 $\mathrm{HCl}$
3 $\mathrm{H}_3 \mathrm{O}^{+}$
4 $\mathrm{Cl}^{-}$
Explanation:
A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $\mathrm{H}^{+}$. Ex. $\mathrm{H}_2 \mathrm{O}$. $\underset{\text { Acid }}{\mathrm{HCl}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { base }}}{\mathrm{Cl}^{-}}+\underset{\substack{\text { Conjugate } \\ \text { acid }}}{\mathrm{H}_3 \mathrm{O}^{+}}$ - Bronsted-Lowry acids are proton/ $/ \mathrm{H}^{+}$doners (Lose $\left.\mathrm{H}^{+}\right)$
229530
Which one of the following salts gives an acidic solution in water?
1 $\mathrm{CH}_3 \mathrm{COONa}$
2 $\mathrm{NH}_4 \mathrm{Cl}$
3 $\mathrm{NaCl}$
4 $\mathrm{CH}_3 \mathrm{COONH}_4$
Explanation:
Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $\mathrm{HCl}$ is a strong acid. $\mathrm{NH}_4 \mathrm{Cl}$ ? $\mathrm{NH}_4^{+}+\mathrm{Cl}^{-}$ $2 \mathrm{H}_2 \mathrm{OG}$ ? $\mathrm{OH}^{-}+\mathrm{H}_3 \mathrm{O}^{+}$ $\mathrm{NH}_4^{+}+\mathrm{OH}^{-}$?? $\mathrm{NH}_4 \mathrm{OH}$
AP-EAMCET-2007
Ionic Equilibrium
229534
When a particular aqueous solution is diluted by a factor of ten with $\mathrm{K}_2 \mathbf{O}$, the $\mathrm{pH}$ increases by one unit. the solution most likely contains a
1 Weak acid
2 Strong base
3 Strong acid
4 Buffer
Explanation:
The increasing of $\mathrm{pH}$ by one unit, that means the solution is more acidic because the $\mathrm{pH}$ scale show the acidic character from 1 to 7 . Less the value in $\mathrm{pH}$ scale, higher acidity of the solution will be. Weak acid $\rightarrow$ Acid that don't completely dissociated in solution. Strong acid $\rightarrow$ Completely dissociated in solution ExaChloric acid hydrobromic acid. Buffer $\rightarrow$ A buffer Solution are resist a change in $\mathrm{pH}$ when small acid or alkali are added.
**SCRA-2014**
Ionic Equilibrium
229535
Consider the following regarding potash alum: 1.It has 24 water molecules. 2.It swells on heating. 3.Its aqueous solution is basic. 4.It is white in colour. Which of the above statements are correct?
1 1 and 2 only
2 1,3 and 4
3 2,3 and 4
4 1,2 and 4
Explanation:
The formula of potash alum is $\mathrm{K}_2 \mathrm{SO}_4 \mathrm{Al}_2\left(\mathrm{SO}_4\right)_3 .24 \mathrm{H}_2 \mathrm{O}$. It is white in colour. It has 24 water molecules and it swells on heating.
SCRA 2010
Ionic Equilibrium
229537
In the reaction $\mathrm{H}_2 \mathrm{O}+\mathrm{HCl} \rightarrow \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$, the species that acts as Bronsted base is :
1 $\mathrm{H}_2 \mathrm{O}$
2 $\mathrm{HCl}$
3 $\mathrm{H}_3 \mathrm{O}^{+}$
4 $\mathrm{Cl}^{-}$
Explanation:
A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $\mathrm{H}^{+}$. Ex. $\mathrm{H}_2 \mathrm{O}$. $\underset{\text { Acid }}{\mathrm{HCl}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { base }}}{\mathrm{Cl}^{-}}+\underset{\substack{\text { Conjugate } \\ \text { acid }}}{\mathrm{H}_3 \mathrm{O}^{+}}$ - Bronsted-Lowry acids are proton/ $/ \mathrm{H}^{+}$doners (Lose $\left.\mathrm{H}^{+}\right)$
229530
Which one of the following salts gives an acidic solution in water?
1 $\mathrm{CH}_3 \mathrm{COONa}$
2 $\mathrm{NH}_4 \mathrm{Cl}$
3 $\mathrm{NaCl}$
4 $\mathrm{CH}_3 \mathrm{COONH}_4$
Explanation:
Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $\mathrm{HCl}$ is a strong acid. $\mathrm{NH}_4 \mathrm{Cl}$ ? $\mathrm{NH}_4^{+}+\mathrm{Cl}^{-}$ $2 \mathrm{H}_2 \mathrm{OG}$ ? $\mathrm{OH}^{-}+\mathrm{H}_3 \mathrm{O}^{+}$ $\mathrm{NH}_4^{+}+\mathrm{OH}^{-}$?? $\mathrm{NH}_4 \mathrm{OH}$
AP-EAMCET-2007
Ionic Equilibrium
229534
When a particular aqueous solution is diluted by a factor of ten with $\mathrm{K}_2 \mathbf{O}$, the $\mathrm{pH}$ increases by one unit. the solution most likely contains a
1 Weak acid
2 Strong base
3 Strong acid
4 Buffer
Explanation:
The increasing of $\mathrm{pH}$ by one unit, that means the solution is more acidic because the $\mathrm{pH}$ scale show the acidic character from 1 to 7 . Less the value in $\mathrm{pH}$ scale, higher acidity of the solution will be. Weak acid $\rightarrow$ Acid that don't completely dissociated in solution. Strong acid $\rightarrow$ Completely dissociated in solution ExaChloric acid hydrobromic acid. Buffer $\rightarrow$ A buffer Solution are resist a change in $\mathrm{pH}$ when small acid or alkali are added.
**SCRA-2014**
Ionic Equilibrium
229535
Consider the following regarding potash alum: 1.It has 24 water molecules. 2.It swells on heating. 3.Its aqueous solution is basic. 4.It is white in colour. Which of the above statements are correct?
1 1 and 2 only
2 1,3 and 4
3 2,3 and 4
4 1,2 and 4
Explanation:
The formula of potash alum is $\mathrm{K}_2 \mathrm{SO}_4 \mathrm{Al}_2\left(\mathrm{SO}_4\right)_3 .24 \mathrm{H}_2 \mathrm{O}$. It is white in colour. It has 24 water molecules and it swells on heating.
SCRA 2010
Ionic Equilibrium
229537
In the reaction $\mathrm{H}_2 \mathrm{O}+\mathrm{HCl} \rightarrow \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$, the species that acts as Bronsted base is :
1 $\mathrm{H}_2 \mathrm{O}$
2 $\mathrm{HCl}$
3 $\mathrm{H}_3 \mathrm{O}^{+}$
4 $\mathrm{Cl}^{-}$
Explanation:
A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $\mathrm{H}^{+}$. Ex. $\mathrm{H}_2 \mathrm{O}$. $\underset{\text { Acid }}{\mathrm{HCl}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { base }}}{\mathrm{Cl}^{-}}+\underset{\substack{\text { Conjugate } \\ \text { acid }}}{\mathrm{H}_3 \mathrm{O}^{+}}$ - Bronsted-Lowry acids are proton/ $/ \mathrm{H}^{+}$doners (Lose $\left.\mathrm{H}^{+}\right)$
