Among aqueous 1 N solutions, the pH of HCl , $\mathrm{HNO}_2$ and $\mathrm{CH}_3 \mathrm{COOH}$ follows the order
$\mathrm{HCl}<\mathrm{HNO}_2<\mathrm{CH}_3 \mathrm{COOH}$
$\mathrm{CH}_3 \mathrm{COOH}<\mathrm{HNO}_2<\mathrm{HCl}$
$\mathrm{HNO}_2<\mathrm{CH}_3 \mathrm{COOH}<\mathrm{HCl}$
$\mathrm{HCl}<\mathrm{CH}_3 \mathrm{COOH}<\mathrm{HNO}_2$
The ionic radii of $\mathrm{N}^{3-}, \mathrm{O}^{2-}$ and $\mathrm{F}^{-}$follow the trend
$\mathrm{N}^{3-}>\mathrm{O}^{2-}>\mathrm{F}^{-}$
$\mathrm{F}^{-}>\mathrm{N}^{3-}>\mathrm{O}^{2-}$
$\mathrm{O}^{2-}>\mathrm{F}^{-}>\mathrm{N}^{3-}$
$\mathrm{F}^{-}>\mathrm{O}^{2-}>\mathrm{N}^{3-}$
30 mL of 0.1 M acetic acid is mixed with 60 mL of 0.1 M sodium acetate. If $K_a=1.8 \times 10^{-5}$ what will be the pH of the solution?
4.6
5.2
4.8
5.04
0.1 m of urea and 0.05 m of $\mathrm{CaCl}_2$ are dissolved separately in equal volumes of water. Which solution will have higher elevation in boiling point?
Urea solution
$\mathrm{CaCl}_2$ solution
Both will show equal elevation
None will show elevation
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