Answer
Verified
394.5k+ views
Hint: Conjugate base are those molecules in which one H-atom is absent whereas conjugate acid has one extra hydrogen atom. Bronsted acid donates whereas bronsted base accepts a hydrogen ion.
Complete step by step answer:
(a) we have to identify the conjugate base from the given choices.
- As we know that conjugate base contains one less hydrogen atom and also we can identify them by counting the number of H-atoms in the reactant as well the product side.
- If there is any decrease in the number of H-atoms, they will be considered as the conjugate base and vice versa.
- So, to write the conjugate base we will remove one H-atom form each compound.
- Hence, the conjugate is:
${{\text{S}}^{2-}},{{\text{H}}_{2}}\text{O, HPO}_{4}^{-}\text{, SO}_{4}^{-}\text{, }{{\text{F}}^{-}}\text{, C}{{\text{H}}_{3}}\text{CO}{{\text{O}}^{-}}\text{, }{{\text{C}}_{6}}{{\text{H}}_{5}}{{\text{O}}^{-}}\text{, ClO}_{4}^{-}\text{, N}{{\text{H}}_{3}}$
(b) Similarly, for conjugate acid, we will add an extra H-atom to the given compound i.e.
${{\text{H}}_{2}}\text{O, C}{{\text{H}}_{3}}\text{COOH, HCl,HCO}_{3}^{-}\text{,C}{{\text{H}}_{3}}\text{NH}_{3}^{+}\text{, C}{{\text{H}}_{3}}\text{COOH}_{2}^{+}\text{, N}{{\text{H}}_{3}}$
(c) Now, we have to identify those compounds which act as both Bronsted acid as well as base i.e. they can accept as well as donate a pair of electrons.
- So, from the given compound, ${{\text{H}}_{2}}\text{O, HCO}_{3}^{-};\text{ N}{{\text{H}}_{3}},\text{ H}{{\text{S}}^{-}}$can act as both.
Now, we have to identify the substance which is a stronger acid.
- So, we know that strong acids can easily give ${{\text{H}}^{+}}$ i.e. more easily they give ${{\text{H}}^{+}}$ions, more is the acidic strength.
- So, among the given compound the order will be $\text{HI}$˃ $\text{HCl}$; ${{\text{H}}_{2}}\text{S}{{\text{O}}_{4}}$˃${{\text{H}}_{2}}\text{C}{{\text{O}}_{3}}$; ${{\text{H}}_{2}}\text{S}$˃ ${{\text{H}}_{2}}\text{O}$; ${{\text{C}}_{6}}{{\text{H}}_{5}}\text{OH}$˃${{\text{C}}_{2}}{{\text{H}}_{5}}\text{OH}$.
(e) Now, we have to identify the strong base and we know that they can easily dissociate hydroxyl ions.
- So, from the given compounds strong bases are:
$\text{O}{{\text{H}}^{-}}$˃ $\text{C}{{\text{l}}^{-}}$; $\text{NH}_{2}^{-}$˃ $\text{O}{{\text{H}}^{-}}$; $\text{O}{{\text{H}}^{-}}$˃ $\text{C}{{\text{H}}_{3}}\text{CO}{{\text{O}}^{-}}$; $\text{C}{{\text{H}}_{3}}\text{CO}{{\text{O}}^{-}}$˃ $\text{C}{{\text{l}}^{-}}$; $\text{C}{{\text{H}}_{3}}\text{N}{{\text{H}}_{2}}$˃$\text{N}{{\text{H}}_{3}}$
(f) Now, we have to identify the Lewis acid and Lewis base. Those species which have vacant orbitals to accept electrons are Lewis acid where those who can donate electron pairs are Lewis base.
- From the given compound, Lewis acids are ${{\text{H}}^{+}}\text{, B}{{\text{F}}_{3}}\text{, N}{{\text{i}}^{2+}}\text{, AlC}{{\text{l}}_{3}}\text{, SnC}{{\text{l}}_{4}}$ whereas ${{\text{S}}^{2}}\text{, O}{{\text{H}}^{-}}\text{, N}{{\text{F}}_{3}}\text{, N}{{\text{H}}^{3}}\text{, }{{\left( \text{C}{{\text{H}}_{3}} \right)}_{2}}\text{O}$ are Lewis base.
Note: The difference between conjugate acid and acid is that acids can dissociate to hydrogen ions whereas conjugate acids are formed by the acceptance of H-atom.
Complete step by step answer:
(a) we have to identify the conjugate base from the given choices.
- As we know that conjugate base contains one less hydrogen atom and also we can identify them by counting the number of H-atoms in the reactant as well the product side.
- If there is any decrease in the number of H-atoms, they will be considered as the conjugate base and vice versa.
- So, to write the conjugate base we will remove one H-atom form each compound.
- Hence, the conjugate is:
${{\text{S}}^{2-}},{{\text{H}}_{2}}\text{O, HPO}_{4}^{-}\text{, SO}_{4}^{-}\text{, }{{\text{F}}^{-}}\text{, C}{{\text{H}}_{3}}\text{CO}{{\text{O}}^{-}}\text{, }{{\text{C}}_{6}}{{\text{H}}_{5}}{{\text{O}}^{-}}\text{, ClO}_{4}^{-}\text{, N}{{\text{H}}_{3}}$
(b) Similarly, for conjugate acid, we will add an extra H-atom to the given compound i.e.
${{\text{H}}_{2}}\text{O, C}{{\text{H}}_{3}}\text{COOH, HCl,HCO}_{3}^{-}\text{,C}{{\text{H}}_{3}}\text{NH}_{3}^{+}\text{, C}{{\text{H}}_{3}}\text{COOH}_{2}^{+}\text{, N}{{\text{H}}_{3}}$
(c) Now, we have to identify those compounds which act as both Bronsted acid as well as base i.e. they can accept as well as donate a pair of electrons.
- So, from the given compound, ${{\text{H}}_{2}}\text{O, HCO}_{3}^{-};\text{ N}{{\text{H}}_{3}},\text{ H}{{\text{S}}^{-}}$can act as both.
- So, we know that strong acids can easily give ${{\text{H}}^{+}}$ i.e. more easily they give ${{\text{H}}^{+}}$ions, more is the acidic strength.
- So, among the given compound the order will be $\text{HI}$˃ $\text{HCl}$; ${{\text{H}}_{2}}\text{S}{{\text{O}}_{4}}$˃${{\text{H}}_{2}}\text{C}{{\text{O}}_{3}}$; ${{\text{H}}_{2}}\text{S}$˃ ${{\text{H}}_{2}}\text{O}$; ${{\text{C}}_{6}}{{\text{H}}_{5}}\text{OH}$˃${{\text{C}}_{2}}{{\text{H}}_{5}}\text{OH}$.
(e) Now, we have to identify the strong base and we know that they can easily dissociate hydroxyl ions.
- So, from the given compounds strong bases are:
$\text{O}{{\text{H}}^{-}}$˃ $\text{C}{{\text{l}}^{-}}$; $\text{NH}_{2}^{-}$˃ $\text{O}{{\text{H}}^{-}}$; $\text{O}{{\text{H}}^{-}}$˃ $\text{C}{{\text{H}}_{3}}\text{CO}{{\text{O}}^{-}}$; $\text{C}{{\text{H}}_{3}}\text{CO}{{\text{O}}^{-}}$˃ $\text{C}{{\text{l}}^{-}}$; $\text{C}{{\text{H}}_{3}}\text{N}{{\text{H}}_{2}}$˃$\text{N}{{\text{H}}_{3}}$
(f) Now, we have to identify the Lewis acid and Lewis base. Those species which have vacant orbitals to accept electrons are Lewis acid where those who can donate electron pairs are Lewis base.
- From the given compound, Lewis acids are ${{\text{H}}^{+}}\text{, B}{{\text{F}}_{3}}\text{, N}{{\text{i}}^{2+}}\text{, AlC}{{\text{l}}_{3}}\text{, SnC}{{\text{l}}_{4}}$ whereas ${{\text{S}}^{2}}\text{, O}{{\text{H}}^{-}}\text{, N}{{\text{F}}_{3}}\text{, N}{{\text{H}}^{3}}\text{, }{{\left( \text{C}{{\text{H}}_{3}} \right)}_{2}}\text{O}$ are Lewis base.
Note: The difference between conjugate acid and acid is that acids can dissociate to hydrogen ions whereas conjugate acids are formed by the acceptance of H-atom.
Recently Updated Pages
Basicity of sulphurous acid and sulphuric acid are
Three beakers labelled as A B and C each containing 25 mL of water were taken A small amount of NaOH anhydrous CuSO4 and NaCl were added to the beakers A B and C respectively It was observed that there was an increase in the temperature of the solutions contained in beakers A and B whereas in case of beaker C the temperature of the solution falls Which one of the following statements isarecorrect i In beakers A and B exothermic process has occurred ii In beakers A and B endothermic process has occurred iii In beaker C exothermic process has occurred iv In beaker C endothermic process has occurred
What is the stopping potential when the metal with class 12 physics JEE_Main
The momentum of a photon is 2 times 10 16gm cmsec Its class 12 physics JEE_Main
How do you arrange NH4 + BF3 H2O C2H2 in increasing class 11 chemistry CBSE
Is H mCT and q mCT the same thing If so which is more class 11 chemistry CBSE
Trending doubts
State the differences between manure and fertilize class 8 biology CBSE
Why are xylem and phloem called complex tissues aBoth class 11 biology CBSE
Difference between Prokaryotic cell and Eukaryotic class 11 biology CBSE
Difference Between Plant Cell and Animal Cell
What would happen if plasma membrane ruptures or breaks class 11 biology CBSE
Give 10 examples for herbs , shrubs , climbers , creepers
What precautions do you take while observing the nucleus class 11 biology CBSE
What would happen to the life of a cell if there was class 11 biology CBSE
Change the following sentences into negative and interrogative class 10 english CBSE