How do you explain the detection of HI group basic radicals based on a

1.	How do you explain the detection of HI group basic radicals based on application of solubility product?
Answer» Group reagent: NH₄OH ⇌ NH₄⁺ + OH^– ; NH₄Cl ⇌ NH₄⁺ + Cl^– Radicals: Al³⁺, Cr³⁺, Fe³⁺ Here NH₄Cl is a strong electrolyte under goes complete dissociation where as NH₄OH is a weak electrolyte under goes partial dissociation and attains equilibrium between it’s ions and molecules. In this solution because of common ion (NH₄⁺) effect supression of degree of dissociation of NH₄OH takes place. As a result [OH^–] decreases. Hence the metal radical forms it’s respective hydroxides [Al(OH)₃, Cr(OH)₃, Fe(OH)₃]. Whose solubility product is less than ionic product. Hence forms precipitate.

How do you explain the detection of HI group basic radicals based on application of solubility product?

Answer»

Group reagent: NH₄OH ⇌ NH₄⁺ + OH^– ; NH₄Cl ⇌ NH₄⁺ + Cl^–

Radicals: Al³⁺, Cr³⁺, Fe³⁺

Here NH₄Cl is a strong electrolyte under goes complete dissociation where as NH₄OH is a weak electrolyte under goes partial dissociation and attains equilibrium between it’s ions and molecules. In this solution because of common ion (NH₄⁺) effect supression of degree of dissociation of NH₄OH takes place. As a result [OH^–] decreases. Hence the metal radical forms it’s respective hydroxides [Al(OH)₃, Cr(OH)₃, Fe(OH)₃]. Whose solubility product is less than ionic product. Hence forms precipitate.

Discussion

No Comment Found

Related InterviewSolutions

`2.5 ` mL of `(2)/(5)` M weak monoacidic base `(K_(b)=1xx10^(-12) "at" 25^(@)C)` is titrated with `(2)/(15)` M HCl in water at `25^(@)` C. The concentration of `H^(+)` at equivalence point is `(K_(w) = 1 xx 10^(-14) "at" 25^(@)C)`A. `3.7xx10^(-13)M`B. `3.2xx10^(-7) M`C. `3.2xx10^(-2)M`D. `2.7xx10^(-2)M`
Which of the following equimolar solutions can act as a buffer solution?(a) NH4Cl and NH4OH(b) HCl and NaCl(c) HCOOH and HCOONa(d) HNO3 and NH4NO3
The range of pH for acidic and basic buffer is where `K_(a)` and `K_(b)` are the acid base dissociation constants, respectively.A. form `pH=pK_(a)+-2 to pH=pK_(b)+-2`B. from `pH=pK_(a)+1to pH=pK_(b)+1`C. from `pH=pK_(a)+-1to pH=pK_(b)+-1`D. from `pH=pK_(a)+1to pH=pK_(b)-1`
Which of the following expression tepresents the Henderson equation for an acidic buffer ?A. `pH=(1)/(2)pK_(a)-(1)/(2)logC`B. `pH=pK_(a)-l"og"(["Conjugate base"])/(["Acid"])`C. `pH=pK_(a)+"log"(["Conjugate base"])/(["Acid"])`D. `pH=pK_(a)`
An acidic buffer solution can be prepared by mixing equimolar amounts ofA. `B(OH)_(3)` and `Na_(2)B_(4)O_(7).10H_(2)O`B. `NH_(3)` and `NH_(4)CI`C. `HCI` and `NaCI`D. `CH_(3)COOH` and `CH_(3)COONa`
Through a solution containing `Cu^(2+) and Ni^(2+),H_(2)S` gas is passed after adding dil HCl, which will precipitate out and why ?
Give an example of acidic buffer?
How does dilution with water affect the pH of a buffer solution?
Through a solution containing Cu2+and Ni2+,H2S gas is passed after adding dill HCl, which will precipitate out and why?
Write the expression for Ksp for AB3 type salt With solubility s.