To an aqueous solution of AgNO_3,some NaOH_{( | vedclass

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Question

(D) The reaction between $AgNO_3$ and $NaOH$ produces a brown precipitate of silver oxide: $2AgNO_{3(aq)} + 2NaOH_{(aq)} 	o Ag_2O_{(s)} + H_2O_{(l)}

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$Ag$

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(D) The reaction between $AgNO_3$ and $NaOH$ produces a brown precipitate of silver oxide: $2AgNO_{3(aq)} + 2NaOH_{(aq)} 	o Ag_2O_{(s)} + H_2O_{(l)} + 2NaNO_{3(aq)}$ (Brown ppt.) When $H_2O_2$ is added to this brown precipitate,it acts as a reducing agent and reduces $Ag_2O$ to metallic silver,which appears as a black precipitate: $Ag_2O_{(s)} + H_2O_{2(aq)} 	o 2Ag_{(s)} + H_2O_{(l)} + O_{2(g)}$ (Black ppt.) Therefore,the black precipitate is finely divided metallic silver $(Ag)$.

To an aqueous solution of $AgNO_3$,some $NaOH_{(aq)}$ is added until a brown precipitate is obtained. To this,$H_2O_2$ is added dropwise. The precipitate turns black with the evolution of $O_2$. The black precipitate is:

Similar Questions

In which of the following reactions does $H_2O_2$ act as a reducing agent?

$I. \, H_2O_2 + O_3 \rightarrow H_2O + 2O_2$
$II. \, H_2O_2 + Ag_2O \rightarrow 2Ag + H_2O + O_2$
The role of hydrogen peroxide in the above reactions is respectively:

Calculate the strength of $10$ volume solution of hydrogen peroxide. (in $, g/L$)

The volume strength of $1 \, M \, H_2O_2$ is : (Molar mass of $H_2O_2 = 34 \, g \, mol^{-1}$)

Electrolysis of $X$ gives $Y$ at anode. Vacuum distillation of $Y$ gives $H_2O_2$. The number of peroxy $(O-O)$ bonds present in $X$ and $Y$ respectively are :

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