Question

The solubility of AgCl in 0.1M aqueous NaCl solution is (K_(sp) of AgCl=1.8times10^(-10))​

Answer 1

☆Concept:

▪︎AgCl is less soluble than NaCl,so its confirmed that NaCl will dissociate more than AgCl.

▪︎NaCl ions will be much higher than AgCl ions..

OR we can say that,dissociated $\ Cl^{-1}$ of NaCl will be much higher than AgCl, $\ Cl^{-1}$ ions

☆solution:

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$

》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$

they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,

bcz the Cl ions AgCl is negligible.

----------

$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$

$\sf{ 1.8×10^{-10} = [S][0.1]}$

$\bf{ S=1.8×10^{-9}}$

-----

so,the amount of Ag ions dissolve will be the same amount of solubility of AgCl.

$\bf{ S=1.8×10^{-9}}$

×××××-------××××××-------×××××××

♧hope it helps!♧

Answer 2

Explanation:

$\huge\pink{\boxed{\blue{\boxed{ \purple{ \boxed{{\pink{Answer}}}}}}}} \\ \large\pink{\boxed{\blue{\boxed{ \purple{ \boxed{{\pink{Your~answer↓}}}}}}}}$

☆Concept:

▪︎AgCl is less soluble than NaCl,so its confirmed that NaCl will dissociate more than AgCl.

▪︎AgCl is less soluble than NaCl,so its confirmed that NaCl will dissociate more than AgCl.▪︎NaCl ions will be much higher than AgCl ions..

▪︎AgCl is less soluble than NaCl,so its confirmed that NaCl will dissociate more than AgCl.▪︎NaCl ions will be much higher than AgCl ions..OR we can say that,dissociated $\ Cl^{-1}$ of NaCl will be much higher than AgCl, $\ Cl^{-1}$ ions

☆solution:

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible.

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$$\sf{ 1.8×10^{-10} = [S][0.1]}$

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$$\sf{ 1.8×10^{-10} = [S][0.1]}$$\bf{ S=1.8×10^{-9}}$

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$$\sf{ 1.8×10^{-10} = [S][0.1]}$$\bf{ S=1.8×10^{-9}}$-----

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$$\sf{ 1.8×10^{-10} = [S][0.1]}$$\bf{ S=1.8×10^{-9}}$-----so,the amount of Ag ions dissolve will be the same amount of solubility of AgCl.

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$$\sf{ 1.8×10^{-10} = [S][0.1]}$$\bf{ S=1.8×10^{-9}}$-----so,the amount of Ag ions dissolve will be the same amount of solubility of AgCl.$\bf{ S=1.8×10^{-9}}$

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$$\sf{ 1.8×10^{-10} = [S][0.1]}$$\bf{ S=1.8×10^{-9}}$-----so,the amount of Ag ions dissolve will be the same amount of solubility of AgCl.$\bf{ S=1.8×10^{-9}}$×××××-------××××××-------×××××××

》$\ NaCl \rightarrow{ Na^{+1}+Cl^{-1}}$》$\ AgCl \rightarrow{ Ag^{+1}+Cl^{-1}}$they both are present in same aqueous solution, so if we take solubility of AgCl than,the Cl ions will be 0.1M,bcz the Cl ions AgCl is negligible. ----------$\bf{ K_{sp} = [Ag^{+1}][Cl^{-1}]}$$\sf{ 1.8×10^{-10} = [S][0.1]}$$\bf{ S=1.8×10^{-9}}$-----so,the amount of Ag ions dissolve will be the same amount of solubility of AgCl.$\bf{ S=1.8×10^{-9}}$×××××-------××××××-------×××××××♧hope it helps!♧

$\huge \fcolorbox{black}{cyan}{♛Hope it helps U♛}$