For which of the following mixtures will Ag2SO4(s)precipitate?150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq)150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq)150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.40 M AgNO3(aq)150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.50 M AgNO3(aq)

*

*


The solubility product for the reaction is equilibrium constant where the solid ionic compound dissociates into its ions in a solution. The solubility product is denoted asKsp\rmK_\rmspKsp​. The solubility product value relates to the saturated solution and indicates the precipitate level of the compound. The formation precipitation starts when ionic product exceeds the solubility product.

You are watching: For which of the following mixtures will ag2so4(s) precipitate?


The solubility product value of the compound depends on the concentrations of its ions in a solution.

Example: AB is a solid ionic compound.

Precipitation: If the solubility product value is lesser than the concentration of the ions present in the solution, the compound precipitates in the solution.


The given solid ionic compound is Ag2SO4\rmA\rmg_\rm2\rmS\rmO_4Ag2​SO4​

The equilibrium equation for the ionic compound is given below:

Therefore, the solubility product of the ionic compound is

Ksp=2=1.2×10−5\beginarrayc\\\rmK_\rmsp\,\rm = \,\left< \rmA\rmg^\rm + \right>^\rm2\left< \rmSO_4^2 - \right>\\\\ = 1.2 \times 10^ - 5\\\endarrayKsp​=2=1.2×10−5​

The balanced equation for the reaction of AgNO3andNa2SO4:\rmAgN\rmO_3\;\rmand N\rma_\rm2\rmS\rmO_\rm4:AgNO3​andNa2​SO4​:

The initial concentration of \left< \rmA\rmg^ + \right> ions in AgNO3\rmAgN\rmO_3AgNO3​is given below:

initial=5.0mL×0.20mmolAgNO3mL×1molAg+1molAgNO3(150.0+5.0)mL=0.00645M\beginarrayc\\\left< \rmA\rmg^ + \right>_\rminitial = \frac5.0\rmmL \times \frac\rm0\rm.20mmol AgN\rmO_3\rmmL \times \frac1\rm mol A\rmg^ + 1\rm mol AgN\rmO_3\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.00645\rmM\\\endarrayinitial​=(150.0+5.0)mL5.0mL×mL0.20mmolAgNO3​​×1molAgNO3​1molAg+​​=0.00645M​

The initial concentration of \left< \rmSO_4^2 - \right> ions in Na2SO4\rmN\rma_\rm2\rmS\rmO_\rm4Na2​SO4​is given below:

initial=150.0mL×0.10mmolNa2SO4mL×1molSO42−1molNa2SO4(150.0+5.0)mL=0.0968M\beginarrayc\\\left< \rmSO_\rm4^\rm2 - \right>_\rminitial = \frac150.0\rmmL \times \frac\rm0\rm.10mmol N\rma_\rm2\rmS\rmO_\rm4\rmmL \times \frac1\rm mol SO_4^2 - 1\rm mol N\rma_\rm2\rmS\rmO_\rm4\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.0968\rmM\\\endarrayinitial​=(150.0+5.0)mL150.0mL×mL0.10mmolNa2​SO4​​×1molNa2​SO4​1molSO42−​​​=0.0968M​

The ionic product of Ag2SO3\rmA\rmg_\rm2\rmS\rmO_\rm3Ag2​SO3​is given below:

KIP=initial2initial=(0.00645)2(0.0968)=4.0×10−6\beginarrayc\\\rmK_\rmIP = \left< \rmA\rmg^ + \right>_\rminitial^2\left< \rmSO_4^2 - \right>_\rminitial\\\\ = \left( 0.00645 \right)^2\left( 0.0968 \right)\\\\ = 4.0 \times 10^ - 6\\\endarrayKIP​=initial2​initial​=(0.00645)2(0.0968)=4.0×10−6​

The ionic product (KIP)\left( \rmK_\rmIP \right)(KIP​) is less than the solubility product (Ksp)\left( \rmK_\rmsp \right)(Ksp​),

KIPKsp⇒precipitationdoesnottakesplace\rmK_\rmIP KIP​Ksp​⇒precipitationdoesnottakesplace

The balanced equation for the reaction of AgNO3andNa2SO4:\rmAgN\rmO_3\;\rmand N\rma_\rm2\rmS\rmO_\rm4:AgNO3​andNa2​SO4​:

The initial concentration of \left< \rmA\rmg^ + \right> ions in AgNO3\rmAgN\rmO_3AgNO3​is given below:

initial=5.0mL×0.30mmolAgNO3mL×1molAg+1molAgNO3(150.0+5.0)mL=0.00968M\beginarrayc\\\left< \rmA\rmg^ + \right>_\rminitial = \frac5.0\rmmL \times \frac\rm0\rm.30mmol AgN\rmO_3\rmmL \times \frac1\rm mol A\rmg^ + 1\rm mol AgN\rmO_3\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.00968\rmM\\\endarrayinitial​=(150.0+5.0)mL5.0mL×mL0.30mmolAgNO3​​×1molAgNO3​1molAg+​​=0.00968M​

The initial concentration of \left< \rmSO_4^2 - \right> ions in Na2SO4\rmN\rma_\rm2\rmS\rmO_\rm4Na2​SO4​is given below:

initial=150.0mL×0.10mmolNa2SO4mL×1molSO42−1molNa2SO4(150.0+5.0)mL=0.0968M\beginarrayc\\\left< \rmSO_\rm4^\rm2 - \right>_\rminitial = \frac150.0\rmmL \times \frac\rm0\rm.10mmol N\rma_\rm2\rmS\rmO_\rm4\rmmL \times \frac1\rm mol SO_4^2 - 1\rm mol N\rma_\rm2\rmS\rmO_\rm4\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.0968\rmM\\\endarrayinitial​=(150.0+5.0)mL150.0mL×mL0.10mmolNa2​SO4​​×1molNa2​SO4​1molSO42−​​​=0.0968M​

The ionic product of Ag2SO3\rmA\rmg_\rm2\rmS\rmO_\rm3Ag2​SO3​is given below:

KIP=initial2initial=(0.00968)2(0.0968)=9.1×10−6\beginarrayc\\\rmK_\rmIP = \left< \rmA\rmg^ + \right>_\rminitial^2\left< \rmSO_4^2 - \right>_\rminitial\\\\ = \left( 0.00968 \right)^2\left( 0.0968 \right)\\\\ = 9.1 \times 10^ - 6\\\endarrayKIP​=initial2​initial​=(0.00968)2(0.0968)=9.1×10−6​

The ionic product (KIP)\left( \rmK_\rmIP \right)(KIP​) is less than the solubility product(Ksp)\left( \rmK_\rmsp \right)(Ksp​),

KIPKsp⇒precipitationdoesnottakesplace\rmK_\rmIP KIP​Ksp​⇒precipitationdoesnottakesplace

The balanced equation for the reaction of AgNO3andNa2SO4:\rmAgN\rmO_3\;\rmand N\rma_\rm2\rmS\rmO_\rm4:AgNO3​andNa2​SO4​:

The initial concentration of \left< \rmA\rmg^ + \right> ions in AgNO3\rmAgN\rmO_3AgNO3​is given below:

initial=5.0mL×0.40mmolAgNO3mL×1molAg+1molAgNO3(150.0+5.0)mL=0.0129M\beginarrayc\\\left< \rmA\rmg^ + \right>_\rminitial = \frac5.0\rmmL \times \frac\rm0\rm.40mmol AgN\rmO_3\rmmL \times \frac1\rm mol A\rmg^ + 1\rm mol AgN\rmO_3\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.0129\rmM\\\endarrayinitial​=(150.0+5.0)mL5.0mL×mL0.40mmolAgNO3​​×1molAgNO3​1molAg+​​=0.0129M​

The initial concentration of \left< \rmSO_4^2 - \right> ions in Na2SO4\rmN\rma_\rm2\rmS\rmO_\rm4Na2​SO4​is given below:

initial=150.0mL×0.10mmolNa2SO4mL×1molSO42−1molNa2SO4(150.0+5.0)mL=0.0968M\beginarrayc\\\left< \rmSO_\rm4^\rm2 - \right>_\rminitial = \frac150.0\rmmL \times \frac\rm0\rm.10mmol N\rma_\rm2\rmS\rmO_\rm4\rmmL \times \frac1\rm mol SO_4^2 - 1\rm mol N\rma_\rm2\rmS\rmO_\rm4\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.0968\rmM\\\endarrayinitial​=(150.0+5.0)mL150.0mL×mL0.10mmolNa2​SO4​​×1molNa2​SO4​1molSO42−​​​=0.0968M​

The ionic product of Ag2SO3\rmA\rmg_\rm2\rmS\rmO_\rm3Ag2​SO3​is given below:

KIP=initial2initial=(0.0129)2(0.0968)=1.6×10−5\beginarrayc\\\rmK_\rmIP = \left< \rmA\rmg^ + \right>_\rminitial^2\left< \rmSO_4^2 - \right>_\rminitial\\\\ = \left( 0.0129 \right)^2\left( 0.0968 \right)\\\\ = 1.6 \times 10^ - 5\\\endarrayKIP​=initial2​initial​=(0.0129)2(0.0968)=1.6×10−5​

The ionic product (KIP)\left( \rmK_\rmIP \right)(KIP​) is greater than the solubility product (Ksp)\left( \rmK_\rmsp \right)(Ksp​),

KIP>Ksp⇒precipitationtakesplace\rmK_\rmIP > \rmK_\rmsp \Rightarrow \rmprecipitation takes placeKIP​>Ksp​⇒precipitationtakesplace

The balanced equation for the reaction of AgNO3andNa2SO4:\rmAgN\rmO_3\;\rmand N\rma_\rm2\rmS\rmO_\rm4:AgNO3​andNa2​SO4​:

The initial concentration of \left< \rmA\rmg^ + \right> ions in AgNO3\rmAgN\rmO_3AgNO3​is given below:

initial=5.0mL×0.50mmolAgNO3mL×1molAg+1molAgNO3(150.0+5.0)mL=0.0161M\beginarrayc\\\left< \rmA\rmg^ + \right>_\rminitial = \frac5.0\rmmL \times \frac\rm0\rm.50mmol AgN\rmO_3\rmmL \times \frac1\rm mol A\rmg^ + 1\rm mol AgN\rmO_3\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.0161\rmM\\\endarrayinitial​=(150.0+5.0)mL5.0mL×mL0.50mmolAgNO3​​×1molAgNO3​1molAg+​​=0.0161M​

The initial concentration of \left< \rmSO_4^2 - \right> ions in Na2SO4\rmN\rma_\rm2\rmS\rmO_\rm4Na2​SO4​is given below:

initial=150.0mL×0.10mmolNa2SO4mL×1molSO42−1molNa2SO4(150.0+5.0)mL=0.0968M\beginarrayc\\\left< \rmSO_\rm4^\rm2 - \right>_\rminitial = \frac150.0\rmmL \times \frac\rm0\rm.10mmol N\rma_\rm2\rmS\rmO_\rm4\rmmL \times \frac1\rm mol SO_4^2 - 1\rm mol N\rma_\rm2\rmS\rmO_\rm4\left( 150.0 + 5.0 \right)\rmmL\\\\ = 0.0968\rmM\\\endarrayinitial​=(150.0+5.0)mL150.0mL×mL0.10mmolNa2​SO4​​×1molNa2​SO4​1molSO42−​​​=0.0968M​

The ionic product of Ag2SO3\rmA\rmg_\rm2\rmS\rmO_\rm3Ag2​SO3​is given below:

KIP=initial2initial=(0.0161)2(0.0968)=2.5×10−5\beginarrayc\\\rmK_\rmIP = \left< \rmA\rmg^ + \right>_\rminitial^2\left< \rmSO_4^2 - \right>_\rminitial\\\\ = \left( 0.0161 \right)^2\left( 0.0968 \right)\\\\ = 2.5 \times 10^ - 5\\\endarrayKIP​=initial2​initial​=(0.0161)2(0.0968)=2.5×10−5​

The ionic product (KIP)\left( \rmK_\rmIP \right)(KIP​) is greater than the solubility product(Ksp)\left( \rmK_\rmsp \right)(Ksp​),

KIP>Ksp⇒precipitationtakesplace\rmK_\rmIP > \rmK_\rmsp \Rightarrow \rmprecipitation takes placeKIP​>Ksp​⇒precipitationtakesplace

Ans:

For the mixture, 150.0mLof0.10MNa2SO4(aq)and5.0mLof0.20MAgNO3(aq)\rm150\rm.0mL of 0\rm.10 M N\rma_\rm2\rmS\rmO_\rm4\left( \rmaq \right)\rm and 5\rm.0 mL of 0\rm.20 M AgN\rmO_\rm3\left( \rmaq \right)150.0mLof0.10MNa2​SO4​(aq)and5.0mLof0.20MAgNO3​(aq) precipitation does not take place.

For the mixture, 150.0mLof0.10MNa2SO4(aq)and5.0mLof0.30MAgNO3(aq)\rm150\rm.0mL of 0\rm.10 M N\rma_\rm2\rmS\rmO_\rm4\left( \rmaq \right)\rm and 5\rm.0 mL of 0\rm.30 M AgN\rmO_\rm3\left( \rmaq \right)150.0mLof0.10MNa2​SO4​(aq)and5.0mLof0.30MAgNO3​(aq) precipitation does not take place.

For the mixture, 150.0mLof0.10MNa2SO4(aq)and5.0mLof0.40MAgNO3(aq)\rm150\rm.0mL of 0\rm.10 M N\rma_\rm2\rmS\rmO_\rm4\left( \rmaq \right)\rm and 5\rm.0 mL of 0\rm.40 M AgN\rmO_\rm3\left( \rmaq \right)150.0mLof0.10MNa2​SO4​(aq)and5.0mLof0.40MAgNO3​(aq) precipitation takes place.

See more: New Song Every Other Day / Day 143 / Booze Me Up And Get Me High Lyrics

For the mixture, 150.0mLof0.10MNa2SO4(aq)and5.0mLof0.50MAgNO3(aq)\rm150\rm.0mL of 0\rm.10 M N\rma_\rm2\rmS\rmO_\rm4\left( \rmaq \right)\rm and 5\rm.0 mL of 0\rm.50 M AgN\rmO_\rm3\left( \rmaq \right)150.0mLof0.10MNa2​SO4​(aq)and5.0mLof0.50MAgNO3​(aq) precipitation takes place.