Concepts and reason
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 asK s p {{\rm{K}}_{{\rm{sp}}}} K s p . 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.
Fundamentals
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 A g 2 S O 4 {\rm{A}}{{\rm{g}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_4} A g 2 S O 4
The equilibrium equation for the ionic compound is given below:
Therefore, the solubility product of the ionic compound is
K s p = [ A g + ] 2 [ S O 4 2 − ] = 1 . 2 × 1 0 − 5 \begin{array}{c}\\{{\rm{K}}_{{\rm{sp}}}}\,{\rm{ = }}\,{\left[ {{\rm{A}}{{\rm{g}}^{\rm{ + }}}} \right]^{\rm{2}}}\left[ {{\rm{SO}}_4^{2 - }} \right]\\\\ = 1.2 \times {10^{ - 5}}\\\end{array} K s p = [ A g + ] 2 [ S O 4 2 − ] = 1 . 2 × 1 0 − 5
The balanced equation for the reaction of A g N O 3 a n d N a 2 S O 4 : {\rm{AgN}}{{\rm{O}}_3}\;{\rm{and N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}: A g N O 3 a n d N a 2 S O 4 :
The initial concentration of [ A g + ] \left[ {{\rm{A}}{{\rm{g}}^ + }} \right] [ A g + ] ions in A g N O 3 {\rm{AgN}}{{\rm{O}}_3} A g N O 3 is given below:
[ A g + ] i n i t i a l = 5 . 0 m L × 0 . 2 0 m m o l A g N O 3 m L × 1 m o l A g + 1 m o l A g N O 3 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 0 6 4 5 M \begin{array}{c}\\{\left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}} = \frac{{5.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.20mmol AgN}}{{\rm{O}}_3}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol A}}{{\rm{g}}^ + }}}{{1{\rm{ mol AgN}}{{\rm{O}}_3}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.00645{\rm{M}}\\\end{array} [ A g + ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 5 . 0 m L × m L 0 . 2 0 m m o l A g N O 3 × 1 m o l A g N O 3 1 m o l A g + = 0 . 0 0 6 4 5 M
The initial concentration of [ S O 4 2 − ] \left[ {{\rm{SO}}_4^{2 - }} \right] [ S O 4 2 − ] ions in N a 2 S O 4 {\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}} N a 2 S O 4 is given below:
[ S O 4 2 − ] i n i t i a l = 1 5 0 . 0 m L × 0 . 1 0 m m o l N a 2 S O 4 m L × 1 m o l S O 4 2 − 1 m o l N a 2 S O 4 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 9 6 8 M \begin{array}{c}\\{\left[ {{\rm{SO}}_{\rm{4}}^{{\rm{2 - }}}} \right]_{{\rm{initial}}}} = \frac{{150.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.10mmol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol }}SO_4^{2 - }}}{{1{\rm{ mol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.0968{\rm{M}}\\\end{array} [ S O 4 2 − ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 1 5 0 . 0 m L × m L 0 . 1 0 m m o l N a 2 S O 4 × 1 m o l N a 2 S O 4 1 m o l S O 4 2 − = 0 . 0 9 6 8 M
The ionic product of A g 2 S O 3 {\rm{A}}{{\rm{g}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{3}}} A g 2 S O 3 is given below:
K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 0 6 4 5 ) 2 ( 0 . 0 9 6 8 ) = 4 . 0 × 1 0 − 6 \begin{array}{c}\\{{\rm{K}}_{{\rm{IP}}}} = \left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}^2{\left[ {{\rm{SO}}_4^{2 - }} \right]_{{\rm{initial}}}}\\\\ = {\left( {0.00645} \right)^2}\left( {0.0968} \right)\\\\ = 4.0 \times {10^{ - 6}}\\\end{array} K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 0 6 4 5 ) 2 ( 0 . 0 9 6 8 ) = 4 . 0 × 1 0 − 6
The ionic product ( K I P ) \left( {{{\rm{K}}_{{\rm{IP}}}}} \right) ( K I P ) is less than the solubility product ( K s p ) \left( {{{\rm{K}}_{{\rm{sp}}}}} \right) ( K s p ) ,
K I P < K s p ⇒ p r e c i p i t a t i o n d o e s n o t t a k e s p l a c e {{\rm{K}}_{{\rm{IP}}}} < {{\rm{K}}_{{\rm{sp}}}} \Rightarrow {\rm{precipitation does not takes place}} K I P < K s p ⇒ p r e c i p i t a t i o n d o e s n o t t a k e s p l a c e
The balanced equation for the reaction of A g N O 3 a n d N a 2 S O 4 : {\rm{AgN}}{{\rm{O}}_3}\;{\rm{and N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}: A g N O 3 a n d N a 2 S O 4 :
The initial concentration of [ A g + ] \left[ {{\rm{A}}{{\rm{g}}^ + }} \right] [ A g + ] ions in A g N O 3 {\rm{AgN}}{{\rm{O}}_3} A g N O 3 is given below:
[ A g + ] i n i t i a l = 5 . 0 m L × 0 . 3 0 m m o l A g N O 3 m L × 1 m o l A g + 1 m o l A g N O 3 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 0 9 6 8 M \begin{array}{c}\\{\left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}} = \frac{{5.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.30mmol AgN}}{{\rm{O}}_3}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol A}}{{\rm{g}}^ + }}}{{1{\rm{ mol AgN}}{{\rm{O}}_3}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.00968{\rm{M}}\\\end{array} [ A g + ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 5 . 0 m L × m L 0 . 3 0 m m o l A g N O 3 × 1 m o l A g N O 3 1 m o l A g + = 0 . 0 0 9 6 8 M
The initial concentration of [ S O 4 2 − ] \left[ {{\rm{SO}}_4^{2 - }} \right] [ S O 4 2 − ] ions in N a 2 S O 4 {\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}} N a 2 S O 4 is given below:
[ S O 4 2 − ] i n i t i a l = 1 5 0 . 0 m L × 0 . 1 0 m m o l N a 2 S O 4 m L × 1 m o l S O 4 2 − 1 m o l N a 2 S O 4 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 9 6 8 M \begin{array}{c}\\{\left[ {{\rm{SO}}_{\rm{4}}^{{\rm{2 - }}}} \right]_{{\rm{initial}}}} = \frac{{150.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.10mmol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol }}SO_4^{2 - }}}{{1{\rm{ mol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.0968{\rm{M}}\\\end{array} [ S O 4 2 − ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 1 5 0 . 0 m L × m L 0 . 1 0 m m o l N a 2 S O 4 × 1 m o l N a 2 S O 4 1 m o l S O 4 2 − = 0 . 0 9 6 8 M
The ionic product of A g 2 S O 3 {\rm{A}}{{\rm{g}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{3}}} A g 2 S O 3 is given below:
K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 0 9 6 8 ) 2 ( 0 . 0 9 6 8 ) = 9 . 1 × 1 0 − 6 \begin{array}{c}\\{{\rm{K}}_{{\rm{IP}}}} = \left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}^2{\left[ {{\rm{SO}}_4^{2 - }} \right]_{{\rm{initial}}}}\\\\ = {\left( {0.00968} \right)^2}\left( {0.0968} \right)\\\\ = 9.1 \times {10^{ - 6}}\\\end{array} K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 0 9 6 8 ) 2 ( 0 . 0 9 6 8 ) = 9 . 1 × 1 0 − 6
The ionic product ( K I P ) \left( {{{\rm{K}}_{{\rm{IP}}}}} \right) ( K I P ) is less than the solubility product( K s p ) \left( {{{\rm{K}}_{{\rm{sp}}}}} \right) ( K s p ) ,
K I P < K s p ⇒ p r e c i p i t a t i o n d o e s n o t t a k e s p l a c e {{\rm{K}}_{{\rm{IP}}}} < {{\rm{K}}_{{\rm{sp}}}} \Rightarrow {\rm{precipitation does not takes place}} K I P < K s p ⇒ p r e c i p i t a t i o n d o e s n o t t a k e s p l a c e
The balanced equation for the reaction of A g N O 3 a n d N a 2 S O 4 : {\rm{AgN}}{{\rm{O}}_3}\;{\rm{and N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}: A g N O 3 a n d N a 2 S O 4 :
The initial concentration of [ A g + ] \left[ {{\rm{A}}{{\rm{g}}^ + }} \right] [ A g + ] ions in A g N O 3 {\rm{AgN}}{{\rm{O}}_3} A g N O 3 is given below:
[ A g + ] i n i t i a l = 5 . 0 m L × 0 . 4 0 m m o l A g N O 3 m L × 1 m o l A g + 1 m o l A g N O 3 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 1 2 9 M \begin{array}{c}\\{\left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}} = \frac{{5.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.40mmol AgN}}{{\rm{O}}_3}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol A}}{{\rm{g}}^ + }}}{{1{\rm{ mol AgN}}{{\rm{O}}_3}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.0129{\rm{M}}\\\end{array} [ A g + ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 5 . 0 m L × m L 0 . 4 0 m m o l A g N O 3 × 1 m o l A g N O 3 1 m o l A g + = 0 . 0 1 2 9 M
The initial concentration of [ S O 4 2 − ] \left[ {{\rm{SO}}_4^{2 - }} \right] [ S O 4 2 − ] ions in N a 2 S O 4 {\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}} N a 2 S O 4 is given below:
[ S O 4 2 − ] i n i t i a l = 1 5 0 . 0 m L × 0 . 1 0 m m o l N a 2 S O 4 m L × 1 m o l S O 4 2 − 1 m o l N a 2 S O 4 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 9 6 8 M \begin{array}{c}\\{\left[ {{\rm{SO}}_{\rm{4}}^{{\rm{2 - }}}} \right]_{{\rm{initial}}}} = \frac{{150.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.10mmol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol }}SO_4^{2 - }}}{{1{\rm{ mol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.0968{\rm{M}}\\\end{array} [ S O 4 2 − ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 1 5 0 . 0 m L × m L 0 . 1 0 m m o l N a 2 S O 4 × 1 m o l N a 2 S O 4 1 m o l S O 4 2 − = 0 . 0 9 6 8 M
The ionic product of A g 2 S O 3 {\rm{A}}{{\rm{g}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{3}}} A g 2 S O 3 is given below:
K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 1 2 9 ) 2 ( 0 . 0 9 6 8 ) = 1 . 6 × 1 0 − 5 \begin{array}{c}\\{{\rm{K}}_{{\rm{IP}}}} = \left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}^2{\left[ {{\rm{SO}}_4^{2 - }} \right]_{{\rm{initial}}}}\\\\ = {\left( {0.0129} \right)^2}\left( {0.0968} \right)\\\\ = 1.6 \times {10^{ - 5}}\\\end{array} K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 1 2 9 ) 2 ( 0 . 0 9 6 8 ) = 1 . 6 × 1 0 − 5
The ionic product ( K I P ) \left( {{{\rm{K}}_{{\rm{IP}}}}} \right) ( K I P ) is greater than the solubility product ( K s p ) \left( {{{\rm{K}}_{{\rm{sp}}}}} \right) ( K s p ) ,
K I P > K s p ⇒ p r e c i p i t a t i o n t a k e s p l a c e {{\rm{K}}_{{\rm{IP}}}} > {{\rm{K}}_{{\rm{sp}}}} \Rightarrow {\rm{precipitation takes place}} K I P > K s p ⇒ p r e c i p i t a t i o n t a k e s p l a c e
The balanced equation for the reaction of A g N O 3 a n d N a 2 S O 4 : {\rm{AgN}}{{\rm{O}}_3}\;{\rm{and N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}: A g N O 3 a n d N a 2 S O 4 :
The initial concentration of [ A g + ] \left[ {{\rm{A}}{{\rm{g}}^ + }} \right] [ A g + ] ions in A g N O 3 {\rm{AgN}}{{\rm{O}}_3} A g N O 3 is given below:
[ A g + ] i n i t i a l = 5 . 0 m L × 0 . 5 0 m m o l A g N O 3 m L × 1 m o l A g + 1 m o l A g N O 3 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 1 6 1 M \begin{array}{c}\\{\left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}} = \frac{{5.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.50mmol AgN}}{{\rm{O}}_3}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol A}}{{\rm{g}}^ + }}}{{1{\rm{ mol AgN}}{{\rm{O}}_3}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.0161{\rm{M}}\\\end{array} [ A g + ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 5 . 0 m L × m L 0 . 5 0 m m o l A g N O 3 × 1 m o l A g N O 3 1 m o l A g + = 0 . 0 1 6 1 M
The initial concentration of [ S O 4 2 − ] \left[ {{\rm{SO}}_4^{2 - }} \right] [ S O 4 2 − ] ions in N a 2 S O 4 {\rm{N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}} N a 2 S O 4 is given below:
[ S O 4 2 − ] i n i t i a l = 1 5 0 . 0 m L × 0 . 1 0 m m o l N a 2 S O 4 m L × 1 m o l S O 4 2 − 1 m o l N a 2 S O 4 ( 1 5 0 . 0 + 5 . 0 ) m L = 0 . 0 9 6 8 M \begin{array}{c}\\{\left[ {{\rm{SO}}_{\rm{4}}^{{\rm{2 - }}}} \right]_{{\rm{initial}}}} = \frac{{150.0{\rm{mL}} \times \frac{{{\rm{0}}{\rm{.10mmol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}{{{\rm{mL}}}} \times \frac{{1{\rm{ mol }}SO_4^{2 - }}}{{1{\rm{ mol N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}}}}}{{\left( {150.0 + 5.0} \right){\rm{mL}}}}\\\\ = 0.0968{\rm{M}}\\\end{array} [ S O 4 2 − ] i n i t i a l = ( 1 5 0 . 0 + 5 . 0 ) m L 1 5 0 . 0 m L × m L 0 . 1 0 m m o l N a 2 S O 4 × 1 m o l N a 2 S O 4 1 m o l S O 4 2 − = 0 . 0 9 6 8 M
The ionic product of A g 2 S O 3 {\rm{A}}{{\rm{g}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{3}}} A g 2 S O 3 is given below:
K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 1 6 1 ) 2 ( 0 . 0 9 6 8 ) = 2 . 5 × 1 0 − 5 \begin{array}{c}\\{{\rm{K}}_{{\rm{IP}}}} = \left[ {{\rm{A}}{{\rm{g}}^ + }} \right]_{{\rm{initial}}}^2{\left[ {{\rm{SO}}_4^{2 - }} \right]_{{\rm{initial}}}}\\\\ = {\left( {0.0161} \right)^2}\left( {0.0968} \right)\\\\ = 2.5 \times {10^{ - 5}}\\\end{array} K I P = [ A g + ] i n i t i a l 2 [ S O 4 2 − ] i n i t i a l = ( 0 . 0 1 6 1 ) 2 ( 0 . 0 9 6 8 ) = 2 . 5 × 1 0 − 5
The ionic product ( K I P ) \left( {{{\rm{K}}_{{\rm{IP}}}}} \right) ( K I P ) is greater than the solubility product( K s p ) \left( {{{\rm{K}}_{{\rm{sp}}}}} \right) ( K s p ) ,
K I P > K s p ⇒ p r e c i p i t a t i o n t a k e s p l a c e {{\rm{K}}_{{\rm{IP}}}} > {{\rm{K}}_{{\rm{sp}}}} \Rightarrow {\rm{precipitation takes place}} K I P > K s p ⇒ p r e c i p i t a t i o n t a k e s p l a c e
Ans:
For the mixture, 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 2 0 M A g N O 3 ( a q ) {\rm{150}}{\rm{.0mL of 0}}{\rm{.10 M N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\left( {{\rm{aq}}} \right){\rm{ and 5}}{\rm{.0 mL of 0}}{\rm{.20 M AgN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right) 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 2 0 M A g N O 3 ( a q ) precipitation does not take place.
For the mixture, 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 3 0 M A g N O 3 ( a q ) {\rm{150}}{\rm{.0mL of 0}}{\rm{.10 M N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\left( {{\rm{aq}}} \right){\rm{ and 5}}{\rm{.0 mL of 0}}{\rm{.30 M AgN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right) 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 3 0 M A g N O 3 ( a q ) precipitation does not take place.
For the mixture, 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 4 0 M A g N O 3 ( a q ) {\rm{150}}{\rm{.0mL of 0}}{\rm{.10 M N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\left( {{\rm{aq}}} \right){\rm{ and 5}}{\rm{.0 mL of 0}}{\rm{.40 M AgN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right) 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 4 0 M A g N O 3 ( a q ) precipitation takes place.
For the mixture, 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 5 0 M A g N O 3 ( a q ) {\rm{150}}{\rm{.0mL of 0}}{\rm{.10 M N}}{{\rm{a}}_{\rm{2}}}{\rm{S}}{{\rm{O}}_{\rm{4}}}\left( {{\rm{aq}}} \right){\rm{ and 5}}{\rm{.0 mL of 0}}{\rm{.50 M AgN}}{{\rm{O}}_{\rm{3}}}\left( {{\rm{aq}}} \right) 1 5 0 . 0 m L o f 0 . 1 0 M N a 2 S O 4 ( a q ) a n d 5 . 0 m L o f 0 . 5 0 M A g N O 3 ( a q ) precipitation takes place.