Solubility & Equilibrium K sp

Solubility & Equilibrium The beginning XY (s) ==> X + + Y - The beginning XY (s) ==> X + + Y -

Solubility & Equilibrium The beginning XY (s) ==> X + + Y - As time continues the [ions] begins to increase. The beginning XY (s) ==> X + + Y - As time continues the [ions] begins to increase.

Solubility & Equilibrium Greater the chance that they will collide and reform XY (s) <== X + + Y - When it becomes saturated it reaches equilibrium. XY (s) X + + Y - Greater the chance that they will collide and reform XY (s) <== X + + Y - When it becomes saturated it reaches equilibrium. XY (s) X + + Y -

Solubility & Equilibrium Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y  Solubility = molar solubility = mol/L Be careful ~ sometimes given g/L or have to solve for g/L Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y  Solubility = molar solubility = mol/L Be careful ~ sometimes given g/L or have to solve for g/L

Solubility & Equilibrium Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 1) Just ions, no solids Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 1) Just ions, no solids

Solubility & Equilibrium Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 2) It doesn’t matter if you have stuff on the bottom. Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 2) It doesn’t matter if you have stuff on the bottom.

Solubility & Equilibrium Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 3) Not solubility - that’s an equilibrium position(Q) (will more dissolve or not?) Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 3) Not solubility - that’s an equilibrium position(Q) (will more dissolve or not?)

Solubility & Equilibrium Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 4) Equilibrium so remember ICE Equilibrium Constant for Solubility-K sp K sp = [X + ] x [Y - ] y 4) Equilibrium so remember ICE

K sp Calculations The solubility of copper (I) bromide is 2.0 x mol/L at 25 C. Calculate K sp.

K sp Calculations The solubility of copper(I) bromide is 2.0 x mol/L at 25°C. Calculate K sp. CuBr(s) Cu +1 + Br -1 I 0 0 C + x + x E 2.0 x x The solubility of copper(I) bromide is 2.0 x mol/L at 25°C. Calculate K sp. CuBr(s) Cu +1 + Br -1 I 0 0 C + x + x E 2.0 x x 10 -4

K sp Calculations The solubility of copper(I) bromide is 2.0 x mol/L at 25°C. Calculate K sp. CuBr(s) Cu +1 + Br -1 Ksp = [2.0 x10 -4 ][2.0 x ] = 4.0 x (no units for K) The solubility of copper(I) bromide is 2.0 x mol/L at 25°C. Calculate K sp. CuBr(s) Cu +1 + Br -1 Ksp = [2.0 x10 -4 ][2.0 x ] = 4.0 x (no units for K)

K sp Calculations – Your Turn The solubility of silver phosphate is 1.60 x M. Calculate its K sp.

K sp Calculations The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I

K sp Calculations The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I00 C The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I00 C

K sp Calculations The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I00 C +x +2x E The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I00 C +x +2x E

K sp Calculations The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I00 C +x +2x E +x +2x The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - I00 C +x +2x E +x +2x

Ksp Calculations The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2

Ksp Calculations The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] 2 The K sp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] 2

Ksp Calculations The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] x = [x][2x] 2 The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] x = [x][2x] 2

Ksp Calculations The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] x = [x][2x] x = 4x 3 The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] x = [x][2x] x = 4x 3

Ksp Calculations The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] x = [x][2x] x = 4x 3 x = 3.3 x mol/L The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - Ksp = [Cu +2 ][IO 3 - ] 2 Ksp = [x][2x] x = [x][2x] x = 4x 3 x = 3.3 x mol/L

Ksp Calculations The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - [Cu +2 ]= 3.3 x mol/L [IO 3 - ]=2(3.3 x mol/L) = 6.6 x mol/L The Ksp value of copper(II) iodate is 1.4 x at 25°C. Calculate its solubility. Cu(IO 3 ) 2(s) Cu IO 3 - [Cu +2 ]= 3.3 x mol/L [IO 3 - ]=2(3.3 x mol/L) = 6.6 x mol/L

Ksp Calculations – Your Turn The Ksp of mercury (II) sulfide is 1.6 x Find its molar solubility.

Ksp Calculations What does it all mean? According to K sp, EVERYTHING is at least very, very, very, very slightly soluble. Looking at the K sp can help you figure out the solubility of compounds compared to each other – with a couple key rules about doing it! What does it all mean? According to K sp, EVERYTHING is at least very, very, very, very slightly soluble. Looking at the K sp can help you figure out the solubility of compounds compared to each other – with a couple key rules about doing it!

Ksp Calculations What does it all mean? 1)Salts that produce the same # of ions can be compared to see which one is the most/least soluble. AgBrvsAgIvsAgCl Ksp values 5.0x x x Appendix A25 What does it all mean? 1)Salts that produce the same # of ions can be compared to see which one is the most/least soluble. AgBrvsAgIvsAgCl Ksp values 5.0x x x Appendix A25

Ksp Calculations What does it all mean? 2)If the salts break into different # of ions, you can’t just look. Must calculate. What does it all mean? 2)If the salts break into different # of ions, you can’t just look. Must calculate.

Ksp Calculations 2 example problems: Which is more soluble: copper (II) carbonate or cadmium carbonate? Ksp = 2.5 x Ksp = 5.2 x example problems: Which is more soluble: copper (II) carbonate or cadmium carbonate? Ksp = 2.5 x Ksp = 5.2 x

Ksp Calculations 2 example problems: Which is more soluble: tin (II) hydroxide or strontium phosphate? Ksp = 3.0 x Ksp = 1.0 x example problems: Which is more soluble: tin (II) hydroxide or strontium phosphate? Ksp = 3.0 x Ksp = 1.0 x