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Entry Task: March 5 th Tuesday. Question: Calculate the solubility of AgI in water in moles per liter given its K sp value of 8.3 x 10 -17 .
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Entry Task: March 5th Tuesday Question: Calculate the solubility of AgI in water in moles per liter given its Ksp value of 8.3 x 10-17. A saturated solution of AgI also containing NaI is found to have an iodide ion concentration of 0.020 M. What is the concentration of silver ions? You have 10 minutes
Agenda: • Discuss Solubility, Precipitation and Ions ws • Major self-check on content so far & discuss it • HW: Pre-lab Determine Ksp
CaC2O4(s) Ca2+(aq) + C2O42-(aq) 17.6- Precipitation and Separation of Ions 17.37 A 1.00L solution is saturated at 25°C with calcium oxalate, CaC2O4, is evaporated to dryness, giving a 0.0061 g residue of CaC2O4. Calculate the solubility-product constant for this salt. Calculate the molarity 0.0061g/127.99 = 4.77 x10-5M of CaC2O4 Ksp= [4.77 x10-5][4.77 x10-5] Ksp= 2.3 x10-9
Mn(OH)2(s) Mn2+(aq) + 2OH1-(aq) 17.6- Precipitation and Separation of Ions 17.41 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at (a) at pH of 7.0; pH of 7 means there are 1.0 x10-7 OH ions 1.6x10-13= [x][1.0 x10-7]2 1.6x10-13 = [x] 1.0 x10-14 The molarity is 16M (16)(1 L) = 16 moles * 89 = • 1424 or 1.4 x103g/ liter
Mn(OH)2(s) Mn2+(aq) + 2OH1-(aq) 17.6- Precipitation and Separation of Ions 17.41 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at (b) at pH of 9.5; pH of 9.5= pOH 4.5 means there are 3.2 x10-5 OH ions 1.6x10-13= [x][3.2 x10-5]2 1.6x10-13 = [x] 1.0 x10-9 The molarity is 1.6x10-4M (1.6x10-4)(1 L) = 1.6x10-4 moles * 89 = • 1.4x10-2g/ liter
Mn(OH)2(s) Mn2+(aq) + 2OH1-(aq) 17.6- Precipitation and Separation of Ions 17.41 Calculate the solubility of Mn(OH)2 in grams per liter when buffered at (c) at pH of 11.8; pH of 11.8= pOH 2.2 means there are 6.3 x10-3 OH ions 1.6x10-13= [x][6.3 x10-3]2 1.6x10-13 = [x] 3.98 x10-5 The molarity is 4.02x10-9M (4.02x10-9)(1 L) = 4.02x10-9 moles * 89 = • 3.6x10-7g/ liter
17.6- Precipitation and Separation of Ions 17.49 (a) Will Ca(OH)2 precipitate from solution if the pH of a 0.050M solution of CaCl2 is adjusted to 8.0? Ksp= 6.5x10-6= [Ca+]OH-]2 pH of 8 = pOH of 6 = 1.0x10-6M of OH Q = [0.050]1.0x10-6]2 Q = 5.0 x 10-14 Ksp = 6.5 x 10-6 Ksp is bigger meaning no precipitate
17.6- Precipitation and Separation of Ions 17.49 (b) Will Ag2SO4 precipitate when 100 ml of 0.050M AgNO3 is mixed with 10 mls of 5.0 x10-2M NaSO4 solution? In 0.100 L of 0.050 MAgNO3 there are (0.100 L) (0.050M) = 5.0 x 10-3 moles of Ag+1 ions
17.6- Precipitation and Separation of Ions 17.49 (b) Will Ag2SO4 precipitate when 100 ml of 0.050M AgNO3 is mixed with 10 mls of 5.0 x10-2M Na2SO4solution? In 0.010 L of 5.0 x10-2MNaNO3 there are (0.010 L) (5.0 x10-2M) = 5.0 x 10-4 moles of SO4-2 ions
17.6- Precipitation and Separation of Ions 17.49 (b) Will Ag2SO4 precipitate when 100 ml of 0.050M AgNO3 is mixed with 10 mls of 5.0 x10-2M Na2SO4solution? • We have to convert the moles in to molarity but use the combined volume. 5.0 x 10-3 moles of Ag+1 ions 5.0 x 10-4 moles of SO4-2 ions
17.6- Precipitation and Separation of Ions 17.49 (b) Will Ag2SO4 precipitate when 100 ml of 0.050M AgNO3 is mixed with 10 mls of 5.0 x10-2M Na2SO4solution? • We have to convert the moles in to molarity but use the combined volume. 5.0 x10-3 moles/0.110L = • 4.55 x10-2M of Ag+1 ions 5.0 x10-4 moles/0.110L = 4.55 x10-3M of SO4-2 ions Substitute the values into the Ksp expression and solve for Q
17.6- Precipitation and Separation of Ions 17.49 (b) Will Ag2SO4 precipitate when 100 ml of 0.050M AgNO3 is mixed with 10 mls of 5.0 x10-2M Na2SO4solution? Q = [Ag+]2[SO42] • 9.4 106 (4.55 x10-2)2(4.55 x10-3) = • Q= 9.4 106 Ksp= 1.5 x 10-5 • Q is smaller than Ksp that means • No precipitate will occur
17.6- Precipitation and Separation of Ions 17. 53 A solution contains 2.0 x10-4M Ag+ and 1.5 x 10-3 M Pb+2. If NaI is added, will AgI (Ksp= 8.3x10-17) or PbI2 (Ksp= 7.9 x10-9) precipitate first? Specify the concentration of I- needed to begin precipitation.
17.6- Precipitation and Separation of Ions 17. 53 A solution contains 2.0x10-4M Ag+ and 1.5 x 10-3 M Pb+2. If NaI is added, will AgI (Ksp= 8.3x10-17) or PbI2 (Ksp= 7.9 x10-9) precipitate first? Specify the concentration of I- needed to begin precipitation. Lets look at Ag+ with I-: Ksp = [Ag+][l-] 8.3 x10-17 = (2.0 x10-4)(x) = l- ions 8.3 x10-17= 2.0 x10-4 4.2 x 10-13 l- ions
17.6- Precipitation and Separation of Ions 17. 53 A solution contains 2.0x10-4M Ag+ and 1.5 x 10-3 M Pb+2. If NaI is added, will AgI (Ksp= 8.3x10-17) or PbI2 (Ksp= 7.9 x10-9) precipitate first? Specify the concentration of I- needed to begin precipitation. Lets look at Pb+2 with I-: Ksp = [Pb+][l-]2 7.9 x10-9 = (1.5 x 10-3)(x)2 = l- ions 7.9 x10-9 = 1.5 x 10-3 x2=5.3 x 10-6 l- ions x=2.3 x 10-3 l- ions
17.6- Precipitation and Separation of Ions 17. 53 A solution contains 2.0x10-4M Ag+ and 1.5 x 10-3 M Pb+2. If NaI is added, will AgI (Ksp= 8.3x10-17) or PbI2 (Ksp= 7.9 x10-9) precipitate first? Specify the concentration of I- needed to begin precipitation. Which concentration is smaller? 4.2 x 10-13l- ions with Ag+ 2.3 x 10-3 l- ions- ions with Pb+2 This means that it will Agl precipitate as such a small concentration verses Pbl2.