{/eq}, c. {eq}AgCN; K_{sp} = 5.97 \times 10^{-17} a. BaCrO4; molar solubility = 1.08 * 10-5 M b. Ag2SO3; molar solubility = 1.55 * 10-5 M c. Pd(SCN)2; molar solubility … Get the detailed answer: What is the molar solubility of AgI in pure water? Answer to: Which of the following compounds will have the highest molar solubility in pure water? Also, there are teachers that insist on units for the Ksp. 1.12 x 10-8 c. 8.00… The ammonium phosphate polyatomic ion, NH4PO42¯, is an uncommon one. 1) The dissociation equation and the Ksp expression: Remember, this is the answer because the dissolved ions and the solid are also in a one-to-one molar ratio. Here the choice is lead (II) sulfate: a. The molar solubility is the number of moles that can be dissolved per liter of a solution until the solution becomes saturated. It could show up on the test! I do that by first assigning a variable, s, to the molar solubility of AgCl. Example #6: Calculate the [Ba2+] if the [SO42¯] = 0.0153 M. Ksp = 1.07 x 10¯10. Comment: it's important that you know how substances ionize. AgCl is easy, but you may not know that CuSCN (example #4) and silver azide (example #5) also ionize in a 1:1 molar ratio like AgCl. {/eq}. Warning: You may know lots of common ions but, in a problem like the one under discussion, you may get an unusual one thrown at you on the test. 3.7 million tough questions answered. This dissociates: Note how I ignored the s in (0.0153 + s). Solution for The molar solubility of Ag2S is 1.26 x 10-16 mol L-1 in pure water. Do not tell them that some guy (me!) One last thing. Sciences, Culinary Arts and Personal {eq}\boxed{PbSO_4; K_{sp} = 1.82 \times 10^{-5}} I have had lots of people in my classes take the square root of the x2 side, but not the other. Be prepared! Calculate the value of Ks under these conditions. 3) Keep in mind that the key point is the one-to-one ratio of the ions in solution. This problem has been solved! Calculating the molar solubility is left to the student. {/eq}, b. Use the given molar solubilities in pure water to calculate Ksp for each compound. Example #10: The molar solubility of Ba 3 (PO 4) 2 is 8.89 x 10¯ 9 M in pure water. Anything else makes the problem unworkable and that is not the intent of the question writer. By the way, the sulfate already present in solution came from some other sulfate-containing compound, say sodium sulfate, Na2SO4. K_{sp} = [A^{n+} ][X^{n-} ] {/eq}. An unsaturated solution is a solution in which all solute has dissolved. Mick H. asked • 04/20/18 Calculate the molar solubility of PbI2 (Ksp = 1.4x10^-8)in (a) Pure water (b) On 0.50 L of solution that contains 15.0 g of FeI3 . Thanks. Question: Which Of The Following Compounds Will Have The Highest Molar Solubility In Pure Water? {eq}MgCO_3; K_{sp} = 6.82 \times 10^{-6} The solubility of CaSO4 is measured and found to... Titration of a Strong Acid or a Strong Base, LeChatelier's Principle: Disruption and Re-Establishment of Equilibrium, Collision Theory: Definition & Significance, Gibbs Free Energy: Definition & Significance, The Common Ion Effect and Selective Precipitation, Acid-Base Buffers: Calculating the pH of a Buffered Solution, The pH Scale: Calculating the pH of a Solution, Buffer System in Chemistry: Definition & Overview, Ionic Equilibrium: Definition & Calculations, Dalton's Law of Partial Pressures: Calculating Partial & Total Pressures, What is Salt Hydrolysis? Study Guides. True or false? This is known as the molar solubility of the compound in water at a given temperature (usually 25 Celsius). Based on this 1:1 dissociation stoichiometry, the {eq}K_{sp} {/eq} expression in terms of the molar solubility in pure water "x", is written as: From this relation we see that the salt compound in the list with the highest {eq}K_{sp} {/eq} value, will have the highest molar solubility. Initial buret reading, ml 6.50me omi 18,0kme 2 Volume delivered, mL AV=Vr-V 17.35me 10. x = 0.0501x 17.35 x=o.oscoceam 10x=0.0501x 18.00 x20.9018M Part II. In a saturated aqueous solution of an ionic (salt) compound, there is a certain dissolved molarity of this compound present. Now, I look at the relationship between AgCl and Cl¯. Which of the following compounds will have the highest molar solubility in pure water? Calculate its solubility in moles per liter. That's because s is very small compared to 0.0153. 7) Now, we take the square root of both sides. The Ksp value does not have any units on it, but when you get to the value for s, be sure to put M (for molarity) on it. Booster Classes. Notice how I did not say 'saturated solution' in the problem. Services, Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations, Working Scholars® Bringing Tuition-Free College to the Community. So, the molar solubility of AgCl is 1.33 x 10¯5 moles per liter. Personalized courses, with or without credits. Example #2: Aluminum phosphate has a Ksp of 9.83 x 10¯21. See the answer. Data Concentration of the Na2S2O3 solution:_0.OSIM Part I. Molar Solubility in pure water Trial 2 Trial 1 Data 10.oone 10.oome Volume saturated Ca(IO3)2 titrated, mL | 17.85 me 24.some Final buret reading, ml (Sin becomes colorless.) Homework Help. Example #1: Silver chloride, AgCl, has a Ksp = 1.77 x 10¯10. A saturated solution is a solution in which the maximum amount of solute has been dissolved. Note azide, a fairly uncommon polyatomic ion. All other trademarks and copyrights are the property of their respective owners. a. The constituent ion concentrations that result from this molar solubility, have their solubility product described by a constant {eq}K_{sp} {/eq} at the same temperature. Get the detailed answer: What is the molar solubility of AgI in pure water? 3.78 x 10-12 b. Bonus Example: Magnesium ammonium phosphate, MgNH4PO4, Ksp = 2.5 x 10¯13. Your dashboard and recommendations. {eq}PbSO_4; K_{sp} = 1.82 \times 10^{-5} Ksp (AgI) = 8.51 × 10-17. The molar solubility of AgI is 9.0 x 10 -9 mol/L. I see that it is also a 1:1 molar ratio, leading me to this: I am now ready to substitute into the Ksp expression. Calculate the K sp for Ba 3 (PO 4) 2. Calculate the Ksp for Ag2S. 1) The compound in solution is BaSO4. Therefore we do not have to perform individual calculations for each compound. What is its molar solubility in pure water? © copyright 2003-2020 Study.com. {/eq}, e. {eq}NiS; K_{sp} = 3.00 \times 10^{-20} I hope I'm not too insulting when I emphasize both sides. 4) We have to reason out the values of the two guys on the right. - Definition & Examples, The Bronsted-Lowry and Lewis Definition of Acids and Bases, Determining Rate Equation, Rate Law Constant & Reaction Order from Experimental Data, Lewis Structures: Single, Double & Triple Bonds, Acid-Base Equilibrium: Calculating the Ka or Kb of a Solution, Precipitation Reactions: Predicting Precipitates and Net Ionic Equations, CLEP Natural Sciences: Study Guide & Test Prep, Middle School Life Science: Tutoring Solution, Holt McDougal Modern Chemistry: Online Textbook Help, Praxis Chemistry (5245): Practice & Study Guide, College Chemistry: Homework Help Resource, CSET Science Subtest II Chemistry (218): Practice & Study Guide, ISEB Common Entrance Exam at 13+ Geography: Study Guide & Test Prep, Holt Science Spectrum - Physical Science with Earth and Space Science: Online Textbook Help, Biological and Biomedical That's the value that I want to determine. In a saturated aqueous solution of an ionic (salt) compound, there is a certain dissolved molarity of this compound present. The Ksp for MgF2 is 6.4 x 10-9. The solubility of CaF 2 (molar mass 78.1) at 18°C is reported to be 1.6 mg per 100 mL of water. All of the salt compounds shown dissociate in a 1:1 ratio of ions. Ksp (AgI) = 8.51 × 10-17. The "A" is the metal cation portion and "X" is the anion portion, where "n" is a positive integer value: {eq}AX (s) \leftrightharpoons A^{n+} + X^{n-} \\ Earn Transferable Credit & Get your Degree, Get access to this video and our entire Q&A library. Example #5: Silver azide has the formula AgN3 and Ksp = 2.0 x 10¯8. Select one: a. Show transcribed image text . Switch to. on the Internet says they are wrong. That allows this equation: Example #3: Calculate the molar solubility of barium sulfate, Ksp = 1.07 x 10¯10. Home. Solution: 1) Here is the dissociation equation: AlPO 4 (s) ⇌ Al 3+ (aq) + PO 4 3 ¯(aq) 2) Here is the K sp expression: K sp = [Al 3+] [PO 4 3 ¯] 3) Keep in mind that the key point is the one-to-one ratio of the ions in solution. The formula for K sp is: K sp = [Ag + ] [I –] K sp = s 2 = 8.5 x 10 -17. where s is the concentration of each ion at equilibrium. This means that the two ions are equal in their concentration. {/eq}. Now, solve for s: s 2 = 8.5 x 10 -17. s = [latex]\sqrt {8.5 \times 10^ {-17} } [/latex] s = 9.0 x 10 -9 mol/L. We can simply consider the following solubility equilibrium of a generic 1:1 salt compound. All rights reserved. Iron (III) hydroxide could be... What is the molar solubility of PbS in water?

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