The molar solubility of AgI is 9.0 x 10 -9 mol/L. This is known as the molar solubility of the compound in water at a given temperature (usually 25 Celsius). Now, I look at the relationship between AgCl and Cl¯. Be prepared! All rights reserved. When you see this, you need to assume that it is a saturated solution. By the way, the sulfate already present in solution came from some other sulfate-containing compound, say sodium sulfate, Na2SO4. 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. Calculating the molar solubility is left to the student. - 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 Calculate the Ksp for Ag2S. Earn Transferable Credit & Get your Degree, Get access to this video and our entire Q&A library. Services, Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations, Working Scholars® Bringing Tuition-Free College to the Community. 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. Calculate the value of Ks under these conditions. Your dashboard and recommendations. 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-} \\ Calculate the K sp for Ba 3 (PO 4) 2. Anything else makes the problem unworkable and that is not the intent of the question writer. The Ksp for MgF2 is 6.4 x 10-9. Solution for The molar solubility of Ag2S is 1.26 x 10-16 mol L-1 in pure water. 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. Therefore we do not have to perform individual calculations for each compound. This … Home. That allows this equation: Example #3: Calculate the molar solubility of barium sulfate, Ksp = 1.07 x 10¯10. 1.12 x 10-8 c. 8.00… 3) Keep in mind that the key point is the one-to-one ratio of the ions in solution. {/eq}, b. This dissociates: Note how I ignored the s in (0.0153 + s). True or false? Show transcribed image text . 4) We have to reason out the values of the two guys on the right. A) PbS, Ksp=9.04 X 10-29 B) PbSO4, Ksp = 1.82 X 10-8 C) MgCO3, Ksp = 6.82 X 10-6 D) FeS, Ksp= 3.72 X 10-19 E) Agi, Ksp = 8.51 X 10-17. All other trademarks and copyrights are the property of their respective owners. An unsaturated solution is a solution in which all solute has dissolved. We can simply consider the following solubility equilibrium of a generic 1:1 salt compound. Study Guides. 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. 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. Select one: a. Calculate its solubility in moles per liter. 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? Example #5: Silver azide has the formula AgN3 and Ksp = 2.0 x 10¯8. 3.78 x 10-12 b. Our experts can answer your tough homework and study questions. What is its molar solubility in pure water? Get the detailed answer: What is the molar solubility of AgI in pure water? Ksp (AgI) = 8.51 × 10-17. Note azide, a fairly uncommon polyatomic ion. {eq}\boxed{PbSO_4; K_{sp} = 1.82 \times 10^{-5}} Which of the following compounds will have the highest molar solubility in pure water? The reasons behind this are complex and beyond the scope of the ChemTeam's goals for this web site. One last thing. Get the detailed answer: What is the molar solubility of AgI in pure water? All of the salt compounds shown dissociate in a 1:1 ratio of ions. Example #6: Calculate the [Ba2+] if the [SO42¯] = 0.0153 M. Ksp = 1.07 x 10¯10. 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. The ammonium phosphate polyatomic ion, NH4PO42¯, is an uncommon one. {eq}PbSO_4; K_{sp} = 1.82 \times 10^{-5} It could show up on the test! So, the molar solubility of AgCl is 1.33 x 10¯5 moles per liter. a. Example #2: Aluminum phosphate has a Ksp of 9.83 x 10¯21. This means that the two ions are equal in their concentration. a. BaCrO4; molar solubility = 1.08 * 10-5 M b. Ag2SO3; molar solubility = 1.55 * 10-5 M c. Pd(SCN)2; molar solubility … Answer to: Which of the following compounds will have the highest molar solubility in pure water? In a saturated aqueous solution of an ionic (salt) compound, there is a certain dissolved molarity of this compound present. That's the value that I want to determine. Thanks. Example #1: Silver chloride, AgCl, has a Ksp = 1.77 x 10¯10. Booster Classes. Homework Help. We will completely ignore the sodium ion, because it plays no role in the Ksp equilibrium. 1) The compound in solution is BaSO4. Sciences, Culinary Arts and Personal I hope I'm not too insulting when I emphasize both sides. {/eq}. Here the choice is lead (II) sulfate: a. Personalized courses, with or without credits. This problem has been solved! 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. That's because s is very small compared to 0.0153. {/eq}. 3.7 million tough questions answered. See the answer. Switch to.