All rights reserved. Ksp of PbF2 is 3.3x10^-8 8 years ago. I know that the answer is Ksp = 3.98x10^-8, I just want to how to get this. Please answer in details with all steps. (A) PbF2 Ksp = 4.0 × 10^-8 ___ × 10^(___) M, ___ g/L (B) Ag2CO3 Ksp = 8.1 × 10^-12 ___ × 10^(___) M, ___ × 10^(___) g/L (C) Bi2S3 Ksp = 1.6 × 10^-72 Relevance. Should I call the police on then? When 2.15 x 10^-3 moles of PbF2 dissolves you get 2.15 x 10^-3 moles of Pb2+ and 4.30 x 10^-3 moles of F-. Answer to: Calculate the solubility of PbF2 in water at 25 C . By: J.R. S. answered • 04/20/18. Tutor. 1.2 × 10−4 . Ksp = 3.6 x 10 {/eq}. The 2 in Xy2 is a subscript. Question: Calculate The Solubility At 25 °C Of PbCro, In Pure Water And In A 0.0010 M Na CrO Solution. 5.0 (104) Ph.D. University Professor with 10+ years Tutoring Experience. One litre of water is able to dissolve 2.08x10^-3 mol of PbF2 at 25°C. Calculate the solubility of PbF2 in water at 25C . You'll find data in the ALEKS Data tab. 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 . You'll Find K,, Data In The ALEKS Data Tab. Hang. The solubility of PbF2 in water is 0.680 g/L. Round your answer to 2 significant digits. Click hereto get an answer to your question ️ a) Calculate the solubility of PbF2 in pure water. what type of reaction is Na2B4O7.10H2O + 2HCl -> 2NaCl(aq) + 5H2O + 4B(OH)3. Your . If it... Rank the following in order of increasing... Answer the following questions about the... Silver hydroxide has a solubility of 1.23 \times... A solution of PbI_2 has Pb^{2+} = 4.5 x 10^{-5}... 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? Select one: a. I got 4.3x10^-6 but the back of the book is the answer is 3.5x10^-8 can someone show me how to do this, cause i don't know what i did wrong in my calculations X=2.1 e-3 M. 0 0. 1.5 × 10−8 5. Ksp of PbF2 is {eq}3.3x10^-8 Join Yahoo Answers and get 100 points today. Please explain the steps to do it, thanks. PbF2 = > Pb2+ + 2 F-at equilibrium the solubility of PbF2 = [Pb2-] = x . Hi I'm pretty sure this is an easy question, but when I tried it a got 6.75x10^-16 which i know is not right. Services, Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations, Working Scholars® Bringing Tuition-Free College to the Community. One litre of water is able to dissolve 2.08x10^-3 mol of PbF2 at 25°C. The molar solubility of lead(II) fluoride (PbF2) is2.1 x 10-3 mol/L in pure water at 25ºC. Calculate the solubility product of lead chloride in pure water. Calculate the solubility of PbF2 in water at . I went to a Thanksgiving dinner with over 100 guests. Get your answers by asking now. 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 . Relevance. The value of the constant identifies the degree of which the compound can dissociate in water. For example the higher the Ksp the more soluble the compound is. Calculate the Ksp for PbF2. Favorite Answer. Any help will be much appreciated :). double displasment, single displacement, neutralize)? Follow • 2. Still have questions? L^-1 . Create your account. 1 Answer. You have been told that the solubility of PbF2 is 2.15 x 10^-3 moles/liter. You'll find Ksp data in the ALEKS Data tab. Please answer in details with all steps. Favorite Answer. Determine the molar solubility of Y for XY2 if Ksp is 2.2x10^-4. So...... Ksp = (2.15 x 10^-3)(4.30 x 10^-3)^2 = 3.98 x 10^-8, interior the salt answer of barium phosphate the, undissociated salts and dissociated salts are in equlibrium as Ba3(PO4)2 <--> 3Ba3+ + 2(PO4)2- then, Ksp = [Ba3+]^3 x [(PO4)2-]^2 if S is the solubility of the salt, then Ksp = (3S)^3 x (2S)^2 = (3x a million.4 x 10^-8)^3 x (2 x a million.4 x 10^-8)^2 = 5.8085 x 10^-38. - 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