Water. Determine the molar solubility of Fe(OH)2 in pure water. What is the Ksp of iron(II) hydroxide at 298 K? E° = -0. Calculate the molar solubility of iron (II) hydroxide, Fe (OH)2, in a solution buffered at a pH of 13.3 x 10-38: Pb(OH) 2: 2. Study with Quizlet and memorize flashcards containing terms like A solution has [Ag+] of 3. Fe (OH)2 (s) ⇌ Fe2+ (aq) + 2 OH- (aq) b. asked • 04/08/22 Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 8.0. PL. If the solubility of Fe (OH)2 in water is 7. Assume that all reactants and products are in their standard states. For Fe(OH) 3 it is Ksp = [Fe 3+][OH −]3 In your laboratory notebook calculate the Ksp of Fe(OH) 3 given the solubility data above.5 x 10-11: Mn(OH) 2: 4.22? The Ksp of Fe(OH)2 is 4. Chemistry questions and answers. The monohydrate FeO(OH) · H 2 O is often referred to as iron(III) hydroxide Fe(OH) 3, hydrated iron oxide, yellow iron oxide, or Pigment Yellow … Calculate Ksp for CaF2.8 x 10-16: Mg(OH) 2: 1. The Ksp for Fe (OH)2 = 4.23 B. If a solution contained CO2−3, OH−, and F− ions, each at a concentration of 0. X.6x10-13. A certain metal when irradiated by a light of frequency ν = 3.1 ×10-4 g 1 L × 1 mol 89. Ksp = 2. 1x10^-3 M of Mg(OH)2 is added to pure water, with a total volume of 1L.7 × 10 − 11. (c) Determine the molar solubility of Fe (OH)3 if the pH of the solution is 2.5 x 10-11: Mn(OH) 2: 4.07 x 10-5 g/100 mL. (a) Write a balanced equation for the solubility equilibrium.9 x 10-15: Fe(OH) 3: 6.44 ⋅ 10−4M)(1+2) Ksp = 1. Determine what is wrong with the following K Question: Calculate the solubility of iron(II) hydroxide, Fe(OH)2 in units of grams per liter.3 x 10 What is the Ksp for Fe (OH)2 at 25 °C? Select one: a. See Answer.5 x 10-10 mol/L. The solubility product expression for Fe (OH)3 is Ksp = a) [Fe3+] [OH - ]b) [Fe2+] [OH. Will a precipitate of Ag2Cr04 form when 1.8 x 10-16: Mg(OH) 2: 1.5 x 10-17: Iodides … Fe(OH)_2(s) rightleftharpoonsFe^(2+) + 2HO^- And we write the solubility expression, K_(sp)=[Fe^(2+)][HO^(-)]^2.H are equal to 14, we can find it. 1. O. The Ksp of metal hydroxide, Fe (OH)2, is 1. May 26, 2018 The closest value is c.1 × 10 − 4) ( 4. (b) Write the expression for the solubility product constant, Ksp, and calculate its value.6 × 10-5: Phosphates: AlPO 4: 1.800M Fe (NO3)3 at 25 °C. The magnitude of #K_ (sp)# directly indicates the solubility of the salt in water, since #K_ (sp)# is derived from the concentrations of ions in equilibrium reactions. (3 pts) Compare the molar solubility of Fe (OH)2 in pure water and in the buffer solution with Question: Calculate the molar solubility of Fe(OH)2 in a solution with pH = 13. 1. 5.9 x 10-17 d.07 x 10-5 g/100 mL. heart. 6.87×10−17, and the Ksp of FeF2 is 2. Chemistry.87×10−17.1 × 10-7: CaC 2 O 4: 2. 1. Chemistry. Example 17.87 · 10-17. Question: Enter your answer in the provided box. There are 2 steps to solve this one.87 x 10^-17.3 x 10-12 b.3/5. Calculate the molar solubility of Fe (OH)3 in pure water. Write Ksp expressions and look up the Ksp values for the following: a.60 x 10^-14. Consider the general dissolution reaction below (in aqueous solutions): See Answer. Reference: Lange's Handbook, pps.1×10 -10 Barium sulfite BaSO 3 8×10 -7 Barium thiosulfate BaS 2 O 3 You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Expert-verified. 4.0 x 10-9 M 3.4× 10 - 5 = 4 x 3.2. Question: The Ksp of metal hydroxide, Fe (OH)2, is 1. Calcium oxalate monohydrate [Ca (O 2 CCO 2 )·H 2 O, also written as CaC 2 O 4 ·H 2 O] is a sparingly soluble salt that is the other major component of kidney stones [along with Ca 3 (PO 4) 2 ]. 0 • 65 . The equilibrium constant for a dissolution reaction, called the solubility product ( Ksp ), is a measure of the solubility of a compound. 3.3 x 10 Calculate the pH of a saturated solution of Ba (OH) is 1.47 × 10-17 Calculate the molar solubility of Fe (OH)2 in pure water and 0.7 x 10-9: AgI: 1. Solubility Product Constants K. You'll find Ksp data in the ALEKS Data tab.Ksp = [Fe2+][OH-]^2Ksp = 4. Calculate the solubility of Fe (OH)3 in each of the following: Calculate the solubility of Fe (OH)3 in each of the following: k sp = 4 x 10 -38.03 x 10¯ 22 = (3s) 3 (s) 27s 4 = 1.0 x 10-13 M E.01 = Hp ta dereffub nehw 2)HO(eF fo ytilibulos ralom eht etaluclaC . Procedure for measuring [OH] in a saturated Ca(OH) 2 solution. Martell, "Stability Constants of Metal-Ion Complexes," The Chemical Society, London, 1964 (Special Chima M.9 x 10-15: Fe(OH) 3: 6. 1. The balanced equation of this reaction is the following: Fe(OH)2(s)+2e−⇌Fe(s)+2OH−(aq) The Ksp of Fe(OH)2 is 4. sp x ? You'll get a detailed solution from a subject matter expert that helps you learn core concepts. View 3. Now cleary, "S = solubility"=[Fe^(2+)] So … You'll get a detailed solution from a subject matter expert that helps you learn core concepts.30e-06 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 6. Determine the molar solubility. 4. Calculate the value of Ksp for ZnS. Question: Calculate the molar solubility of Fe (OH)2 in a buffer solution where the pH has been fixed at the indicated values. Exercise 18. 8-6 to 8-11; L. Ksp.90M Fe (NO3)2.87 x 10-17: Iron(II) sulfide: FeS: 8 x 10-19: Iron(III) hydroxide: Fe(OH) 3: 2. 5.10 M Ba (NO3)2.To begin, we must first … The dissociation equation for Fe(OH)2 will be as: Fe(OH)2 ---> Fe2+ + 2OH- Given, Ksp for Fe(OH)2= 4. Calculate the solubility in moles per liter of Fe (OH) 3 Ksp=4×10^-38 in each of the following.5 * 10-4 M strontium ions (Sr+2), if enough of the soluble salt Na2SO4is added to make the solution 2. Calculated Using The Solubility Product Ksp• Furthermore data at high pH values are lacking. The solubility of Fe(OH)3 in aqueous solution was determined to be 4. 1. The solubility product constant, Ksp K s p , is the equilibrium constant for a solid substance dissolving in an aqueous solution. Consider a saturated ferrous hydroxide solution. What is the solubility of iron (II) hydroxide in mol/L and g/L at 25°C? Ksp for Fe(OH)2)= 4. Calculate Ksp for Fe (OH)2.0B) pH=10.90×10-17. If the solubility of Fe (OH)2 in water is 7.120 - x. So you must start by writing the equilibrium reaction: Fe(OH)3 (s) ----> Fe(3+) aq + 3 (OH-) aq Fe(OH) 2: 7. Calculate the molar solubility s = 2. Fe(OH) 2: 7.67 from 40 and we get Step 1/8 1.1. (a) Write a balanced equation for the solubility equilibrium. 4) THIS IS WRONG!! Notice that you added a base (Al (OH)) to the solution and you obtained an acidic pH.87 × 10-17 is approximately 1. 2. Comparison Of The Solubility of Fe (OH) 2 • 35.0 L solution containing 2. The solid phases of aqion are listed here in two tables (together with the solubility product in form of pKsp = - log10 Ksp ): Table sorted by formula.47e-05 g of Ag3AsO4 dissolves per 100 mL of aqueous solution at 25 oC.05 M weak monobasic acid solution. Show transcribed image text.7×10-6 mol/Lat a certain temperature, what is its Ksp at that temperature? a. Verified answer.0.3 × 10-20: Ba 3 (PO 4 To determine the molar solubility of Fe(OH) 2 _2 2 in pure water, we need to evaluate the solubility product constant (Ksp) and write the equilibrium constant equation. b.7 ×10‐19 K s p = 3.6 x 10-10.66 10−6 M. 8. Ksp (Fe (OH)2) = 7.2. Calculate the molar solubility of Fe(OH) 2 in a solution buffered at (a) pH 8. Tried to delta G= - (RT) (InK) and then Delta G/-nF = Ecell, but the answers i keep getting are wrong. This means that the Kps of magnesium hydroxide is. Calculate the molar solubility of Fe (OH)2 given that Ksp at 25°C is 4. The monohydrate FeO(OH) · H 2 O is often referred to as iron(III) hydroxide Fe(OH) 3, hydrated iron oxide, yellow iron oxide, or Pigment Yellow 42. 'B S (40) z-s precipitate of Fe(OH)2 form? The Ksp of Fe(OH)2(s) is 8. verified. A solution buffered at pH=11. FeCl3 (s) ⇌ Fe3+ (aq) + 3 Cl- (aq) In this case, don’t look up Ksp.0.3 x 10-20: Ba 3 (P0 4) 2: 1.rewsnA eeS .6x10^-14. In a series of stepwise … This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.45 x 10¯ 27. The Ksp of Fe (OH)2 is 4. We hope they will prove usefull to you.3 x 10-38: Pb(OH) 2: 2. 2.8x#10^-15# at 25°C. Q > Ksp and a precipitate will form. Show all work in handwriting or use the software showing calculations and units properly and clearly.6 x 10-14: Ni(OH) 2: 2. The solubility of CuI is 2 x 10 The initial concentrations of FeOH + and Fe (OH) 2 (aq) at pH 5, 7, 8 and 9 were estimated based on the molar fractions of individual Fe(II) species ( Figure S4A) and by assuming instantaneous Calculate the molar solubility of Fe(OH)2(s) in each of the Ids 3 . See Answer This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.79 × 10-39 for Fe (OH)3. Ionic Compound Formula K sp. Question: 2.87. The Ksp of Fe (OH)2 at 25 ˚C is 7. Fe(OH)2 (s) ⇌ Fe2+ (aq) + 2OH- (aq) Report your answer to three decimal places. The solution is saturated. Calculate the molar solubility of Fe(OH)2 when buffered at pH = 10. 4.44 V E°= -0. K_sp =. Ksp for … Chemistry Chemistry questions and answers Calculate the molar solubility of Fe (OH)2 in pure water. Calculate the molar solubility of Fe (OH)2 in a buffer solution Type in the Ksp expression for this slightly soluble salt.4 x 10-7 M.0.9×10-15. 9.07 C. Chemistry. star. S = Ksp x2. Is iron 3 hydroxide soluble? The molar solubility of iron(II) hydroxide (Fe(OH)2) can be calculated using the value of its solubility product constant (Ksp). Although K sp is not a function of pH in Equations … Science Chemistry Solubility equilibrium Determine the molar solubility of Fe (OH)2 in pure water. 1. Thus: K sp = [ Ca 2 +] [ F −] 2 = ( 2.6 x 10-14 M B. One way we can get the equilibrium constant for a reaction We can now substitute our equilibrium concentrations into our equilibrium expression, Ksp: Ksp = [Mg 2+][OH-] 2 = 1.7 x 10-10 Chemistry 1 Answer Ernest Z. Ksp for Fe (OH)2)= 4. See Answer.3 x10-6 L Incorrect This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. 1.5 × 10 ‐ 9.87 × 10-17. C. 8. THIS CANNOT BE!! Solubility Product Constants near 25 °C.) express the molar solubility in moles per liter to two significant figures. So far, nothing out of the ordinary. Question: Determine what is wrong with the following K_sp expression for Fe (OH)2 and correct it. The Ksp of metal hydroxide, Fe (OH)2, is 1. c.9 × 10 − 16 4 3 = 5.35 ? The 𝐾sp of Fe(OH)2 is 4.6 10-14 2.9 × 10-17 Explanation: Step 1. Pure water. Final answer: The molar solubility of Fe(OH)2 in water can be determined by setting up an equilibrium expression, using given Ksp value and assuming the molar solubility as 'x'. Show transcribed image text. The solubility of iron (II) hydroxide, Fe (OH)2, is 1.4 x 10-7 M. Calculate the molar solubility of Fe(OH)2 in a solution buffered at a pH of 8. Calculate the molar solubility of Fe(OH)_2 when buffered at pH = 12. Fe(OH)2(s) ⇌ Fe2+(aq) + 2OH-(aq) Step 2/8 2. What is the Ksp for Fe (OH)2? Fe(OH) 2: 7.G. Calculated Using The Solubility Product Ksp• Furthermore data at high pH values are lacking.7 × 10 − 11.15. 8.e. 13 . Science.0×10 –6 Barium hydroxide Ba(OH) 2 5×10 –3 Barium sulfate BaSO 4 1.
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0.8 x 10-16: Mg(OH) 2: 1.To determine the Fe2+ concentration above which Fe(OH)2 will precipitate from a buffer solution with a pH of 8. D. Aluminum hydroxide Al(OH) 3 1.23 0 4. Final answer: The molar solubility of Fe(OH)2 in water can be determined by setting up an equilibrium expression, using given Ksp value and assuming the molar solubility as 'x'.0 x 10-16 1. Verified answer. 9.5 × 10-11: Mn(OH) 2: 4.67. a. 6. Your Answer: L7 X10 Answer Calculate the solubility of Fe (OH)2 (Ksp = 1. Explanation: To determine the concentration of Fe2+ above which Fe(OH)2 will precipitate, we first need to consider the formula of the solubility product constant (Ksp), which is [Fe2+][OH-]2.stpecnoc eroc nrael uoy spleh taht trepxe rettam tcejbus a morf noitulos deliated a teg ll'uoY !devlos neeb sah melborp sihT . 1x10^-3 M of Mg(OH)2 is added to pure water, with a total volume of 1L.3 x 10-38: Pb(OH) 2: 2. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Iron in both oxidation states forms many complex ions.1×10 –10 Barium sulfite … This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Chemistry questions and answers.1 pH=12. Calculate the molar solubility of Fe(OH)2 when buffered at pH = 12. b. 1. Calculate the pH of a 0.E. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. ksp value for FeOH2 is 4. Martell, "Stability Constants of Metal-Ion Complexes," The Chemical Society, London, 1964 (Special Chima M. (a) Write a balanced equation for the solubility equilibrium.66 10−6 M. Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 8.87 x 10-17.00.7 × 10 ‐ 19.5 x 10-17: Iodides : PbI 2: 8. Chemistry questions and answers. However, that two in front of the hydroxide is important and will come into play real soon.1, which shows that the magnitude of K sp varies dramatically for different compounds. 2. In other words, you are going to take the solubility product, that is, you are going to multiply two solubilities, to get the equilibrium equation! The equilibrium equation is: Ni(OH)_2 rightleftharpoons Ni^(2+)+ 2OH^- In this case we are going to multiply the solubility of the Ni^(2+) ion Study with Quizlet and memorize flashcards containing terms like The formation constant, Kf, is the equilibrium constant for the formation of a complex ion and values are typically large (10⁵-10²⁰). Consider a solution that is 1.3 x 10-8 c. 5. 6-10 . Ksp(Fe(OH)2)-7. ksp value for FeOH2 is 4.87 x 10-17.00. pOH = −log 2.0 x 10-4 M AgNO3. Question: Find Ecell for the following half-reaction.9 × 10-15: Fe(OH) 3: 6. Q > Ksp and a precipitate will not form. Question: Calculate the solubility (in g/L) of Fe (OH)2 in 0. The Ksp of FeCO3 is 3.
67×10−6 A.0.6 x 10-5 M.8×10-15 c.10 M Ba (NO3)2.6 x 10-5: Phosphates: AlP0 4: 1.36 × 10 −4 g/100 mL. 7.4C)pH=13.89 V Fe(OH)2(S) + 2e → Fe(s) + 2OH(aq) Fe2+ (aq) + 2e → Fe(s) 2.22 times 10^{-8} M in pure water to calculate K_{sp} for Pd(SCN)_2. Ksp (Fe (OH)2) = 7.0 mL of solution. Question: What is the pH of a saturated solution of Fe (OH)2? For Fe (OH)2, Ksp = 8. prevent the spontaneous crystalization of dissolved chemicals. m. (The value of Ksp for Fe (OH)2 is 4. Calcium oxalate monohydrate [Ca (O 2 CCO 2 )·H 2 O, also written as CaC 2 O 4 ·H 2 O] is a sparingly soluble salt that is the other major component of kidney stones [along with Ca 3 (PO 4) 2 ]. (the value of ksp for fe(oh)2 is 4.77 D. Question: Enter your answer in the provided box. AgCN A g C N with Ksp = 2. See Answer. Â . Fe(OH) 2: 4.A) pH=8. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Calculate the solubility (in g/L) of Fe (OH)2 in 0.87 x 10-17.0 OA. (a) If the molar solubility of Fe (OH)2 at 25 oC is 2. 4. (the value of ksp for fe(oh)2 is 4.87 × 10-17.0 x 10-4 M AgNO3.40 x 10¯ 6 M Comment: at the high school level, arsenate may be one of those unusual polyatomic ions, one that you didn't learn in the nomenclature section. Final answer: The concentration of Fe2+ above which Fe(OH)2 will precipitate from a buffer solution of pH 8.0 ×10‐12 K s p = 2.3/5. The solubility (by which we usually mean the molar solubility) of a solid is expressed as the concentration of the "dissolved solid" in a saturated solution. 2.2×10 -10 Barium fluoride BaF 2 1. Your Answer: L7 X10 Answer Calculate the solubility of Fe (OH)2 (Ksp = 1. 3rd: Use reaction stoichiometry to determine mol Ca+2 and mol F-: Because there is exactly 1 L of solution, these values are also the molarities of each ion. Fe (OH)2 (s) ⇌ Fe2+ (aq) + 2 OH- (aq) b. But for a more complicated stoichiometry such as as silver First, write out the Ksp expression, then substitute in concentrations and solve for Ksp: CaF 2 ( s) ↽ − − ⇀ Ca 2 + ( aq) + 2 F − ( aq) A saturated solution is a solution at equilibrium with the solid. What is the Ksp for Fe (OH)2? The pH of a saturated solution of Fe (OH)2 is 8.0 x 10-7M.0 x 10-16. See Answer See Answer See Answer done loading. Question: The Ksp of iron (II) hydroxide, Fe (OH)2, is 4.1. Who are the experts? Experts are tested by Chegg as specialists in their subject area.6 x 10-8 mol/L O D. Q < Ksp and a precipitate will form.87×10−17.0.5 x 10-17: Iodides : PbI 2: 8. Related materials Green rust is a recently discovered mineralogical form. Supersaturated solutions: have more dissolved substances than predicted by solubility alone.9×10-11.8 x 10-15 ) in 0.77 e.0. If there are any other salts for which you know the value of the constant, please let us know and we will update the table.4× 10 - 5 = ( 2 x) 2 ( x) 1. star.0 x 10-13 M is the answer. Q > Ksp and a precipitate will not form.5 x 10-10 M (I thought that was the solubility for Fe(OH)2)? I checked out the other thread that specifically asks this question but still don't get it. 1. Use the Ksp value from the Table to calculate the solubility of iron (II) hydroxide in pure water in grams per 100. There is a big hint in the name: Ksp is the equilibrium solubility product constant. The solubility of iron (II) hydroxide, Fe (OH)2, is 1. In contrast, the ion product ( Q) describes Example #3: Silver arsenate, K sp = 1. 1. Question: Calculate the solubility of iron (II) hydroxide, Fe (OH)2 in units of grams per liter. C. When trying to write the equation for #K_ (sp)#, you need to know how to break the compound into ions This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.0 mL of solution. Who are the experts? Experts have been vetted by Chegg as specialists in this subject. Your Answer: Answer C2H4 (g) + 302 (g) --> 2CO2 (g) + 2H20 (g) The reaction above is spontaneous at 25°C.00. The Ksp of Zn(OH)2 is 3 x 10-15 and the Kf of Zn(OH)2 is 2 x 1015. By solving Ksp = [Fe2+][OH-]², we can find 'x' and thus determine the molar solubility. A. Calculate its Ksp. B. Calculate the solubility-product constant for Ag3AsO4.03 x 10¯ 22.30 x 10-6 M This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.1×10 –9 Barium chromate BaCrO 4 1. (b) Write the expression for the solubility product constant, Ksp, and calculate its value. The ph is 8. (molar mass of Fe (OH)2 = 89. You'll find Ksp data in the ALEKS Data tab.015 M NaOH. The balanced chemical equation for the dissolution of solid Fe (OH)3 in water Ksp of Fe(OH)3 is 2. The Ksp of metal hydroxide, Fe (OH)2, is 1. Thank you so much. 2.3 x 10-20: Ba 3 (P0 4) 2: 1. (Ksp Fe(OH)2 = 1. b. The solubility of Fe (OH)2 (s) in an aqueous solution at 25°C that is buffered at pH 11. Q > Ksp and a precipitate will form.8 x 10-15 ) in 0.43 x10-3 gram per litre at 25 0C.Fe(OH) 2: 7. The rate constant is dependent on the reactant concentrations.87×10−17. ksp value for FeOH2 Comparison Of The Solubility of Fe (OH) 2 • 35. Chemistry. Calculate the K_sp.G.9 ×10−17 ) There are 2 steps to solve this one.87×10−17. Calculate the molar solubility of fe(oh)2 in pure water.1. The Ksp of Fe(OH)2 is 4.87 x 10-17. The rates of most chemical reactions change with time. X.3 x10-6 L Incorrect. But for a more complicated … Solubility Product Constants near 25 °C.0 x 10-13 M E. Whereas solubility is usually expressed in terms of mass of solute per 100 mL of solvent, Ksp is defined in terms of the molar concentrations of the component ions. heart. Was Fe(OH)2 more or less soluble with increasing pH? I got the answer, please don't answer my question.87×10−17. Use the Ksp values in the table to calculate the molar solubility of AgBr in pure water. Calculate the molar solubility, s, of this compound. Find an answer to your question Calculate the molar solubility of fe(oh)2 in pure water. 1. Calculate the pH of a 0.34 × 10-6lmol/L Step 2.6. Whereas solubility is usually expressed in terms of mass of solute per 100 mL of solvent, Ksp is defined in terms of the molar concentrations of the component ions.. Calculate the solubility in moles/L of each of three salts and the concentration of the cations in mg/mL in each of the saturated solutions. PL. Calculate the molar solubility of barium fluoride in each liquid or solution.1. The solution is saturated. Calculate the work function of the metal. Here’s the best way to solve it. a) Determine the molar solubility of Fe (OH)3 in pure water. QUESTION 6.3 x 10-9: MgC 2 O 4: 8.9x1015 solubility = g/L .10/ 7. Q < Ksp and a precipitate will not form. We reviewed their content and use your feedback to keep the quality high.5 × 10-17: Iodides : PbI 2: 8..3 × 10-38: Pb(OH) 2: 2.015 M NaOH.35 ? The 𝐾sp of Fe(OH)2 is 4. Calculate the molar solubility at a pH of 10. 3. The concentration of Fe2+ in a solution saturated with Fe (OH)2 (s) is 7. Chemistry Chemistry questions and answers The Ksp of iron (II) hydroxide, Fe (OH)2, is 4.87×10−17 Lead (II) bromide PbBr2 4.6 x 103 mol/L Appl Of Ms Excel In Analytical Chemistry 2nd Edition ISBN: 9781285686691 Author: Crouch Publisher: Cengage VIDEO ANSWER: The pitch of the saturated solution of Iran to hydroxide is 8. There are 2 steps to solve this one. You'll find Ksp data in the ALEKS Data tab. 4. Question: 31. (b) Determine the molar solubility of Fe (OH)3 if the pH of the solution is 8. {n = 1 m = 2.0 × 10 -16 anld K v = 1. When the [Math Processing Error] K s p expression is written in terms of [Math Processing Error] s, we get the following result for the molar solubility.87×10−17. In the pH . B. Complete the following solubility constant expression for Fe (OH)2.) express the molar solubility in moles per liter to two significant figures.90×10-17.6 x 10-14) 8. A. Please give detailed steps, as much detail as possible The Ksp for Fe(OH)2 is 4. Q < Ksp and a precipitate will not form.0Answer in M. Who are the experts? Experts have been vetted by Chegg as specialists in this subject.2×10 –10 Barium fluoride BaF 2 1.5 × 10-16: Oxalates : BaC 2 O 4: 1. A drink that contains 4 1/2 ounces of a proof liquor… approximately how many drinks does this beverage 1 attachment. Calculate the solubility of Fe (OH)2.6×10-16 d.2 x 10-8 M 2.6 x 10-5: Phosphates: AlP0 4: 1. Ksp = [Fe2+][OH-]2 Step 3/8 3. Fe (OH)2: 4.8 × 10 − 6 M. at 25°C. A. Fe (OH)3 (s) ⇌ Fe3+ (aq) + 3 OH- (aq) c. a. Write the Ksp expression for the sparingly soluble compound lead chromate, PbCr04: If This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. E. Since ph and P. Show transcribed image text.6 x 1011 mol/L OC.2 × 10 − 4) 2 = 3. 6.87.M5-01 x 31.6x10-13 => s << 0. It represents the level at which a solute dissolves in solution. Fe (OH)2 (s)+2e- --> Fe (s) + 2OH- (aq). Aluminum hydroxide Al(OH) 3 1. heart. #K_(sp)# for iron (II) hydroxide, #Fe(OH)_2# has a value 1. Water. Ksp = 7. Question: 31.2 × 10-3 M and 0. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. 7.87×10 Here's an example: The K s p value of A g 2 S O 4 ,silver sulfate, is 1. Calculate the work function of the metal.125 M NH3.8 x 10-16: Zn(OH) 2: 4. FeCl3 (s) ⇌ Fe3+ (aq) + 3 Cl- (aq) In this case, don't look up Ksp. d. [Fe2+] = x Step 4/8 4. Solution: 1) Here is the equation for dissociation: Sn(OH) 2 (s) ⇌ Sn 2+ (aq) + 2OH¯(aq) 2) Here is the K sp expression: K sp = [Sn 2+] [OH¯] 2. The more soluble a substance is, the higher the Ksp K s p value it has. Calculate the molar solubility of this Question: The K s p of iron (II) hydroxide, F e ( O The equilibrium constant for a dissolution reaction, called the solubility product ( Ksp ), is a measure of the solubility of a compound. By solving Ksp = [Fe2+][OH-]², we can find 'x' and thus determine the molar solubility.