A solution contains 0.100 M each of Ni2+ and Sn2+ ions. To separate them, the sulfide salt of...
Question:
A solution contains 0.100 M each of {eq}Ni^{2+} {/eq} and {eq}Sn^{2+} {/eq} ions. To separate them, the sulfide salt of each of the ions must be formed. What concentration of {eq}S^{2-} {/eq} must be added to accomplish this separation if the {eq}K_{sp} {/eq} of {eq}NiS = 6.3 \times 10^{-27} {/eq} and {eq}SnS = 1.1 \times 10^{-29} {/eq}?
Ksp:
When a solution is saturated, undissolved solutes are in equilibrium with their dissolved ions. This equilibrium state is governed by the constant known as Ksp. Like other equilibrium constants, Ksp is influenced by temperature such that the higher the temperature, the higher the Ksp. It can also be used to approximate the solubilities of sparingly soluble salts relative to each other where lower Ksp means lower solubility.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answer{eq}\rm{NiS }{/eq} and {eq}\rm{SnS }{/eq} are both 1:1 binary salts. Moreover, the concentration of their cations is the same. This means, we only...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations
from
Chapter 11 / Lesson 5
17K
Learn about solubility product constant. Understand the definition of Ksp, the Ksp formula, how to calculate Ksp, and how to find molar solubility from Ksp.
Related to this Question
- A solution contains .036 M Cu^2+ and .044 M Fe^2+. A solution containing sulfide ions is added to selectively precipitate one of the metal ions from solution. at what concentration of sulfide ion with
- What is the concentration of lead ions and sulfide ions in a saturated solution of lead sulfide (PbS) solution at 25^oC?
- If sodium sulfide is dissolved in water, what can be said about the concentration of the sodium ion? (a) It has the same concentration as the sulfide ion. (b) Its concentration is half that of the sulfide ion. (c) Its concentration is twice that of the s
- You decide to use sulfide precipitates to separate the copper(II) ions from the manganese(II) ions in a solution that is 0.20 M Cu^{2+} and 0.20 M Mn^{2+}. Determine the minimum sulfide ion concentration that will result in the precipitation of one cati
- In the process of separating Pb2+ ions from Cu2+ ions as sparingly soluble iodates, what is the Pb2+ concentration when Cu2+ begins to precipitate as sodium iodate is added to a solution that is initi
- A solution contains Mg^2+ and Cu^2+ ions. How could you separate them?
- Identify the ions that are present in each solution, and calculate their concentrations. If 1 L of each solution are mixed, will a precipitate be formed? Why? a. 2 x 10-3 M Pb(NO3)2(aq) b. 2 x 10-3 M Na2SO4(aq)
- The equilibrium concentration of sulfide ion in a saturated iron(III) sulfide solution is ____?
- The equilibrium concentration of sulfide ion in a saturated lead sulfide solution is
- Determine the concentration of Mn2+ in a 0.2 M solution of Na2S, a soluble salt. (Ksp of MnS = 2.5 x 10-10)
- A solution contains 7.00 x10-3 M potassium hydroxide and 1.05 x10-2 M ammonium sulfide. Solid iron(II) acetate is added slowly to this mixture. What is the concentration of sulfide ion when hydroxide ion begins to precipitate?
- A solution containing 0.1 M Pb(NO3)2 and 0.1 M AgNO3 has solid NaI added to it until one of the compounds is about to precipitate. Which compound will precipitate first, and what is the concentration of I^- ions when this occurs?
- Iron (II) sulfide is dissolved in water. Calculate the molar solubility if the solution also has potassium sulfide mixed into it to a concentration of 0.302 M.
- what is the concentration of silver ions and chloride ions in a saturated silver chloride solution at 25 C (Ksp= 1.8 � 10^-10)
- When 20 ml of a 0.10 M silver nitrate solution is mixed with 25 ml of a 0.080 M solution of sodium sulfide, producing a precipitate of silver sulfide, what is the final concentration of sulfide ion?
- A solution contains 8.10 10 3 M potassium sulfide and 9.92 10 3 M sodium hydroxide. Solid iron (III) nitrate is added slowly to this mixture A. What is the formula of the substance that precipitates first? B. What is the concentration of iro
- What is the concentration of K^+ ions in a 0.025 M K_2CO_3 solution assuming complete dissociation?
- A solution contains the metal ions listed below, all at the same concentration. The addition of thioacetamide, CH3CSNH2, produces sulfide ion, S2-, causing the ions to precipitate as the sulfides. Each sulfide begins to precipitate at a different concentr
- What concentration of chloride ion is required to precipitate 99.9% of the lead ion from a solution with Pb^{2+} = 0.045 mol/L?
- A 1.00 L solution contains 5.00 x 10^{-5} M Cu(NO_3)_2 and 1.00 x 10^{-3} M ethylenediamine. What is the concentration of Cu(H2O)_6^{2+} ions in the solution at equilibrium?
- What is the Pb^{2+} concentration in a saturated solution of PbCl_2, if the concentration of chloride ion is 0.023 M? Units: K_{SP} = 1.72 times 10^{-5} M.
- An aqueous solution containing both Sr^{2+} and CO_3^{2-} ions is mixed in order to precipitate SrCO_3(s). Given there are 0.800 mL of 2.49 M Sr^{2+} ions, calculate the mass of SrCO_3 that is formed. Assume that all of the Sr^{2+} ions are consumed. The
- A 3.60-L solution of 1.60 x 10^-3 M Pb(NO3)2 is mixed with a 0.60-L solution of 0.53 M NaCl. Calculate Qc for the dissolution of PbCl2 (Ksp = 1.6 x 10^-5). No precipitate has formed.
- What volume of a 0.176 M Na_2S solution contains 1.01 g of Na^+ ions?
- What volume of a 0.158 M Na_2S solution contains 1.01 g of Na^+ ions?
- What is the concentration of a potassium ion in 2.0 M of potassium sulfide?
- How should the ions Hg22+ and Ni2+ be separated in aqueous solution by selective precipitation?
- How should the ions Ag+, Ba2+, and Cr3+ be separated in aqueous solution by selective precipitation?
- How should the ions Ag+, Pb2+, and Cu2+ be separated in aqueous solution by selective precipitation?
- PLEASE HELP! Consider a solution that is 2.3* 10-2 M in Fe2+ and 1.1* 10-2 M in Mg2+. What is the remaining concentration of the cation that precipitates first, when the other cation just begins to pr
- A solution contains 0.50 M lead ions, P b 2 + , and 0.00010 M zinc ions, Z n 2 + . If solid N a 2 S is slowly added to the solution, which salt precipitates first, P b S or Z n S ? What is the concentration of the first ion that precipitates when t
- A solution contains .10 M Cl- and .10 M Br-. If Ag+ is added until AgCl just begins to precipitate, what are the concentrations of Ag+ and Br-? ( Ksp for AgCl=1.8x10^-10, Ksp for AgBr= 3.3x10^-13)
- A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation, 99% of metal ion must be precipitated before the other metal ion begins to precipitate, and assume no
- Assume you are given the task of separating Ag^(+) and Fe^(2+) ions in aqueous solution. Determine if each reagent listed below can be used to separate the ions. If the reagent can be used to separate
- What is the concentration of the cation that precipitates first, when the other cation just begins to precipitate? Consider a solution that is 2.2 times 10^{-2} M in Fe^{2+} and 1.6 times 10^{-2} M in Mg^{2+}.
- How to seperate and precipitate cu^2+ ions from Ni^2+ ions in solution
- What is the equilibrium concentration of Pb^2+ in a solution of PbCl_2 that is 0.46 M in chloride ion? PbCl2(s) <=>Pb2+(aq) + 2 Cl^- (aq) Kc = 1.7 * 10^-5
- A solution contains 0.55 g of dissolved Sn4+ ions. How many grams of Na2CO3 must be added to the solution to completely precipitate all of the dissolved Sn4+?
- Suppose 0.250 L of 0.294 M AgNO3 solution is mixed with 0.350 L of 0.300 M Na2CO3 solution. (Ksp for Ag2CO3 is 8.46 x 10-12) a. What mass of the precipitate forms? b. What is the concentration of Ag+ remaining in solution?
- The molar solubility of iron(III) sulfide, Fe2S3, is 1.05 x 10^{-18} mol/L. (1) Express the solubility in units of grams per liter. [{Blank}] g/L (2) Calculate the concentration of sulfide ion in a saturated solution of iron(III) sulfide. [{Blank}] mol
- What is the total concentration of all ions (the sum of their individual concentrations) in aqueous solutions of the following? Hint: Each substance is an electrolyte that dissociates in water to produce ions. Use a table of polyatomic ions if you do not
- what is the concentration of lead ion in a saturated solution of PbCl_2 if the Ksp is 1.6 x10^-5?
- A solution contains 0.25 M Ni(NO_3) and 0.25 M Cu(NO_3)_2. Can metal ions be separated by slowly adding Na_2CO_3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begin to precipitate, and assume t
- Determine the concentration of the cation and anion in each aqueous solution. (Assume complete dissociation of each compound.) 1.) 0.30 M Na_2SO__4 2.) 0.45 M K_2CO 3.) 30.23 M RbBr
- What is the solubility of AgCl, when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write down the equation for the
- What precipitate is most likely formed from a solution containing Ca2+, Na+, OH-, and CO2?
- What concentration of the lead ion, Pb^{2+} , must be exceeded to precipitate PbCl_2 from a solution that is 1.00 \times 10^{-2} M in the chloride ion, Cl^-? (K_{sp} for lead chloride is 1.17 \times
- Calculate the solubility (a) in mol/L and (b) in g/L of AgCl in 2.0 M NH3(aq). What is the concentration of Ag+ in this solution? (Ksp = 1.6 x 10-10; Kf = 1.7 x 107 for Ag(NH3)2+
- What is the concentration of CO32- ion in saturated CaCO3 aqueous solution? The Ksp for CaCO3 is 5.0 x 10-9.
- The concentration of P b 2 + ions and of C O 2 3 ions in a saturated aqueous solution of P b C O 3 is 1.8 10 7 M . (a) Determine K e q for P b C O 3 . (b) Calculate its solubility in g/L and in g/100 mL
- A solution contains 5.72 * 10^{-3} M manganese(II) nitrate and 6.51 * 10^{-3} M lead acetate. Solid ammonium carbonate is added slowly to this mixture. What is the concentration of lead ion when manganese(II) ion begins to precipitate?
- 3. What is the concentration of silver (I) ion in a saturated solution of silver (I) carbonate containing 0.0024 M Na_2CO_3
- Which solution has the largest concentration of chloride ions (Cl-) present in the solution? a. 2.5 M NH4Cl b. 1.5 M FeCl3 c. 2 M MgCl2 d. 3.0 M LiCl
- For the solubility equilibrium Ag_2SO_4 (s) rightleftharpoons 2Ag^+(aq) + SO_4^{-2} (aq), if the concentration of sulfate ion in a saturated solution of Ag_2SO_4 is found to be 0.0155 M, what is the value of K_{sp} for this salt?
- Equal volumes of 0.0150 M barium chloride and 0.0100 M sodium sulfate are mixed. What are the concentrations of the ions present in the final solution? K_sp (BaSO_4) = 1.1 times 10^-10.
- A solution is made by equilibrating the two solids lead carbonate (Ksp = 1.5 \times 10^{-13}) and lead sulfate (Ksp = 1.8 \times 10^{-8}) with water. What are the concentrations of the three ions at equilibrium, if some of each of the solids remain? [Pb^{
- The K_{sp} of nickel sulfide is 4.0 times 10^{-20}. What is the concentration of sulfide ion in a saturated solution of nickel sulfide to which 0.040 mol of nickel nitrate is added?
- Calculate the following when 0.250 L of 0.249 M AgNO_3 solution is mixed with 0.350 L of 0.300 M Na_2CO_3 solution. K_{SP} for Ag_2CO_3 is 8.46 times 10^{-12}. A) What mass of the precipitate forms? B) What is the concentration of Ag^+ remaining in solut
- What is the molar solubility of iron(II) sulfide in a 0.280 M ammonium sulfide solution?
- Specify what ions are present in solution upon dissolving each of the following substances in water:
- What must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO_4, from a solution that is 0.0034 M Sr^2+?
- The concentration of ammonium ion in the solution of the salt called ferrous ammonium sulfate, formula (Fe(NH_4))_2(SO_4)_3, is 0.360 M. What is the concentration of sulfate ions in this solution?
- What is the total concentration of ions in a 0.10 M solution of barium chloride? \\ A. 0.20 M B. 0.30 M C. 0.40 M D. 0.10 M
- What is the silver ion concentration for a saturated solution of Ag2CO3 if the Ksp for Ag2CO3 is 8.4 x 10^-12
- A solution contains 1.04 \times 10^{-2} M sodium chromate and 1.11 \times 10^{-2} M ammonium phosphate. Solid lead nitrate is added slowly to this mixture. What is the concentration of phosphate ion when chromate ion begins to precipitate?
- What precipitate is most likely formed from a solution containing Ca2+, Na+, OH-, and CO32-?
- What is the solubility of AgCl when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) a. Make a reaction table. Include rows for initial concentration, change in concentration, and equ
- How would hydroxide ions influence the concentration of sulfide ions?
- What is the I^- concentration just as AgCl begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl^- and 0.015 M I^-?
- What is the molar solubility of manganese sulfide? M What is the concentration of manganese ions in a saturated solution of manganese sulfide? M Manganese Mn(OH) = 21.9 x 10^-13 MnCO_3 =
- what is the molar solubility of MgF_2 (s) in a solution that has (F^-) ion concentration of 0.40M?
- 1.) Calculate the concentration of the silver ion in a saturated solution of silver chloride, AgCl (Ksp = 1.61 x 10^-10). A. none of these B. 1.61 x 10^-10 C. 1.27 x 10^-5 D. 2.59 x 10^-20 E. 3.2
- Assuming the final concentration of chloride anion after the addition of HCl (precipitation step) was 0.1 M, what is the remaining concentration of Ag+ in the solution? (Ksp for AgCl = 1.7x10-7)
- Suppose you have a water solution that is 0.0010 M Ca2+ and 0.0010 M Mg2+. Describe the precipitation reactions as you slowly add a concentrated solution of sodium carbonate (Na2CO3) to this solution. What would be the concentration of carbonate ions when
- Which of the following solutions contains the largest total concentration of ions, assuming complete dissociation? a. 0.010 M aluminum chloride b. 0.010 M aluminum sulfate c. 0.010 M sodium chloride d. 0.010 M calcium chloride
- If the concentration of AgNO3 is (1.550x10^-4) M and the concentration of NaCl is (4.52x10^-4) M, what is the ion product?
- You have separate 0.10 M aqueous solutions of the following salts: LiNO3, Ca(NO3)2, and Al(NO3)3. In which one would you expect to find the highest particle concentration? Which solution would you expect to conduct electricity most strongly? Explain your
- Calculate the resulting aqueous silver ion concentration in the solution formed by combining 15.0 mL of 0.250 M CaCl_2 (aq), and 30.0mL of 0.400 M AgNO_3 (aq).
- A solution contains 23.1 ppm of dissolved Fe(NO3)3 (241.860 g/mol), which dissociates completely into Fe3+ and NO3- (62.005 g/mol) ions. Find the concentration of NO3- in parts per million.
- A solution contains 1.24 * 10^{-2} M sodium phosphate and 6.69 * 10^{-3} M sodium chromate. Solid barium acetate is added slowly to this mixture. What is the concentration of phosphate ion when chromate ion begins to precipitate?
- A solution contains Ag+ and Hg2+ ions. The addition of 0.100 L of 1.44 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 33.3 g. Find the
- Calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. (a) TlCl(s) in 1.250 M HCl K_{sp} = 1.7 \times 10^{-4} (b) PbI_2(s) in 0.0355 M CaI_2 K_{sp} = 1.4 \times 10^
- A solution contains I^-, \space Br^- \space and \space OH^- ions. If Ag^+ is added, what will the precipitate (s) be?
- A solution contains 1.23 x 10-2 M silver nitrate and 1.07 x 10-2 M lead acetate. Solid ammonium chloride is added slowly to this mixture. What is the concentration of silver ion when lead ion begins to precipitate?
- An aqueous solution is analyzed and found to contain potassium ions and sulfate ions. Write the equation for the dissolution of the salt that produced this solution. If the solution contains 0.600 mol
- Determine the molar solubility of MnS in a solution containing 0.0350 M Na2S. (Ksp of MnS = 2.50 x 10^-10)
- You are given a solution that contains Ca^{2+}\ Al^{3+} and Ag^+ ions. Your goal is to separate these ions by precipitating them from solution one at a time. You have the following solutions at your disposal: Na_2CO_3, NaCl, and Na_2SO_4. Use your textboo
- An ion can be removed from an aqueous solution by 1. formation of a precipitate. 2. the formation of a gas that escapes. 3. All of these 4. the formation of what is essentially a nonelectrolyte.
- A solution contains 0.20 M potassium sulfide and 0.20 M potassium carbonate. Solid nickel(II) nitrate is added slowly to this mixture. What ionic compound precipitates first from the solution? (Hint: It is not necessary to do a calculation, a general ex
- What is the concentration of lead in a saturated solution of PbSO4, given the Ksp of PbSO4 is 6.3 x 10-7?
- What is the equation for the dissociation of Na2S in aqueous solution?
- Which of the following aqueous solutions will contain the highest concentration of hydrated ions (assuming 100% ionization and dissolution)? a. 1.5 M magnesium nitrate b. 0.5 M aluminum chloride c. 0.5 M sodium sulfide d. 2.0 M sodium chloride e. 1.0 M po
- What is the concentration of barium ions in a 0.750 M BaCl2 solution?
- What is the I- concentration just as AgCl begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.0500 M Cl- and 0.0500 M I-? (Ksp values: AgCl = 1.8 times 10-10; AgI = 1 tim
- How can precipitates be dissolved? a. never b. by adding constituent ions to the solution c. by complexing one of the constituent ions in a soluble form
- A solution contains 0.0130 M Pb^{2+} (aq) and 0.0130 M Sr^{2+} (aq). If we add SO_4^{2+} (aq), what will be the concentration of Pb^{2+} (aq) when SrSO_4 (s) begins to precipitate?
- Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2 (aq) and 0.0370 M Ag (aq). What will be the concentration of Ca2 (aq) when Ag2SO4 (s) begins to precipitate?
- Specify what ions are present in solution upon dissolving each of the following substances in water. Express your answers separated by a comma. (NH_4)_2SO_4 Ca(OH)_2 MgI_2 K_2CO_3 HClO_4 NaCH_3COO
- At what molar ~[H_3O^+~] will PbS just start to precipitate from a solution consisting of 1.592 \times 10^{-6} M Pb(NO_3)_2 in 0.100 M H_2S (satd)? H_2S is bubbled through the solution to keep its concentration constant. PbS(s) \to Pb_2^+ (aq) + S_2^- (
- An ion can be removed from an aqueous solution by 1. the formation of a gas that escapes. 2. formation of a precipitate. 3. the formation of what is essentially a nonelectrolyte. 4. All of these.
Explore our homework questions and answers library
Browse
by subject