8-1.    place into 7 separate test tubes 3 drops each of the test solutions for the following anions : Cl-, Br-,                     I-, CN-, Fe(CN)64-,Fe(CN)63-,  and SCN-.            Add 3 drops of AgNO3. Note the color of the precipitate from each test tube. Write the color in row 8-1 in table 6.            Test the solubility of the precipitate with 6N HNO3. Write your observations in row 8-1a in table 6. IONS Chloride Bromide Iodide Cyanide Ferrocyanide ferricyanide thiocyanate         8-1 Color, name and formula of the precipitate.                   8-1a Solubility in HNO3

Q: 44. In which solution will 0.0010 M AgNO3 form a precipitate? a. 2.0x10-7M NaCl (Ksp of…

A: For the precipitation to occur: [Ag+][X-] > Ksp

Q: What mass of AgBr will dissolve in 500.0 mL of 2.55 M NH3? Ksp for AgBr is 5.0 x 10¯13. For the…

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Q: In the presence of I-, Hg2+ forms the complex ion Hgl4²-. The equilibrium concentrations of Hg2+ and…

A:

Q: What mass of AgBr will dissolve in 500.0 mL of 5.10 M NH₃? Ksp for AgBr is 5.0 × 10⁻¹³. For the…

A: The given formation reaction is, AgBr ionizes to give Ag+ and Br- Overall reaction is,

Q: The weak base Mg(OH)2 is weak because it is only partially soluble in water at 25 °C (Ksp =…

A:

Q: Lead (II) Bromide is a slightly soluble solute in water. The following equation represents the…

A: The solubility reaction of PbBr2 is given as, => PbBr2 (s) ----------> Pb2+ (aq) + 2 Br- (aq)…

Q: Should Mg(OH)2(s) precipitate from a solution that is 0.010 M MgCl2 and also 0.10 M NH3?   NH3(aq)…

A: MgCl2 dissociates completely in the solution giving 0.010 M Mg2+ and 0.020 M Cl-1 ions. MgCl2…

Q: 16. 0.20-M Mn2* and 0.010-M Cd? are mixed in a test tube. If NaOH is gradually added into the test…

A: Ksp is the multiplication of solubility of corresponding ions with their appropriate powers. Here…

Q: Calculate the solubility of barium oxalate in pure water and in 0.1M HCI solution, KSP BaC2O4 = 2.3…

A:

Q: 4. A saturated solution of Magnesium hydroxide at 298 K contains 1.71 x 10-4 mol/L Mg2+ ions.…

A: Given :  [Mg+2] = 1.71 x 10-4 mol/L  Volume of Mg(OH)2 solution = 500 ml  Volume of NaOH solution =…

Q: A 1.000g sample of unknown Fe+2 content is titrated with potassium permanganate.  The final color…

A: Given the mas of the sample containing Fe2+(aq) = 1.000 g  Potassium permanganate, KMnO4(aq)…

Q: What is the solubility of BaSO 4 in 0.1625 M Na 2SO 4? K sp(BaSO 4) = 1.500e-9.

A: Solubility product of an electrolyte at a specific temperature is defined as the product of the…

Q: 2. Chromium (III) iodate, Cr(IO3)3, has a solubility product of 5.0 x 10-6. a. Calculate the…

A: a) The reaction will be, CrIO33 ⇔ Cr3+aq + 3IO33-aq The solubility of Cr(IO3)3 is, Ksp = s…

Q: A mixture contains 1.0 x 10-3 M Cu²+ and 1.0 x 10-3 M Mn²*. We want to separate these ions by…

A: The one which is less soluble will precipitate first.

Q: calculate the concentration of lead ion in saturated solution of lead chloride dissolve in 0.10 M…

A: Given : Ksp PbCl2 = 1.8×10-4 Concentration of lead chloride dissolve in 0.10 M NaNO3 = ?

Q: Will a precipitate of Mg(OH)2 form in a   0.0010 M solution of Mg(NO3)2 if the pH of the solution is…

A: For a precipitate formation, the ionic product of ions must be higher than the solubility product.…

Q: For the equilibrium  Al(OH)3 (s) ⇌ Al3+ (aq) + 3 OH-(aq) Ksp = 1.3 × 10-33  (a) What is the minimum…

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Q: Lead (II) fluoride has a Ksp value of 2.7x10-8. What is the concentration of Pb2+ and F- ions in a…

A: The solubility product constant (Ksp) describes the equilibrium between a solid and its constituent…

Q: If 10.0mL of 2.0x10^-3 M Cr(NO3)3 is added to 10.0mL of a pH = 10.0 NaOH solution, will a…

A: The number of moles of a substance is given as the mass of a substance upon its molar mass. The pH…

Q: Write a balanced net ionic equation to show why the solubility of Ni(CN)2(s) increases in the…

A: The net ionic equation depicting the solubility of nickel (II) cyanide in the presence of strong…

Q: An aqueous solution contains 0.10 M Ag", 0.10 M Cd2* and 0.10 M Mn2*. If sulfide ion, S2, is slowly…

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Q: Sodium thiosulfate can remove crystals of AgBr from black-and-white photographic film by reacting…

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Q: The solubility-product constant for PbI2 is 7.1x10-9 . Calculate the weight (in gram) of PbI2 that…

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Q: What is the molar solubility of Ag2SO4 in a solution that is 0.0522 M AgNO3? Ksp= 1.40x10^-5

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Q: What is the Cl- concentration just as Ag2CrO4 begins to precipitate when 1.0 M AgNO3 is slowly added…

A: Interpretation- Concentration of Cl- when AgCrO4 starts to precipitate Concept introduction-…

Q: A 100-mL sulfide-containing water sample was titrated with 12.15 mL of 0.041 M AgNO3 to determine…

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Q: A saturated solution of calcium iodate was made in a 0.0170 M potassium iodate solution. To…

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Q: Calculate the solubility of PbI2 solubility in a 0.20 M Pb(NO3)2 solution. Ksp 1.4 x 10^-8.

A: Ksp is the solubility product which is defined for the solid.

Q: 70

A: The ion product, Q for a compound is be expressed as : If Q > Ksp, the solution is…

Q: In the presence of CN, Fe+ forms the complex ion Fe(CN),*. The equilibrium concentrations of Fe+ and…

A: Equilibrium constant for any given reaction: Given data: Equilibrium concentration of Fe3+=8.5 x…

Q: Chromium (III) iodate, Cr(IO3)3, has a solubility product of 5.0 x 10^-6 . Calculate the solubility…

A: The equilibrium reaction during dissociation of Cr(IO3)3 can be written as follows : The expression…

Q: A solution has a concentration of 1.0 x 105M of both Fe2* and Co3. If strong base (OH') is slowly…

A:

Q: The concentration of iodide ions in a saturated solution of lead (II) iodide is ______M. The…

A: Given: Ksp i.e. the solubility product of PbI2 = 1.4 X 10-8. The solubility reaction of PbI2 can be…

Q: ?For Cu(OH)2, Ksp = 1.6 x 10-19. What is the molar solubility of Cu(OH)2 2.7 x 10-11 M .a 5.1 x…

A: Correct option C.   3.4 x 10-7 M

Q: The substance to be analyzed - is white, highly soluble in water salt. Interaction with water…

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Q: A solution contains 0.018 mole each of I-, Br-, and Cl-. When the solution is mixed with 200. mL of…

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Q: An aqueous solution containing Ca2+, Cl-, CO32-, and NO3- is allowed to evaporate. Which compound…

A: We are give different anionic species i.e Ca2+, Cl-, CO32-, and NO3-.

Q: A sample solution contains two unknown ions. A student did a series of tests on the solution, in the…

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Q: A solution is 5.0 × 10-5 M in each of these ions: Ag*, so;-, CI¯, and Co;-. Which precipitate will…

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Q: 9) Find the solubility product constant for lead (II) iodide if the concentration of l is found to…

A: Note - Since you have asked multiple question, we will do the first question for you. If you want…

Q: What is the maximum concentration of Ag⁺ that can be added to a 0.00140 M solution of Na₂CO₃ before…

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Q: In the presence of CN-, Fe3+ forms the complex ion Fe(CN)63-. The equilibrium concentrations of Fe3+…

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Q: A solution contains 1.0 x 10-2 M Ag+(aq) and 2.0 x 10-2 M Pb2 +(aq). When Cl-(aq) is added, both…

A: One compound or salt precipitates when its ionic product of its ionization is greater than its…

Q: What mass of NaCl is needed to precipitate all the silver ions from 20.0 mL of 0.100 M AgNO3…

A: 1- First determine the moles of Ag+ ion :  Molar mass of AgNO3 =  Moles of AgNO3 = [ Molarity ×…

Q: 3. Precipitate formation provides one means for re- covering precious metal ions from waste water.…

A: The precipitation reaction taking place is given as, => Ag+ (aq) + Cl- --------> AgCl (s)  1)…

Q: What is the solubility of PbSO 4 in 0.1868 M Na 2SO 4? K sp(PbSO 4) = 6.300e-7

A: The solubility of PbSO4 can be calculated as follows

Q: Suppose that we have a solution that is 0.0010 M Cl - and 0.100 M CrO4 2-. If we add 0.100 M AgNO 3,…

A:

Q: Determine the molar solubility of Agl in pure water. K sp (Agl) = 8.51 × 10-17 A. 2.77 x 10-6 M B.…

A: Assuming the molar solubility of AgI is s => s concentration of AgI will dissolve in water…

Q: Really hoping for solutions since I’m having a hard time with this. Pls. skip if unsure or not…

A: Solubility is the property of dissolution of a solute in a solvent to form a solution. The…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.