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Lead(II) nitrate is added slowly to a solution that is
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- Problem 4-4 When a solution of copper(II) chloride, CuCl2, is added to a solution of potassium sulfide, K2S, a black precipitate of copper(II) sulfide, CuS, forms. Write the net ionic equation for the reaction.arrow_forwardLearning Goal: To understand the relationship between precipitation and the solubility product and to be able to predict whether a substance will precipitate or not. Precipitation is the formation of an insoluble substance. For the equation AB(s)⇌A+(aq)+B−(aq)AB(s)⇌A+(aq)+B−(aq), precipitation represents a shift to the left and the production of a solid. From Le Châtelier's principle, we know that when the product of the concentrations of A+A+ and B−B− ions gets above a certain level, the reaction will respond by shifting left to decrease the concentrations of A+A+ and B−B− ions. This critical level, KspKsp Q=[A+][B−]Q=[A+][B−]. where QQ is the ion product. When Q>KspQ>Ksp, precipitation occurs until QQ is equal to KspKsp When Q≤KspQ≤Ksp, a precipitate does not form. Part A Calcium chromate, CaCrO4CaCrO4, has a KspKsp value of 7.10×10−47.10×10−4 . What happens when calcium and chromate solutions are mixed to give 2.00×10−2mol L−12.00×10−2mol L−1 Ca2+Ca2+ and 3.00×10−2mol…arrow_forwardSuppose you have equal volumes of saturated solutions of NaNO3, Na2SO4, and PbS. Which solution would dissolve the most lead(II) sulfate, PbSO4?arrow_forward
- issue 21A saturated solution of copper (II) phosphate, Cu3(PO4)2, has a concentration of 6.1 x 10-7 g per 1.00 x 102 mL of solution at 25 °C. What is Kps for Cu3(PO4)2 at 25°C?arrow_forwardAnswer (i) At 20°C the solubility limit of silver(I)sulfate (Ag2SO4) is 0.800 g/100 mL.What is the molarity of such a solution? (iii) What volume in mL of concentrated H2SO4 (18.0 M) must be used to prepare400 mL of 3.0 M H2SO4 solution?arrow_forwardThe molar solubility of aluminum hydroxide is 0.0610 mol/L at a certain temperature. Calculate Kspfor aluminum hydroxide at this temperature. Express your answer to three significant figures. Ksp = Answerarrow_forward
- Calculate the molar solubility of calcium phosphate Ca3(PO4)2 Ksp=2.0×10−29 when dissolved in a 0.250M solution of calcium chloride. CaCl2 is a soluble salt.molar solubility = Answerarrow_forwardA solution contains 1.45×10-2 M ammonium sulfate and 1.29×10-2 M sodium fluoride.Solid calcium acetate is added slowly to this mixture.A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of calcium ion when this precipitation first begins?[Ca2+] = M Submit Answerarrow_forwardWhat is the molar solubility of AgCl (Ksp = 1.80 × 10⁻¹⁰) in 0.410 M NH₃? (Kf of Ag(NH₃)₂⁺ is 1.7 × 10⁷) (Gpt/ai wrong answer not allowed) Ans should correctarrow_forward
- The beaker on the left below represents a buffer solution of a weak acid HA and its conjugate base, A. (Water molecules and spectator ions have been omitted for clarity.) a Which beaker on the right, X or Y, depicts the solution after the addition of two formula units of NaOH? b How many HCl molecules can be added to the original buffer solution before the buffer capacity is exceeded? c Draw a picture of the solution where the buffer capacity has been exceeded by the addition of HCl.arrow_forward3) Which of the following compounds are insoluble? Select all that apply: CaCO3; Cu(OH)2; CaCl2; Pb(NO3)2; Na2S 4)a) Write the net ionic equation for the following reaction: 0.10 M KOH and 0.10 M CoBr2 b) What is the formula of the precipitate?arrow_forwardQuestion 10 A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation.The I– concentration, which is 8.50×10-5 M, is 10,000 times less than that of the PO43– ion at 0.850 M .A solution containing the silver(I) ion is slowly added. Answer the questions below.Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. Calculate the minimum Ag+ concentration required to cause precipitation of Ag3PO4.arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning