in a container containing 4 liters of 1% solution of calcium chloride Cacl2, solution 92 mg silver nitrate (solid). Accepting d = 1g / ml and Ksp of AgCl = 10-¹⁰, find the precipitate to be formed in this right.

in a container containing 4 liters of 1% solution of calcium chloride Cacl2, solution 92 mg silver nitrate (solid). Accepting d = 1g / ml and Ksp of AgCl = 10-¹⁰, find the precipitate to be formed in this right.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 100CP

See similar textbooks

Related questions

Q: If 1.0 mL of 1.0x10-3 M Ba(NO3)2 is added to 99.0 mL of 1.0x10-4 M Na2CO3, will BaCO3 precipitate…

A: Given, Volume of Ba(NO3)2 = 1.0 mL Molarity of Ba(NO3)2 = 1.0 x 10-3 M Volume of Na2CO3 = 99.0 mL…

Q: Calculate the solubility at 25 Celsius of CuBr in pure water and in a .0040 M CoBr2 solution. ksp…

A: Given:Concentration of CoBr2 = 0.0040M.Ksp of CuBr =6.27×10−9

Q: Will a precipitate form when 25 mL of 0.20M Ba(NO3)2 is mixed with 15 mL of 0.20M NaOH? (Ksp Ba(OH)2…

Q: Calculate Ksp for calcium hydroxide if a saturated solution contains 0.20M of calcium hydroxide.

A: Ksp is tge solubility product of sparingly soluble compound. It can be calculated as the product of…

Q: . Suppose 100.0 mL of a 0.0010 M CaCl2 solution is added to 50.0 mL of a 6.0 × 10-5 M NaF solution…

A: Given reaction and information,

Q: Consider the compounds with the generic formulas listed and their corresponding molar solubilities…

A: a) The solubility reaction of AX is given by AX (s) --------> A+ (aq) + X- (aq)…

Q: The solubility of barium chromate at 25 degrees C is 0.279 mg/ 100 mL. Calculate the Ksp of barium…

A: Solubility = 0.279 mg / 100 ml Solubility = 2.79 mg / L Solubility = 2.79 / 253 = 0.011 m moles…

Q: 96 mL of 0.080 M NaF is mixed with 32 mL of 0.20 M Sr(NO3)2. Calculate the concentration of Sr2+ in…

A: Volume = 96 ml of NaF volume = 32 ml of Sr(NO3)2 concentration = 0.080 M NaF concentration = 0.20 M…

Q: Q4. solution. (KB for ammonia (NH3) is 1.80×10) Calculate the molar solubility of Sn(OH)2 (Ksp =…

A: Given concentration of NH4NO3 = 5.00 M Kb for ammonia, NH3 = 1.80 x 10-5 Ksp of Sn(OH)2 = 3.00 x…

Q: 20.00 mL of 1.100 x 104 mol/L Pb(NO3)2 is mixed with 80.00 mL of a 4.450 x 10-2 mol/L Cal2. The Ksp…

Q: Determine the Ksp of mercury(I) bromide (Hg2Br2), given that its molar solubility i 2.52 x 10¯8 mole…

A: Solubility product(ksp) of mercury (I)bromide is given by :-Hg2Br2⇌Hg22+(aq) + 2Br-(aq)∴ ksp = Hg22+…

Q: If a solution contains 0.001 moles of CrO,2- per liter of solution, what [Ag*] must be exceeded by…

A: Given data: The concentration of CrO42- [CrO42-]=0.001 mol/L. The solubility product of Ag2CrO4 Ksp…

Q: If 100 mL of a 0.00075 M sodium sulfate is mixed with 50.0 mL of 0.015 M barium chloride, will a…

Q: If 125 mL of a solution containing 0.0400 M of Pb(NO3)2(aq) is mixed with 75.0 mL of a solution…

A: We have to find whether there will be precipitate formation of PbCl2 or not.

Q: a. Lead(II) chloride is a white pigment used in 15-century European sculptures. If 275 mL of a 0.134…

Q: An experiment includes precipitation of PbCl2 from 7.50 mL 0.340 M KCl and 15.34 mL 0.0421 M PbNO3.…

Q: At a certain temperature, the molar solubility of Ca(OH)2 in 0.03 M KOH is 1.0 x 10-6 mol/L. What is…

A: Ksp is known as solubility product constant. If any compound does not dissolved completely in the…

Q: A solution contains 6.32x10-³ M lead nitrate and 7.39×10-³ M silver acetate. Solid potassium iodide…

Q: When 15.0 mL of a 9.98×10 M sodium phosphate solution is combined with 12.0 mL of a 9.22×10 M…

A: The reaction quotient, Q for ant reaction aA+bB → cC+ dD is given by the formula :…

Q: How much lead(II) chloride will precipitate if 185 mL of 0.021 M sodium chloride is added to 235 mL…

Q: Zinc hydroxide Zn(OH), has Ksp=4.5x10-17 In pure water calculate its małor solubility ?

A: Given data contains, Ksp=4.5×10-17 The dissociation reaction of zinc hydroxide is given as,…

Q: Calculate the molar solubility of CdS in 0.10 M NH3. Enter your answer as scientific notation with…

A: Given, Ksp for CdS = 8.0 × 10-27 Kf for Cd(NH3)42+ = 1.0 × 107 we have to find molar solubility…

Q: If 650 mL of 4.15x10-4 mol/L BaCl2 is mixed with 550 mL of 4.00 x10-4 mol/L Na2SO4, will a BaSO4…

Q: What is the molar solubility of the hypothetical compound MBr3 in a solution containing…

A: Given: Concentration of NaBr = 0.3000 M And Ksp of MBr3 = 7.2 × 10-7.

Q: Calculate the solubility (mol/ L) of Cu(OH)2 in a) pure water and b) 0.001 NaOH Cu(OH)2 Ksp = 2.2 x…

A: Solubility calculation of a sparingly soluble salt:

Q: to 450 ml of 0.0001 M AgNO3 solution add 50 ml of 0.001M HCl solution. Will there be AgCl…

A: # The precipitation can only occur when the ionic product will exceed the solubility product. # So…

Q: You are trying to separate calcium ions (Ca2+) from lead ions (Pb2+), both present in a mixture and…

Q: If 50.0 mL of 1.50M silver nitrate solution is mixed with 25.0 mL of 1.50M sodium chloride 6.…

Q: alculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H2O. Ksp = 1.00×10-16 at a…

A: Molar solubility is defined as number of moles of solute that can be dissolved per liter of solution…

Q: Find the molar solubility of Ag2CO3 when the concentration of [H3O +] is 1.0x10 ^ 11 M. (Ksp for…

A: Find the molar solubility of Ag2CO3 when the concentration of [H3O+] is 1 x 1011 M . ( Ksp for…

Q: NazSO4 is added gradually to 100 cm3 of a solution that contains 0.15 M Ca2+ and 0.15 M Sr2* ions…

A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…

Q: The molar solubility of Ag2S is 1.26 x 10- 16 M in pure water. Calculate the Ksp for Ag2S. Select…

A: Given: The molar solubility of Ag2S, (s) = 1.26×10-16 M. The Ag2S will be partially dissociated as…

Q: A solution contains 1.33x102 M ammonium sulfate and 1.37x10-2 M sodium hydroxide. Solid lead acetate…

A: Given: Concentration of SO42- (from (NH4)2SO4) = 0.0133 M And the concentration of OH- ions (from…

Q: A solution is 0.050 M Pb +2. What minimum concentration ( in M) of Cl- is required to begin to…

A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…

Q: An imaginary ionic salt Na 5X has a molar solubility of 4.43*10^-12. What is the Ksp value for this…

A: molar solubility of salt = 4.43 * 10-12

Q: Which of the following salts has the least molar solubility in water? Select one: O a. Fes (Ksp = 4…

Q: Calculate the fluoride ion concentration required to begin precipitation of barium fluoride from a…

A: BaF2 ⇌ Ba2+ + 2F- Ksp = [Ba2+]•[F-]2 Given, [Ba2+] = 0.001 M Ksp = 1.7 x 10-6 Therefore, 1.7 x…

Q: What is the molar solubility of CaF2 (Ksp = 3.9 x 10-11)? A 6.24 x 10-6 M B 4.41 x 10-6 M 2.14 x…

Q: The Ksp of calcium fluoride is 5.3 * 10^-9. What is the solubility of calcium fluoride in 2.72 *…

A: Solubility product is an ionic product at equilibrium

Q: To 0.360 L of 0.150 M NH 3 H is added 0.140 LL of 0.110 M MgCl 2.

A: first calculate the moles of every compound used n(NH3)= (0.150 mol/L )(0 .360 L) = 0.054 moles NH3…

Q: The solubility products of Fe(OH)2 and Fe(OH)3 are 10^-17 and 10^-38 respectively. If the…

A: Given data: The solubility product of Fe(OH)2 Ksp= 10-17. The solubility product of Fe(OH)3 Ksp=…

Q: Lead (II) chloride, PbCl2, has Ksp = 1.6 x 10–5. (a) Determine the solubility of PbCl2 expressed in…

Q: assume that 200 ml of 0.8 M KCl solution is mixed with 300 ml of 0.01 M AgNO3 solution. Knowing that…

A: To solve this problem we have to first calculate the number of moles of Ag+ ion and the number of…

Q: An imaginary ionic salt NA2X has a molar solubility of 3.84 x 10 -8 What is the Kgp value for this…

A: Given, Molar solubility of the ionic salt (Na2X) = s = 3.84 × 10-8 M Solubility product constant…

Q: A solution contains 5.61×10 M silver acetate and 5.52x10 M calcium nitrate. Solid sodium sulfite is…

A: The question is based on the concept of solubility product principle. It that states that when a…

Q: Calculate the molar solubility of Cr(OH)3 (Kgp = 6.3 x 10-31 at 25 °C). 5.4x10-11 M O 7.9×10-16 M O…

A: Given data :- Ksp of Cr(OH)3 = 6.3 x 10-31 Temperature = 25 0C

Q: Solid NaI is slowly added to a solution that is 0.010 M in CuI (Ksp = 5.1 x 10-12 ) and 0.010 M in…

Q: Calculate the solubility at 25 °C of CaF₂ in pure water and in a Round both of your answers to 2…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

100%

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

You are trying to separate calcium ions (Ca2+) from lead ions (Pb2+), both present in a mixture and each at a concentration of 0.010 M. You will accomplish this by titrating (adding slowly) sodium sulfate (Na2SO4). (Ksp for CaSO4 = 4.9 x 10-5; Ksp for PbSO4 = 1.3 x 10-8 at 25 °C.). Which will be the first salt to precipitate? What will the concentration of the first ion to precipitate (Ca2+ or Pb2+) be when the second salt begins to precipitate?
*SHOW COMPLETE SOLUTION* If 100 mL of a 0.00075 M sodium sulfate is mixed with 50.0 mL of 0.015 M barium chloride, will a precipitate form? Ksp of barium sulfate is 1.1 x 10-10 . ANS: Qsp = 2.5 x 10-6 ; A precipitate forms. Will a precipitate form when 0.10 L of 8.0 x 10-3 M Pb(NO3 )2 is added to 0.40 L of 5.0 x 10-3 M Na2SO4? Ksp PbSO4 is 6.3 x 10-7 . ANS: Qsp = 6.4 x 10-6 ; A precipitate forms.
Mix 4 liters of 0.02 N K2SO4 solution with 6 liters of solution containing 6.62 grams of lead nitrate Pb (NO3) 2. Does precipitate form in this case, given that Ksp of PbSO4 = 10-⁸?
Estimate the solubility of lead(II) iodide in a. moles per liter of pure water. Solubility = mol/L b. in grams per liter of pure water. Solubility = g/L Ksp for lead(II) iodide is 9.8 x 10-9.
If 100.0 g calcium phosphate (Ksp= 1.3 x 10^-32) are placed in enough water to generate 750.0 mL of solution, calculate the molar solubility of the calcium phosphate solution and the molar solubility of the calcium ion if 30.0 mL of 0.400 M calcium nitrate solution is added to the original solution.
35.0 mL of 6.7 x 10-4 M Ca(NO3)2 is mixed at 25˚C with 65.0 mL of 8.4 x 10–5 M Na2CO3.Compute the initial concentrations of [Ca2+]init and [CO32-]init after mixing.Assume volumes are additive. 3. Should a precipitate form when the solutions in prelab questions #2 above are mixed?Support your answer with a calculation
Sodium carbonate, Na2CO3, is added dropwise to a solution that contains 1.0 X 10-2 M Ag+ and 5.0 X 10-2 M Cd2+. Specify the minimum molar concentrations of carbonate ion needed to precipitate each cation. (Ksp = 8.1 X 10-12 for Ag2CO3; Ksp = 1.8 X 10-14 for CaCO3)
A solution is prepared by mixing 50.0 mL of 0.50 M CaCl2 with 50.0 mL of 0.50 M CoCl2. When NaOH is slowly added to the mixture, which precipitates first? Ksp[Ca(OH)2] = 6.5 × 10–6, Ksp[Co(OH)2] = 2.5 × 10–16
Calculate the molar solubility and solubility in g/L of lithium fluoride (LiF, 25.939 g/mol) in pure water. Ksp = 1.7 x 10-3 Calculate the molar solubility and solubility in g/L of gold(III) chloride (AuCl3, 303.33 g/mol) in pure water. Ksp = 3.2 x 10-25 Calculate the molar solubility and solubility in g/L of gold(III) chloride in a solution that is 0.010 M in MgCl2. Ksp = 3.2 x 10-25
does precipitate form when we mix 10 liters of solution, where 20g of K2CrO4 and 6 liters of 0.001 N solution of barium nitrate Ba (NO3) 2? Ksp (BaCrO4) = 10-janë are dissolved.
An analytical chemist has been given the task of precipitating lead cation (Pb2+) out of solution that is 0.424 M in Pb2+ . At her disposal is a large bottle of solid sodium iodide (NaI). What must the concentration of iodide be for precipitation to begin? (The Ksp of lead iodide is 9.8 x 10-9).
Suppose that 100 mg of Na2CO3 and 100 mg of CaCl2 are added to 1 L of water at pH 9.0 and 25 ̊C. Will a CaCO3 precipitate form? Solve for a closed system with a constant pH. Ksp = 5 x 10-9 at 25 ̊C.