Answered: Which of the following salts is most…

Which of the following salts is most soluble? Ca2(PO4)3 - Ksp = 2.1 10-33 AgCl - Ksp = 1.8 * 10-10 Pbl2 - Ksp = 8.7 10-9 Ga(OH)3 - Ksp = 8.6* 10-9

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.4: Solubility Of Salts

Problem 4RC: 4. What is the solubility of PbSO4 in water at 25°C if the solution already contains 0.25 M...

See similar textbooks

Related questions

Q: What is the molar solubility of a X4Y, (Ksp = 8.67 x 10-7 ) is dissolved in a 3.05*10-2 M XCI4…

A: Given, Ksp of X4Y2 =8.67×10-7 and 3.05×10-2 M XCl4 solution then…

Q: The concentration of SrCO3 in a saturated aqueous solution of salt at 25°C is 3.05 x 10 M. What is…

A: Given Chemical Reaction SrCO3 ( S ) ------------> Sr+2 ( aq ) + CO3 2- ( aq ) Solids and…

Q: The Ksp for Fe(OH)2 at 25°C is 1.6 x 10-14. The solubility of Fe(OH)2(s) in an aqueous solution at…

Q: Calculate the solubility of AgBr in 225 mL of water to which 0.15 g of NaBr has been added. AgBr(s)…

A: Since we have NaBr in solution which has a common Br ion with AgBr hence the concentration of Br-…

Q: 0.281 mol AgNO3 and 3.17 mol NH3 were added to enough water to give 1.00 L of solution at 25 °C.…

Q: Silver carbonate has a Ksp = 9.05×10-10 and a solubility of 0.0006093 M in water. Solid silver…

Q: C. 8.12 d. 3.44 e. 5.28 3. Determine the solubility of the ions that is calculated from the Ksp for…

Q: For p=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X-is 0.75. Calculate how…

A: Answer: For an ion in an electrolyte, its active mass is always the product of its activity…

Q: Calculate the equilibrium Ni2+ concentration of a solution that has been prepared by mixing 50.0 ml…

Q: The solubility of PbSO4 (Ksp=6.3x10-7) decreases with adding which of the following? a. Na2CrO4…

A: In water PbSO4 dissociates as: PbSO4→Pb2++So42- Let the solubility be S mol/L…

Q: solution containing copper(II) nitrate (aq) first has some aqueous ammonia added to it. A white…

A: The question is based on the concept of qualitative analysis. to identify the copper ions in the…

Q: Which of the following is most soluble? A) AgCl: Ksp= [Ag+][Cl–] = 1.82 x 10-10 B) AgBr: Ksp=…

A: The value of Solubility product (Ksp) determines the degree to which the compound can dissociate…

Q: Calculate the Ksp for magnesium fluoride if the solubility of MgF2 in pure water is 0.000234 M.…

A: Dissociation Reaction of MgF2 is as shown below: MgF2 --> Mg2+ +…

Q: 25). The solubility of BiI3 (dissociates to Bi3+ ions and I– ions) is 0.00778 g/L. What is Ksp for…

A: Given : Solubility of BiI3 = 0.00778 g/L.

Q: Calculate the solubility (in mol/L) of silver oxalate, Ag2C204, in 0.15M Na2C204. = 1.0 x 10-11 Ksp…

A: Ksp is the product of concentration of each ions and each ions are raised by respective powers.

Q: 12. A solution containing both Mn+2 and Cd+2 is saturated with H₂S gas, after which the…

A: According to bartleby guidelines we're supposed to answer only first question among these So please…

Q: Calculate the minimum concentration of Cr3+ that must be added to 0.095 M NaF in order to initiate a…

A: Given - - > Concentration of NaF = 0.095 M Now CrF3 = [Cr3+] [F-]

Q: Find the solubility of Cr(OH)3 in a buffer of pH 13. (Ksp of Cr(OH)3 is 6.3x10-31; Kf of Cr(OH)4- is…

Q: After mixing an excess PbCl2 with a fixed amount of water, it is found that the equilibrium…

A: We will first write solubility product equation for PbCl2 and then calculate Ksp .

Q: What is the solubility of CdS (Ksp = 1.0 x 10 28) in pure water? 1.0 x 107 M 1 x 10 14 M 1.0 x 10 28…

A: The solubility equilibrium is :

Q: CuBr is dissolved in water and the following concentrations were found: [Cu+]=1.06*10^-6 M and…

A: Solubility Product : It is generally an equilibrium constant , also it is defined for a solid…

Q: Determine the molar solubility of BaF2 in pure water. Ksp for BaF2 = 2.45 × 10-5. A) 1.83 × 10-2 M…

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: Calculate the solubility of AgCN (Ksp = 2.2 x 10-12) in a solution containing 1.0 M H*. (Ka for HCN…

A: The solubility reaction of AgCN can be written as 1) AgCN (s) ---------> Ag+ (aq) + CN- (aq)…

Q: How many moles of Fe(OH)2 (Ksp = 1.82 x 10-15) will dissolve in 1.5 liter of water buffered at pH =…

A: Given that : Ksp for Fe(OH)2 = 1.82×10-15 We have to determine how many moles of this Fe(OH)2 will…

Q: The solubility of solid silver chromate, which has a Ksp = 9.0 x 10-12 at 25°C, is determined in…

A: Given that: Ksp = 9.0×10-12 molarity of silver nitrate = 0.1 M molarity of sodium chromate = 0.1 M…

Q: 2. What concentration of OH is required to begin the precipitation of Cu(OH)2 from a solution…

A: Given, Concentration of Cu2+ = [Cu2+] = 0.10 M Ksp for Cu(OH)2 = 2.2 × 10-20 Concentration of OH- =…

Q: B. Solid AgCl (Ksp = 1.8×10-10 ) is dissolved in 1 Liter of water , then 0.585 gm of sodium chloride…

A: AgCl will dissociate into ions according to the equation: AgCl (s) ⇌ Ag+(aq) + Cl-(aq) If M is the…

Q: (a) Given that the solubility product of rhodochrosite, MNCO3, is 10-93, calculate the equilibrium…

A: In a solution that contains a solute having low solubility, the ions tend to form precipitate. An…

Q: The Ksp for PbI2(s) is 1.4 × 10-8. Calculate the solubility of PbI2(s) in 0.061 M NaI.

Q: 1. Calculate the SP of iron (II) sulfide if 100 cm3 of its saturated solution contains 1.97*10-8 g…

Q: A solution is prepared that has (EDTA1=0 300 M and (CO,2-1= 0 600 M What is the maximum allowable…

A: (i) In a solution of EDTA-4 and CO3-2, Fe+2 is added. This results in the formation of a complex of…

Q: 38. What is the molar solubility of Ca(OH)2 in pure water? Given: Ksp = 4.68 x 10-6 for Ca(OH)2. A)…

A: “Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: What mass of ZnS (Ksp = 2.5 x 10-22) will dissolve in 325.0 mL of 0.050 M Zn(NO3)2? Ignore the basic…

A: Since Zn(NO3)2 is completely soluble in water as Zn(NO3)2 -----> Zn2+ + 2 NO3- Hence…

Q: Given that Ksp for Ca3(PO4)2 = 2.1 x 10-33, calculate the molar solubility for Ca3(PO4)2 in pure…

Q: 26. Ksp(Cd(OH):(s)) = 6.4 x 10-15. Determine the molar (mol/L) solubility of Cd(OH)2(s) in a buffer…

A: Ther eis more than one question and as per answering guidelines I can only answer first one,if you…

Q: Calculate the molar solubility of BaCO3in a 0.10 M solution of Na2CO3(aq). (Ksp(BaCO3) = 8.1 x 10-9)

A: The given reaction of BaCO3 - Now calculate the molar solubility of BaCO3 -

Q: What is the molar solubility of ZnC₂O4 (Ksp = 2.7 x 108) in 0.100 M Na₂C₂O4 solution? ZnC₂O4(s) Zn²+…

Q: For Ni(OH)2 (Ksp = 1.6 x 10 16) dissolved in a 0.033 M NizP2 solution, calculate: %3D a. Solubility…

Q: The solubility of Ag2CO3 is measured and found to be 3.58×10-2g/L. Use this information to calculate…

Q: Calculate the solubility of Zn(OH)2 ,(KSP Za(OH):-1 x 10-17 in a solution with pOH-8

Q: Ksp for Agl = 1.2 x 10-17. Calculate the molar solubility of Agl in 1 x 10-4 molar AGNO3 solution. O…

A: The given data contains, Ksp for AgI=1.2×10-17Ag+=1×10-4 M.

Q: Is it possible to precipitate 99.0% of 0.010M Ce3+ by adding oxalate (C2042-) without precipitating…

Q: Silver carbonate has a Ksp = 3.33×10-12 and a solubility of 0.00009407 M in water. Solid silver…

A: The question is based on the concept of solubility product. we have to determine the concentration…

Q: Enough silver sulfite (Ag2SO3 , Ksp = 1.5 × 10-14 ) is dissolved in 2.00 L to produce a saturated…

A: Given: pH = 2.00 And volume of solution = 2.00 L Concentration of H+ = 10-pH = 10-2.00 = 1.0 × 10-2…

Q: For AgOH, Kgp = 1.5 x 10*8. What is the molar solubility of AgOH in a solution containing 0.1 M of…

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

Q: The solubility of Cr(OH)3 in 0.1 M solution of NaOH is (Ksp of Cr(OH)3 is 6.3 × 10-31) 1.26 x 10-32…

A: Given : [OH-] = [NaOH] = 0.1 M Balance chemical equation : Cr(OH)3…

Question

Which of the following salts is most soluble?
Ca2(PO4)3 - Ksp = 2.1 10-33
AgCl - Ksp = 1.8 * 10-10
Pbl2 - Ksp = 8.7 10-9
Ga(OH)3 - Ksp = 8.6* 10-9

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
Calculate the solubility in grams per 100 ml H2O for La(IO3)3 (s), Ksp= 6.1*10^-12 BaF2 (s), Ksp= 1.8 *10^-7 CaCO3 (s), Ksp=5.0*10^-9 assuming density of water is 1 g/cc
Calculate the solubility of Au2CrO4 in a 0.13 M solution of Na2CrO4. Ksp for Au2CrO4 is 7.3x10^-40
1. The solubility of Ag₂SO₄ in water at 25 °C is 0.0155 M. What is Ksp for Ag₂SO₄? 2. What is the solubility of La(IO₃)₃ in a solution that contains 0.100 M La³⁺ ions? (Ksp of La(IO₃)₃ is 7.5 × 10⁻¹²)
The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The solubilityof Cd(OH)2can be increased through formation of thecomplex ion CdBr42 - (Kf = 5 x 103). If solid Cd(OH)2 isadded to a NaBr solution, what is the initial concentrationof NaBr needed to increase the molar solubility of Cd(OH)2to 1.0 x 10-3 mol/L?
gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each.(a) BaSiF6, 0.026 g/100 mL (contains SiF6 2− ions)(b) Ce(IO3)4, 1.5 × 10–2 g/100 mL(c) Gd2(SO4)3, 3.98 g/100 mL(d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr6 2− ions)
If 500.0 ml of 4.2 x 10^-3 M Ce(NO3)3 is mixed with 800.0 ml of 5.6x10^-3M NaIO3, will theprecipitate Ce(IO3)3 (Ksp = 1.9 x 10^-10) form?
Enough silver sulfite (Ag2SO3 , Ksp = 1.5 × 10-14 ) is dissolved in 2.00 L to produce a saturated solution. Calculate the mass of silver sulfite that dissolved in 2.00 L in a neutral solution and in a pH = 2.00 solution.
If 50.0 g of silver phosphate (Ksp = 1.8 x 10-18) are placed in enough water to generate 500.0 mL of solution, calculate the following: The molar solubility of the silver phosphate solution. The molar solubility of the silver ion if 30.0 mL of 0.400 M silver nitrate solution is added to the original solution.
51 mL of 0.060 M NaF is mixed with 17 mL of 0.15 M Sr(NO3)2. Calculate the concentration of F- in the final solution. Assume volumes can be added. (Ksp for SrF2 = 2.0×10-10) 0.038 M 0.0075 M 0.045 M 0.015 M 0.00012 M
Write the equation for the dissolution of each solid and the Ksp expression. A. CaF2(s) B. Ag2CO3(s) C. Ba3(PO4)2
0.281 mol AgNO3 and 3.17 mol NH3 were added to enough water to give 1.00 L of solution at 25 °C. Calculate the equilibrium concentration of free silver ion, [Ag+], in this solution. The formation constant for Ag(NH3)2+ (Kf) = 1.50x107 at 25 °C. 0×100 M 2.75×10-9 M 7.18×10-9 M 2.24×10-9 M 4.97×10-9 M