Manganese(II) sulfide is one of the compounds found inthe nodules on the ocean floor that may eventually be a primarysource of many transition metals. The solubility of MnS is 4.710⁻⁴ g/100 mL solution. Estimate the Kₛₚ of MnS.

Manganese(II) sulfide is one of the compounds found inthe nodules on the ocean floor that may eventually be a primarysource of many transition metals. The solubility of MnS is 4.710⁻⁴ g/100 mL solution. Estimate the Kₛₚ of MnS.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 91QRT: Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium...

See similar textbooks

Related questions

Q: The solubility of zinc cyanide at 25°C is 1.66 x 10-6 g/ 100 mL. Calculate the value of kps for this…

A: The ksp of a general chemical equation is - AB(s) --------> A+(aq) + B-(aq) Ksp = [A+] [B-] where…

Q: Calculate the solubility of TlBrO3(s) in water in grams per liter at 25C given that Ksp=1.1x10^-12…

A: Given-> Ksp of TlBrO3 = 1.1 × 10-12

Q: The concentration of S2- in a saturated solution of FeS is 6.17x10-10 mol/L at a certain…

A: We have to predict the Ksp of given salt.

Q: Calculate the molar solubility (in mol/L) of Ag2S(s) at 25 °C in a solution of 0.30 M Na2S(aq). Ksp…

A: The majority of ionic compounds are water-soluble. When a substance is soluble, it dissociates into…

Q: The solubility of Ag(I) in aqueous solutions containing dif-ferent concentrations of Cl is based on…

A: "Since you have posted a question with multiple sub-parts , we will solve first three sub-parts for…

Q: What is the molar solubility of a salt Cal2 in 0.013 M of L aqueous solution at 25 °C? The value of…

A: The solubility equilibrium is: CaL2s⇌Ca2+aq+2L-aq The expression for solubility product for CaL2 is:…

Q: How do you find the solubility constant for Al(OH)3, MnS, and Ca3(PO4)2?

A: For calcium phosphate;

Q: What is the solubility of La(IO,), in a solution that contains 0.400 M IO, ions? (Ksp of La(IO,), is…

A: Ksp=7.5*10-12 IO3-=0.400M

Q: In nature, silver iodide (AgI) is obtained in the form of the mineral iodargyrite. This compound has…

A: A. As we add KI or AgNO3 in a solution containing AgI solubility of AgI decreases and it…

Q: Calculate the solubility of FECO3 (in mol/L) in the following. Assume the Kp of FECO3 = 3.5 x 10-11…

Q: At 20 °C (293 K) and a partial pressure of 105 Pa, the solubility of CO2 in water is 0.169 g/100 mL.…

A: According to Henry's law, the solubility of the gas divided by its pressure is constant: C1P1=C2P2…

Q: An ionic compound A2B dissociates in water according to the equation A2B(s) ⇌ 2A+(aq) + B2–(aq)…

Q: The solubility of Na2CO3 in water at 0ºC is 7g/100mL. What is the Ksp?

A: Density = 7 g/100 ml ...Or because 1L = 1000 ml ....so, = 7 g/100 ml × (1000 ml / 1L ) = 70…

Q: 4. Calculate Ksp for the ff. substances, given the molar concentration of their saturated solution.…

A: Given : Solubility of Ag2SO4 in saturated solution(S) = 1.5 x 10-2 mole/litre Solubility of…

Q: The Ksp of copper(II) carbonate, CuCO3, is 1.4 × 10-10, Calculate the solubility of this compound in…

A: Given Ksp = 1.4 × 10-10 Solubility (S) = ?

Q: What is the molar solubility of nickel(II) sulfide in 0.092 M KCN? For NiS, K- 3.0 x 1019, for…

A: Given: The concentration of KCN is 0.092 M. The solubility product of NiS and the formation constant…

Q: Calculate the solubility (in M) of cobalt(I) hydroxide, Co(OH)2(s) in H2O. Ksp = 2.70x10-16 at a…

Q: What is the maximum concentration of Mg2+ ions that can remain dissolved in a solution that contains…

A: To calculate maximum dissolved [Mg2+] , We will calculate hydroxyl ion concentration from the buffer…

Q: What is the molar solubility of BaF2 (Ksp = 1.8 x 10-7) in a solution containing 0.33 M KF(aq)?

A: BaF2(aq) -----> Ba+2(aq) + 2F-(aq) Ksp = 1.8 x 10-7

Q: 7. A saturated solution of lead(II) bromide contains 0.384 g of PbBr2 per 100. mL of solution. What…

A: Welcome to bartleby ! Introduction : We have to calculate Solubility product .

Q: The solubility of BaCrO4(s) (MM= 253.32) in water is 3.7 milligrams in 1.0L at 25°C. What is the…

A: BaCrO4 ---> Ba2+ + (CrO4)2- s s Ksp = s × s

Q: 10) How many miligrams of BaSO4 are dissolved in a 225 mL sample of BasO(aq)? (Hint: calculate the…

Q: What is the solubility of La(IO,), in a solution that contains 0.400 M IO, ions? (Ksp of La(IO,), is…

A: Welcome to bartleby !

Q: Ksp for copper (II) phosphate, Cu3(PO4)2 is 1.0 x 10-37. Calculate the following: a. molar…

A: Welcome to bartleby ! We have to calculate Solubility and molarity .

Q: Calculate the solubility (in g/L) of CaSO̟(s) in 0.500 M Na, SO̟(aq) at 25°C. The Ksp of CaSO, is…

A: The solubility of a salt decreases in the presence of common ion. The anion (SO42-) is common in…

Q: The Ksp of CaSO4 is 4.93× 10–5. Calculate the solubility (in g/L) of CaSO4(s) in 0.250 M Na2SO4(aq)…

A: Equation for ionisation of CaSO4 :CaSO4 → Ca2++SO42− S S…

Q: 4. What is the solubility in mol/L of barium sulfate in water if its Ksp is 1.5x10⁹?

A: We know that the solubility product of ionic compounds can be defined as the solubility product is a…

Q: In the laboratory, a general chemistry student measured the pH of a 0.359 M aqueous solution of…

A: PH + POH = 14 [OH-] = (Kb × C )1/2

Q: The molar solubility of Fe(OH)2 at 25 °C is 1.6×10−5. What is Ksp for Fe(OH)2? 1.0×10−9…

A: The solubility of Fe(OH)2 is shown below:

Q: The solubility of lead(II) fluoride, PbF2, in pure water is 2.1 × 10–3 moles per liter. Calculate…

A: The solubility is taken as ‘s’. The expression for Ksp calculation is as shown below:

Q: The solubility of MgSO4 in H2O is 9.3 x 10^-3 mol/L. What's the KSP of MgSO4

Q: 2- The concentration of SO, in a saturated solution of Hg2SO4 is 5.54x10-3 mol/L at a certain…

A: Given- Concentration of SO42- = 5.54 × 10-3 Mole/L Ksp of the compound=?

Q: 14. The Kp of PbSO, in water at 25°C is 1.23 X 107. It's molar solubility is ....

A: Please note- As per our company guidelines we are supposed to answer only one question. Kindly…

Q: What is the maximum solubility of Ag2S in a solution that is 2.5 x 10$ M in S2? Ksp(Ag2S) =1.0 x…

A: Silver sulphide Ag2S is a sparingly soluble salt. It dissociates as, Ag2S →2Ag+ +S2-

Q: 1. Calculate the Ksp for MgF2 if it has a solubility of 5.3 x 103.

Q: In which of the following aqueous solutions will Fe(OH)3 be most soluble (i.e. highest molar…

A: Correct answer is (B) 0.150 M HNO3. Solubility of Fe(OH)3 will be maximum in 0.150 M HNO3 solution…

Q: The solubility of calcium arsenate (Ca3(AsO4)2, molar mass = 398.078 g) in water is measured to be…

A: given solubility in g/L. If we want convet solubility into molar solubility Simply divide the…

Q: Calculate the solubility of silver acetate.1 (CH;COOA9) in water at 25 °C, assuming * .the DHLL to…

A: The solubility product constant is the equilibrium constant for the dissolution of a solid substance…

Q: At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0077 M. What is the value of…

A: Ksp is the kind of equilibrium constant when a solid substance dissolves into an aqueous solution.…

Q: 5. Determine the solubility (g/L) for Iron (II) hydroxide at 25.0°C. Ksp = 1.1 x 10 36 %3D

Q: Copper(I) ions in aqueous solution react with NH, (aq) according to Cu*(aq) + 2 NH, (aq) → Cu(NH, ){…

A: "The maximum amount of solute that can dissolve in a known quantity of solvent at a certain…

Q: the molar solubility for Fe(oh)3 in an aqueous solution was determined to be 4.0x10^-3 what is the…

A: The term molar solubility can be defined as the number of moles of a given substance which can be…

Q: Given the equation Ag*(aq) + 2 NH, (aq) → [Ag(NH,),]*(aq) Kf = 2.00 x 107 determine the…

Q: The solubility of calcium arsenate (Ca3(AsO4)2, molar mass = 398.078 g) in water is measured to be…

A: The solubility (S) of calcium arsenate [(Ca3(AsO4)2 is 0.012 g L-¹. The molar mass of calcium…

Q: The molar solubility for CaF2 in water at 25oC is 2.1×10-4 M. What is its Ksp?

A: The solubility expression for CaF2(s) is shown below:

Q: Which ONE of the following is the correct concentration of Cu* ions present in a saturated solution…

Q: Calculate the solubility (in g/L) of CaSO, (s) in 0.300 M Na, SO,(aq) at 25°C. The Ksp of CaSO, is…

Q: The solubility of silver phosphate, Ag3PO4, at 25°C is 1.59 × 10–5 mol/L. What is the Ksp for the…

A: Given that The solubility of silver phosphate, Ag3PO4, at 25°C = 1.59 × 10–5 mol/L. To find: Ksp…

Q: 1. The solubility of copper(I) chloride is 0.0391 g/L. Calculate the Ksp for copper(I) chloride

Q: At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0060 M. What is the value of…

A: Ksp is used to denote the solubility product which may be calculated by the product of concentration…

Q: What is the iron(II) ion concentration in a solution prepared by mixing 353 ml. of 0.446 M iron(II)…

Q: Calculate the mass solubility of AgCO (K = 8.1 x 10, MM = 275.74 g/mol) in a 0.010 M AgNO solution…

A: The compound is actually Ag2CO3(s) with Ksp = 8.1*10-12 The other compound is AgNO3. Since AgNO3…

Q: Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12×10−12. What…

A: The presence of compounds (containing same ions) in partially dissoluble salts results in reduction…

Q: Calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na₂SO4 (aq) at 25°C. The Ksp of CaSO4 is…

Question

Definition Definition Elements containing partially filled d-subshell in their ground state configuration. Elements in the d-block of the periodic table receive the last or valence electron in the d-orbital. The groups from IIIB to VIIIB and IB to IIB comprise the d-block elements.

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

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

Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
What would be the KPs value of Al(OH)3, considering that its solubility is 2,5 x 10^-8 mol/L?
write out the equilibrium expression for the mineral dissolution of Al(OH)3 in water
Consider a body of water in equilibrium with solid calcium sulfate, CaSo4, for which Ksp= 3.0 x 10^-5 at 25 degrees C. Calculate the solubility, in g/L, of calcium sulfate in water assuming that other reactions are negligible. *
Calculate the Gibbs energy and equilibrium constant for the chemical reaction at a temperature of 298.15 K. Hg2Cl2(s) → → 2 Hg(l) +Cl2(g). Does the value of the equilibrium constant you calculated describe your understanding of the spontaneity of the reaction in the direction of the arrow?
a)For the reaction given in Part A, how much heat is absorbed when 3.10 molmol of AA reacts? Express your answer numerically in kilojoules. b)For the reaction in Part A, ΔrS∘=25.0 J K−1 mol−1ΔrS∘=25.0 J K−1 mol−1. What is the standard Gibbs energy of reaction at 281 KK , ΔrG∘ (281K)ΔrG∘ (281K)? Express your answer numerically in kJ mol−1kJ mol−1.
The equilibrium constant for the reaction CO(g) + H2O(g) ⇌ CO2(g) + H2(g) is K = 1.03 × 105 at 298.15 K. Calculate the standard reaction Gibbs energy at this temperature.
Estimate the temperature at which the equilibrium constant for the decomposition of CaCO3(s, calcite) to CO2(g) and CaO(s) becomes 1; assume pCO2 = 1 bar .
The decomposition of a generic diatomic element in its standard state is represented by the equation 1/2 X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.34 kJ·mol−1 at 2000. K and−50.82 kJ·mol−1 at 30003000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, ΔGf=4.34 kJ·mol−1. What is K at that temperature?
Given the following two measurements of the equilibrium constant for a reaction, calculate ΔH° for the reaction. (kJ/mol) T, °C K 30.0 5.2 x 103 50.0 15.4 x 104
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?
How do you find the solubility constant for Al(OH)3, MnS, and Ca3(PO4)2?