Answered: The molar solubility in mol/L of…

Science

Chemistry

The molar solubility in mol/L of Mg(OH)2 (Ksp=1.8x10-11) is 4.2x10-6M 1.8x10-11M 2.6x10-4M 1.7x10-4M

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 73QRT

See similar textbooks

Related questions

Q: The molar solubility of the metal hydroxide (M(OH)2) in water is: M(OH)2 = M2+ + 2ОН Ksp = 5.02 x…

Q: The molar solubility of barium phosphate, Ba3(PO4)2, in pure water is 8.9 x 10-9 M at 25°C. What is…

A: We need to find the Ksp expression in terms of molar solubility, then from the given molar…

Q: Calculate the solubility of calcium phosphate, Ca3(PO4)2 in units of grams per liter. Ksp(Ca3(PO4)2)…

A: The solubility product, Ksp, is the constant equilibrium for an aqueous solution that dissolves a…

Q: The solubility of aqueous PbCr2O7 at 25 oC is 1.55 x 10–2 g/L at 25.0 oC. Calculate the Ksp of…

Q: The molar solubility of the metal hydroxide (M(OH)2) in water is: M(OH)2 M2+ + 20H Ksp = 5.02 x 10-6…

A: Given the equation for dissociation of metal hydroxide M(OH)2⇔M2+ +2OH- and solubility product is…

Q: The molar solubility of the metal hydroxide (M(OH)2) in water is: M(OH)2 M2+ + 20H" Ksp = 5.02 x…

A: We have given that The molar solubility of the metal hydroxide M(OH)2 in water is M(OH)2 ----->…

Q: Determine the molar solubility of CuCl in a solution containing 0.050 M KCl. Ksp (CuCl) = 1.0 ×…

Q: What mass (in grams) of Ba(103)2 (487 g/mol) can be dissolved in 500 mL of water at 25°C when The…

A: Below attached file showing the details answer. All the best. (As per the question asked the correct…

Q: Calcium Fluoride, CaF2 (aka, Fluorite), in a solution containing 19 mg/L of LiF (aka, Griceite),…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Lanthanum (III) sulfate (La2(SO4)3) is a sparingly soluble ionic compound with a Ksp = 2.3.…

Q: What is the molar solubility of a saturated solution of magnesium hydroxide, Mg(OH)2, in water? The…

Q: What is the molar solubility of MgF₂ in a 0.40 M Mg(NO3)2 solution? For MgF2, Ksp = 8.4 X 10-8. 4.6…

Q: What is the molar solubility (in M) of a salt with the formula M2X knowing that its Ksp is 1.20 x…

A: M2X dissociates as: M2X ⇌ 2M+ + X2- Let the solubility of the salt be 's' M2X ⇌ 2M+ + X2-…

Q: The Ksp of manganese(II) hydroxide, Mn(OH)2, is 2.00 × 10-13. Calculate the solubility of this…

A: The question is based on the concept of solubility product Principle. it states that a weak…

Q: The molar solubility of palladium (II) thiocyanate at 25°C is 2.22 x 10-8 M. What is its Ksp value?…

A: molar solubility=S=2.22×10-8M KSP=?

Q: What is the molar solubility of MgF2 in 0.36 M NaF? For MgF2, Ksp = 8.4 x 10–8. 7.1 x 10–4 1.0 x…

Q: The Ksp for an ionic solid, AB2, is 1.529*10-8. The molar mass of this ionic solid is 86.65 g/mol.…

A: A numerical problem based on solubility product, which is to be accomplished.

Q: For the following, please answer all the questions. Suppose the Ksp value for lead sulfide (PbS) is…

A: Let S be the solubility of PbS in water.It is a AB2 type of salt. Hence the formula of solubility…

Q: Calculate the molar solubility of X(OH)3 within water. Ksp X(OH)3 = 8.3 x 10–34 2.6 x 10–9 M…

Q: What is the molar solubility of a saturated solution of magnesium hydroxide, Mg(OH)2, in water? The…

A: Solubility product constant Ksp is an equilibrium constant that is defined as the product of the…

Q: The Ksp for an ionic solid, AB2, is 1.343*10-7. The molar mass of this ionic solid is 98.19 g/mol.…

Q: Calculate the maximum solubility of zinc(II) carbonate (Ksp = 1.46 x10-10) in a solution of 0.1M…

A: Ksp of ZnCO3= 1.46×10-10 concentration of Na2CO3= 0.1M Molar mass of ZnCO3= 125.4g/mol We need to…

Q: The Ksp for an ionic solid, AB2, is 4.602*10-8. The molar mass of this ionic solid is 85.51 g/mol.…

Q: The solubility-product constants, Ksp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and…

A: Given : Concentration of Fe+2 = 1.02 x 10-2 M Concentration of Cd+2 = 1.48 x 10-2 M

Q: The K, of manganese(II) hydroxide, Mn(OH)2, is 2.00 × 10-13 . Calculate the solubility of this…

A: The solubility product is a kind of equilibrium constant and its value depends on temperature. Ksp…

Q: Predict what will happen when you add 280 mg of BaF2 (175.3 g/mol) to 500 mL of water (Ksp of BaF2…

A: The question is based on the concept of solubility product Principle. it states that a weak…

Q: ne solubility

Q: The solubility of tin(ll) sulfide is 2x10^-14 mol/L. Calculate the Ksp of tin (ll) sulfide.

A: Tin(II) sulfide is a sparingly soluble salt and it dissolves in very low quantity in the aquoeous…

Q: Determine the molar solubility for barium fluoride (BaF2). Ksp = 1.8 x 10-7

Q: Determine the molar solubility of CaSO4 in a solution containing 0.100 mol L-1 Na2SO4. Ksp (CaSO4) =…

A: Solubility of the solution is the maximum amount of solute that can be dissolved in a particular…

Q: The solubility-product constants, Kp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and…

A: Step 1: FeCO3FeCO3 → Fe2+ + CO32-Ksp = [Fe2+][CO32-]2.10 x 10-11 = [1.03 x 10-2][CO32-][CO32-] =…

Q: does this solution look like, and what mass of silver chloride is in solution?

A: We have to tell which option is correct

Q: What is the solubility of Ag2CO3 (s) in moles per liter (mol/L) in pure water? O 2.0 x 10-4 O 1.3 x…

Q: Which of the following compounds will have the highest molar solubility in pure water? O MgCO3, Ksp…

Q: What is the molar solubility of a saturated solution of magnesium hydroxide, Mg(OH)2, in water? The…

Q: What is the solubility (in g/L) of aluminum hydroxide (molar mass Al(OH)3= 78 g/mol) at 25°C? The…

Q: e solubility of an ionic compound MX (molar mass = 436 is 6.43 x 103 g/L. What is the Ksp ?

A: Given, molar mass of ionic compound MX = 436 g.mol-1 Solubility of the compound = 6.43 ×10-3 g/L

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…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

The molar solubility in mol/L of Mg(OH)₂ (Ksp=1.8x10^-11) is

	4.2x10^-⁶M
	1.8x10^-11M
	2.6x10^-4M
	1.7x10^-4M

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

Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s /Csp of 1.1 X 10-,<) gives it such low solubility' that it can be safely consumed. What is the molar solubility' of BaSO4. What is its solubility' in grams per 100 g of water?
12.106 The solubility of KCl is 34.7 g per 100 g of water at 20 °C. Calculate its molar solubility in (a) pure water and (b) 0.10 M NaCl.
A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is not appropriate to neglect the changes in the initial concentrations of the common ions. (a) TICl(s) in 0.025 M TlNO3. (b) BaF2(s) in 0.0313 M KF. (c) MgC2O4 in 2.250 L of a solution containing 8.156 g of Mg(NO3)2. (d) Ca(OH)2(s) in an unbuffered solution initially with a pH of 12.700
Calculate the solubility (in grams per liter) of silver chloride in the following. (a) pure water (b) 0.025 M BaCl2 (c) 0.17 M AgNO3
Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving. c. The temperature changes.
Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) AgCl(s) in 0.025 M NaCl. (b) CaF2(s) in 0.00133 M KF. (c) Ag2SO4(s) in 0.500 L of a solution containing 19.50 g of K2SO4. (d) Zn(OH)2(s) in a solution buffered at a pH of 11.45
A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte is said to be a system in equilibrium. Explain. Why is such a system called a heterogeneous equilibrium?
The molar solubility of the metal hydroxide (M(OH)2) in water is: M(OH)2 = M2+ + 2ОН Ksp = 5.02 x 10-6 3.60 x 10-2 M 1.10 x 10-2 M 3.30 x 10-6 M 1.00x 10-5 м 4.31 x 10-6 M
The Ksp for an ionic solid, AB2, is 1.343*10-7. The molar mass of this ionic solid is 98.19 g/mol. Calculate the solubility of this ionic solid in grams per Liter.