Answered: The Solubility Product Constant for…

The Solubility Product Constant for silver hydroxide is 2.0 × 10-8. The molar solubility of silver hydroxide in a 0.193 M silver acetate solution is M.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 15CR

See similar textbooks

Related questions

Q: Silver chloride is often used as a test for silver ion in qualitative analysis. Using the solubility…

A: molar solubilty is defined as no. Of moles of solute dissolved in per liter of solution before the…

Q: The Solubility Product Constant for cobalt(II) carbonate is 8.0 × 10-13 Solid ammonium carbonate is…

Q: What is the solubility products constant (Ksp) of Ag2SO4 that has a molar solubility of 0.350M?

A: We have to find the Ksp of the given Ag2SO4

Q: Refer to the chemical reaction below: PBC12 (s) E Pb2+ +2CI- Calculate the solubility product…

Q: Solid manganese(II) sulfide and solid zinc sulfide are in equilibrium with a solution containing…

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

A: The given data: Ksp of Mg(OH)2 is 1.2 x 10-11 The the molar solubility of a saturated solution of…

Q: What is the solubility (g L-1) of lead(II) Iodide in otherwise pure water, given that the solubility…

Q: 10) Molar solubility of calcium fluoride Find the molar solubility of calcium fluoride in a solution…

A: To find the molar solubility of calcium fluoride in a solution containing 0.70 M Ca(NO3)2 (aq).

Q: Write the expression for the solubility-product constant of the ionic compound: SrSO4

A: Generally solubility product calculated only for spraingly solubility salt not for strong…

Q: onditions the Reaction Quotient, Q, is equal to 1.576x10^-12

A: Concentration in mixture = = M1V1/V1+V2 NaI + Pb(CH3COO) ---> CH3COONa + PbI2 So, PbI2 --->…

Q: Solid copper(Il) acetate is slowly added to 50.0 mL of a 0.0631 M ammonium sulfide solution. The…

A: The Ksp expression for this reaction is:Ksp = [Cu^2+] [S^2-]We know that Ksp for CuS is 7.9 ×…

Q: Which of the following compounds will have the highest molar solubility in pure water? O Fe(OH)3,…

Q: The Solubility Product Constant for lead chromate is 1.8 × 10-¹4. If lead chromate is dissolved in…

A: The solubility product constant (Ksp) demonstrates the equilibrium between a solid and its…

Q: Can AgCl precipitate if you add 5.0 mL of 0.025 mol L-1 HCl solution to 100.0 mL of 0.0010 mol L-1…

Q: 4.) Calculate the solubility product constant, Ksp, for lead(II) chromate. Ksp = x 10:13 Hint: enter…

A: Given that: Molar solubility of lead chromate(S) = 5.7×10-7 M Lead chromate = PbCrO4

Q: Write the expression for the solubility-product constant of the ionic compound: Fe(OH)2

A: Given: Ionic compound, Fe(OH)2 The equation for dissociation of given compound is as follows,…

Q: 3. The solubility product constant (Ksp) of iron (III) chloride is 1.7 x 10-6. Calculate the molar…

A: Solubility product of iron (III) chloride = The solubility product ( Ksp ) of a sparingly soluble…

Q: The solubility product for silver chloride is 1.6 x 10−10. What is the molar solubility of silver…

A: This question can be solved using concepts of solubility. Solubility product of a sparingly salt…

Q: The Solubility Product Constant for iron(III) hydroxide is 6.3 × 10-38. Solid sodium hydroxide is…

A: Step 1: Step 2: Step 3: Step 4:

Q: The Solubility Product Constant for cobalt(II) carbonate is 8.0 x 10-¹3. The molar solubility of…

A: the question is based on solubility equilibria

Q: aturated Br- concentration in aq lead bromide is 2.37×10^-2. The soluability product constant for…

Q: It is experimentally determined that 1.33 x 103 g of silver bromide will dissolve in 100.0 mL of…

A: Solubility Product(Ksp) = It is an equilibrium constant which shows the relation between ions and…

Q: The Solubility Product Constant for magnesium fluoride is 6.4 × 10-9 Solid ammonium fluoride is…

A: Given:- Ksp for MgF2 = 6.4 × 10^-9- Initial concentration of magnesium nitrate [Mg(NO3)2] = 0.0304…

Q: The solubility of Ca3(PO4)2 is 0.3 g/100 mL. Calculate its solubility product constant.

A: Given information is as follows: Solubility = 0.3 g/100 mL Mass of Ca3PO42 = 0.3 g Volume = 100 mL =…

Q: What is the molar solubility of silver chloride in water? The solubility-product constant 1.8x10-10…

Q: What is the solubility product expression for Ca5(PO4)3(Cl)?

A: For the given expression Initially we are drafting dissociation equation and from that Ksp is found…

Q: What is the solubility product expression for Al(OH)3?

Q: molar

Q: When 25.0 mL of a 8.63×10-4 M cobalt(II) acetate solution is combined with 22.0 mL of a 1.70×10-5 M…

Q: Solid copper (II) acetate is slowly added to 50.0 mL of a 0.0631 M ammonium sulfide solution. The…

A: To solve these problems, we can use the solubility product constant (Ksp) and the formula for the…

Q: A student measures the molar solubility of magnesium fluoride in a water solution to be 1.19×10-3 M.…

A: Given that : Molar solubility of magnesium fluoride(MgF2) = 1.19×10-3M MgF2 will dissociate as :…

Q: A student measures the molar solubility of chromium(III) hydroxide in a water solution to be…

A: Given : s = 1.28 x 10-8 M Cr(OH)3(s) ⇌Cr+3(aq) + 3OH-(aq) s…

Q: What is the molar solubility of the ionic compound barium carbonate, BaCO3? The solubility product…

Q: Sodium phosphate is added to a solution that contains 0.0069 M aluminum nitrate and 0.017 M calcium…

A: Solubility product: It is defined as the product of its dissolved ion concentrations raised to the…

Q: The solubility of lead(II) iodide is 1.39 x 10-3 mol/L at a certain temperature. What is the…

Q: The Solubility Product Constant for barium phosphate is 1.3 × 10-29⁹. Solid potassium phosphate is…

A: Solid potassium phosphate is slowly added to 50.0 mL of 0.0350 M barium acetate solution . The…

Q: A student measures the F- concentration in a saturated aqueous solution of barium fluoride to be…

Q: The K of iron(II) hydroxide, Fe(OH)2, is 4.87 x 10-17. Calculate the molar solubility, s, of this…

Q: Calculate the molar solubility of calcium phosphate Ca3(PO4)2 Ksp=2.0×10−29 when dissolved in a…

Q: The Solubility Product Constant for zinc phosphate is 9.1 × 10¯ The molar solubility of zinc…

Q: The Solubility Product Constant for lead phosphate is 3.0 × 10-4. The molar solubility of lead…

A: Solubility product constant for lead phosphate = 3.0 × 10-44.Molar solubility of ammonium phosphate…

Q: The Solubility Product Constant for calcium sulfide is 8.0 × 10-6. The molar solubility of calcium…

A: So, let's assume that solubility of CaS in absence of K2S is: S. So, solubility product, Ksp =…

Q: The Solubility Product Constant for silver iodide is 1.5 × 10-16. The molar solubility of silver…

Q: .Assume the solubility product of Mg(OH)2 is 1.3 x 10 at a certain temperature. What minimum OH…

A: Given: The solubility product of Mg(OH)2 = 1.3 × 10-11 We have to calculate the minimum…

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

**Using References to Determine Solubility**

To solve the problem of finding the molar solubility of silver hydroxide in a 0.193 M silver acetate solution, it is necessary to use the Solubility Product Constant (Ksp).

**Given:**
- **Solubility Product Constant (Ksp) for silver hydroxide, AgOH**: \(2.0 \times 10^{-8}\)

**Problem:**
Calculate the molar solubility of silver hydroxide in a 0.193 M silver acetate solution.

**Explanation:**
Silver hydroxide (AgOH) will dissolve in the silver acetate solution up to the point where the product of the concentrations of the ions equals the \( K_{sp} \). Typically, understanding how common ion effect reduces solubility in such a solution is key.

Fill in the value of the calculated molar solubility in the given space.

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 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

. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?
. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
Even though barium is toxic, a suspension of barium sulphate is administered to patients who need x rays of the gastrointestinal tract. The barium milkshake is safe to drink because the solubility of barium sulfate is so low. Calculate the solubility of barium sulfate in grams per liter using the data in Table 14.4.
Use the solubility product constant from Appendix F to determine whether a precipitate will form if 10.0 mL of 1.0 106 M iron(II) chloride is added to 20.0 mL of 3.0 104 M barium hydroxide.
. K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.
5.4. Supersaturated solutions can be made in which more solute is dissolved in solution than would normally dissolve. These solutions are inherently unstable, however. A seed crystal of calcium acetate, , precipitates the excess solute from a supersaturated solution of calcium acetate. When the excess solute has finished precipitating, a chemical equilibrium is established. Write the chemical equations for that equilibrium, and write the net chemical reaction that occurs overall.
Hard water has a high concentration of calcium and magnesium ions. Focusing on the calcium ion, a common home water -softening process is based on a reversible chemical change that can be expressed by Na2Ze(s)+Ca2+(aq)CaZe(s)+2Na+(aq). Na2Ze represents a solid resin that is like an ionic compound between sodium ions and zeolite ions, a complex arrangement of silicate and aluminate groups; CaZe is the corresponding calcium compound. When, during the day, is this system most likely to reach equilibrium? Why doesnt it reach equilibrium and stay there? Periodically it is necessary to recharge the water softner by running salt water, NaCl(aq), through it. Why is this necessary? What concept is discussed in this chapter does the recharging process illustrate? Zeolite ions are used in home water softners because they have a porous but rigid structure that is weakly attracted to cations, readily allowing an exchange among different ions.
. What is meant by the solubility product for a sparingly soluble salt? Choose a sparingly soluble salt and show how the salt ionizes when dissolved in water, and write the expression for its solubility product.
In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. (a) Describe what happens in the first few minutes after the partition is opened. (b) What would you expect to see several hours later? (c) How is this system analogous to dynamic chemical equilibrium?
The solubility product constant for calcium oxalate is estimated to be 4 109. What is its solubility in grams per liter?
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.
The following is a thought experiment. Imagine that you put a little water in a test tube and add some NaF crystals. Immediately after you add NaF, you observe that the crystals begin dissolving. The quantity of solid NaF decreases, hut before long, it appears that no more NaF is dissolving. The solution is saturated. The equation for the dissolution of NaF in water is NaF(s) —* Na (aq) + F~(aq). As NaF dissolves, what do you think happens to the rate of dissolution? Describe w hat is occurring on the molecular level. Assume that the reverse reaction, Na+(aq) + F“(aq) —* NaF(s), also occurs as the crystal dissolves. In other words, both dissolution and precipitation are taking place. When it appears that there is no more change in the quantin’ of NaF dissolving (the solution is saturated), w hat has happened to the rates of the forward and reverse reactions? Explain your answer.