### Precipitation of Slightly Soluble Ionic SaltsWhen we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will precipitate if $ Q_{sp} $ ____ $ K_{sp} $, and will continue to precipitate until $ Q_{sp} $ ____ $ K_{sp} $.#### Multiple Choice Options:1. $\circ$ is greater than; equals2. $\circ$ is less than; equals3. $\circ$ is less than; is greater than4. $\circ$ equals; is less than5. $\circ$ equals; is greater than#### Explanation:- $ Q_{sp} $ (the ion product) and $ K_{sp} $ (the solubility product constant) are key concepts in determining whether a precipitate will form in a solution.- **Step 1:** If $ Q_{sp} $ (the actual product of ion concentrations in the solution) is greater than $ K_{sp} $ (the maximum product of ion concentrations that can exist together in a solution without forming a precipitate), then the salt will precipitate because the solution is supersaturated.- **Step 2:** Precipitation will continue until $ Q_{sp} $ equals $ K_{sp} $, at which point the solution is saturated, and no more precipitate will form.In summary, when ions of a slightly soluble salt are mixed and $ Q_{sp} $ exceeds $ K_{sp} $, precipitation will occur until $ Q_{sp} $ decreases to equal $ K_{sp} $.

Solution is made up of two components: solute and solvent. The component which is present in major…

When we mix together, from separate sources, the ions of a slightly soluble ionic salt, Ksp, and will continue to precipitate until the salt will precipitate if Qsp Qsp _Ksp. O is greater than; equals is less than; equals is less than; is greater than O equals; is less than equals; is greater than

When we mix together, from separate sources, the ions of a slightly soluble ionic salt, Ksp, and will continue to precipitate until the salt will precipitate if Qsp Qsp _Ksp. O is greater than; equals is less than; equals is less than; is greater than O equals; is less than equals; is greater than

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: 3. Determine the solubility of the given ionic compounds and rewrite the formula with the…

Q: When 12.0 mL of a 5.17×10-4 M manganese(II) acetate solution is combined with 25.0 mL of a 7.96x10-4…

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

Q: the solubility of CuI is 3.2x10^-4 molar. what is the solubility product constant, lap, for CuI

Q: For each of the following compounds, decide whether the compound's solubility in aqueous solution…

A: Here we have to predict the solubility of insoluble salt in acidic and basic medium. If anion of…

Q: What must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO4,…

A: Solubility Product : For a sparingly soluble salt the product of solubility (concentration) of all…

Q: Calculate the mas of AgCl need to contain 7.5g Ag

A: Given, Mass of Ag = 7.5g. The reaction of Ag to give AgCl is

Q: Consider these compounds: A Baso, B. PbF2 C. CuCO, D. PbCl, Complete the following statements by…

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

Q: the value of Ksp for Cu(1O,),.

Q: Fill in the blank for the following question: • If Q > Ksp, precipitate _________________________…

A: Ksp is the product of molar concentrations of the constituent ions of the solid ionic compound where…

Q: At a certain temperature, the solubility of strontium arsenate, Sr, (AsO,),, is 0.0570 g/L. What is…

A: Given: The solubility of strontium arsenate, Sr3(AsO4)2 = 0.0570 g/L We have to calculate the Ksp of…

Q: Suppose that equal volumes of 0.114 M sodium chloride (NaC) and 0.0888 M silver nitrate (AgNO) are…

A: Given: Molarity of sodium chloride = 0.114 M Molarity of silver nitrate = 0.0888 M Solubility…

Q: Note that each of the stock solutions is 0.002 M before mixing. What are the initial concentrations…

Q: 1.3 g of potassium iodide is placed in a 100 mL of 0.11 mol/L lead (II) nitrate solution. (a) Write…

A: The objective of the question is to determine whether a precipitate of lead iodide will form when…

Q: The equilibrium concentration of carbonate ion in a saturated lead carbonate solution is ____M.…

A: The solubility product constant expression for PbCO3 PbCO3 (s) <=> Pb2+ (aq) + CO3- (aq)

Q: 0 Question 12 You combine 100. mL of 0.100 M Fe(NO3)2 and 100. mL of 0.125 M Na₂CO3. Does a…

A: Formation of Precipitate using the solubility product and reaction quotient.

Q: The molar solubility of silver sulfate in a 0.145 M ammonium sulfate solution is М.

A: It is a type of multiple question so I have solved first one for you. If you want to be solved…

Q: The solubility product constant for MX2 is 7.48E-3. What is the molar solubility of MX2? (the answer…

Q: A. Saturated NaCl Solution: Results of adding conc. HCl Chemical Equation for equilibrium system…

A: NOTE- As the question contains the multiple sub parts, we will solve the first sub part for you. To…

Q: Solid calcium sulfate and solid calcium chromate are in equilibrium with a solution containing…

A: Sodium chromate is soluble in water and it ionizes completely in water. The solubility product of…

Q: M sodium hydroxide solution is |(yes or no) m?

A: Reaction is NaOH + ZnCl2 ---> Zn(OH)2 + 2NaCl So , Ionic product for Zn(OH)2 Q = [Zn2+][OH-]2…

Q: Determine if a precipitate forms when 800.0 mL of 2.00 x 10* M Ba(NO,), is added to 200.0 mL of 5.00…

Q: When 25.0 mL of a 9.60×10-5 M potassium phosphate solution is combined with 25.0 mL of a 4.70×10-4 M…

A: Given that 25.0 mL of a 9.60×10-5 M potassium phosphate solution is combined with 25.0 mL of a…

Q: When 15.0 mL of a 7.21×104 M copper(II) chloride solution is combined with 12.0 mL of a 3.67×104 M…

Q: Calculate the solubility-product constant for each of the following substances, given that the molar…

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

Q: The concentrations of lead and carbonate ions in a saturated aqueous solution of PbCO3PbCO3 are both…

A: Lead carbonate dissociates in solution to form lead ions and carbonate ions.

Q: If 12.0 mL of 8.30×104M Ba(CH3COO), are added to 15.0 mL of 1.10×10$ M (NH,);CO3, will solid BaCO3…

A: Given data, Molarity of Ba(CH3COO)2=8.30×10-4MVolume of Ba(CH3COO)2=12.0mL=0.0120LMolarity of…

Q: What happens when equal volumes of 2x104 M aqueous solutions of calcium nitrate, Ca(NO3)2, and…

A: Dissociation of calcium fluoride is,

Q: Zn(s)|Zn2+(aq) || Fe2+(aq, ) | Fe(s) What would you change to increase the Ecell decrease…

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

### Precipitation of Slightly Soluble Ionic Salts

When we mix together, from separate sources, the ions of a slightly soluble ionic salt, the salt will precipitate if $ Q_{sp} $ ____ $ K_{sp} $, and will continue to precipitate until $ Q_{sp} $ ____ $ K_{sp} $.

#### Multiple Choice Options:
1. $\circ$ is greater than; equals
2. $\circ$ is less than; equals
3. $\circ$ is less than; is greater than
4. $\circ$ equals; is less than
5. $\circ$ equals; is greater than

#### Explanation:
- $ Q_{sp} $ (the ion product) and $ K_{sp} $ (the solubility product constant) are key concepts in determining whether a precipitate will form in a solution.
- **Step 1:** If $ Q_{sp} $ (the actual product of ion concentrations in the solution) is greater than $ K_{sp} $ (the maximum product of ion concentrations that can exist together in a solution without forming a precipitate), then the salt will precipitate because the solution is supersaturated.
- **Step 2:** Precipitation will continue until $ Q_{sp} $ equals $ K_{sp} $, at which point the solution is saturated, and no more precipitate will form.

In summary, when ions of a slightly soluble salt are mixed and $ Q_{sp} $ exceeds $ K_{sp} $, precipitation will occur until $ Q_{sp} $ decreases to equal $ K_{sp} $.

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

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

When 22.0 mL of a 2.41×10-4M sodium iodide solution is combined with 15.0 mL of a 2.61×10-4 M lead acetate solution does a precipitate form?| |(yes or no) For these conditions the Reaction Quotient, Q, is equal to
When 15.0 mL of a 2.26×10-4M potassium iodide solution is combined with 12.0 mL of a 7.79×10M lead nitrate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to
what is the concentration of iodide ions in saturated solution of lead (II) iodide? the solubility product constant of Pb2 is 1.40x10^-8use correct units and sig figs
Nitesh
determine whethrer INCREASE, DECREASE or NO EFFECT
When 12.0 mL of a 6.60×10-4 M sodium phosphate solution is combined with 15.0 mL of a 5.56×10-4 M aluminum iodide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to
10. If 223.0 mg of AgBr is completely dissolved in 184.0 ml. of 0.14 M NH3, what is the equilibrium concentration of Ag (aq) in the final solution? KAg(NH3)2] = 1.7E7 Include at least 3 significant figures in your arawer M Grade This Exercise
Solve it asap...
Molar solubility of Barium phosphate is related to its solubility product by equation: s = Ko/108 S = S = \K? /27 K 13 S =
Calculate the value of Q and determine if a precipitate of CaCO, will form when 65.0 mL of 0.035 M CaCl, is added to 45.0 mL of 0.095 M Na,CO,? Ksp CaCO, = 8.7 x 109.
When 18.0 mL of a 2.79x104 M potassium phosphate solution is combined with 18.0 mL of a 7.38×10-4 M barium bromide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to
Which of the following statements is/are TRUE regarding solubility equilibria? I. It is an equilibrium that exists between an undissolved solids and its supersaturated solution. II. The rate of dissolution is equal to the rate of precipitation. III. The concentration of the ions is always equal to the solubility of the salt. Which of the following statements is/are TRUE regarding solubility equilibria? I. It is an equilibrium that exists between an undissolved solids and its supersaturated solution. II. The rate of dissolution is equal to the rate of precipitation. III. The concentration of the ions is always equal to the solubility of the salt. II and III I only I and II II only