Which of the following reactions does not have a Solubility Product (Ksp)? AgCl(s)←→Ag+(aq) + Cl-(aq) MgCO3(s)←→MgO(s) + CO2(g) PbCl2(s)←→Pb2+(aq) + 2Cl-(aq) BaSO4(s)←→Ba2+(aq) + SO42-(aq) Would it be AgCl since it is a very insoluble compound? It appears that they all do have a ksp.

Which of the following reactions does not have a Solubility Product (Ksp)? AgCl(s)←→Ag+(aq) + Cl-(aq) MgCO3(s)←→MgO(s) + CO2(g) PbCl2(s)←→Pb2+(aq) + 2Cl-(aq) BaSO4(s)←→Ba2+(aq) + SO42-(aq) Would it be AgCl since it is a very insoluble compound? It appears that they all do have a ksp.

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter17: Solubility And Complex-ion Equilibria

Section: Chapter Questions

Problem 17.112QP

See similar textbooks

Related questions

Q: Which of the following substances is more soluble in a hydrochloric acid solution than in a sodium…

A: The compound which is more soluble in acidic solution means, it likely to be basic in nature.In the…

Q: NH+4 and NH3 are and acid=base conjugate pair. How many moles of NH4Cl must be added to 2.0 L of a…

A: Moles of NH3 =Molarity × Volume = 0.1 M × 2 L = 0.2 moles Kb = 1.8 × 10-5,…

Q: Consider H2Se03(aq) --> H+(aq) + HSEO3-(aq) where [H+] = [HSE03-] = 0.200 M. The K %3D = 0.907 at…

A: We are given [H+] = [HSeO3-] = 0.2M K = 0.907 We have to find the molarity of H2SeO3

Q: One student, when experiencing a headache, decided to ingest a solution of acetylsalicylic acid…

A: Given , Concentration of acetylsalicylic, [C9H8O4] = 0.1mol/L Ka = 5.6 x 10-4

Q: A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H,O(1) =…

A: The equilibrium constant Ka expresses the relation between products and reactants of a reaction at…

Q: A 1.034-g sample of impure oxalic acid is dissolved in water and an acid-base indicator added. The…

A: Given: Mass of sample = 1.034 g Volume of NaOH = 34.47 mL Molarity of NaOH = 0.485 M

Q: 1) The equation below represents the equilibrium process of a saturated solution of Ca(OH)2 If the…

A: "Le Chatelier's principle" is mainly utilized for the prediction of effect of some various changes…

Q: A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L…

A: Given: Volume of lactic acid solution = 35.0 mL Volume of NaOH solution required to reach…

Q: Phosphoric acid is a triprotic acid (Kal To find the pH of a buffer composed of H₂PO¯ (aq) and…

A: The Ka values for the phosphoric acid areThe phosphoric acid has the following ionizations H3PO4 ⇌…

Q: Write the equilibrium expression for the reaction Zn2+(aq) + 2 NH3(aq) Zn(NH3)2+(aq)

A: The given reaction will be: Zn2+(aq) + 2 NH3(aq) <--> Zn(NH3)2+(aq)

Q: An organic acid(HA) has a molecular weight of 100. g mol^-1, a Kow=5.6 and a Ka=2.7x10^-2. If…

Q: . The ionization of phosphoric acid, H3PO4(aq), involves multiple reactions. The ionization…

Q: Fill in the left side of this equilibrium constant equation for the reaction of benzoic acid…

A: The Equilibrium constant for a reaction A + B ⇔ C + D Can be written as K = [C][D][A][B],…

Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4 and 5.4 × 10^–10,…

Q: 6. What are the equilibrium concentrations of a 0.80 M HCN solution for each species (in M to two…

A: we have to calculate the equilibrium concentration of all species for the HCN solution

Q: NiCO3 (s) ---> Ni^2+(aq) + CO3^2-(aq) K1 = 6.6 x 10^-9 HCO3^-(aq) + H2O(ℓ) CO3^2-(aq)…

Q: A buffer solution is prepared in such a way that the concentration of propanoic acid is 8.0 ×…

A: Given, Ka = 1.34 ×10−5 C2H5COOH(aq) + H2O(l) ⇌ H3O+(aq) + C2H5COO−(aq) propanoic acid…

Q: A solution may contain any or all of the following cations: Ag+, Pb2+, Ba2+, Ni2+ in an UNKNOWN…

A: Identification of cations

Q: Calculate the volume of 4.0 M KOH necessary to dissolve 1.0 g of Al metal according to Al(s) + 2…

A: Given, 4.0 M KOH 1.0 g of Al metal Molar mass of Al metal is 26.981539 g/mol Mole of 1.0 g of Al…

Q: A buffer solution is prepared in such a way that the concentration of propanoic acid is 8.5 × 10−1 M…

A: pH of buffer solution is calculated by using Henderson-Hasselbalch equation. pH = pKa +…

Q: Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10,…

A: a) Given: Volume of HF=50 mL Concentration of HF= 0.2 M Concentration of NaH2BO3= 0.5 M Volume of…

Q: Use Lewis structures to show how electron pairs move and bonds form and break in this reaction, and…

A: SO3 and H2O lewis structure is given SO3 will behave as an electrophile due to the presence of…

Q: At 25 °C, only 0.0210 mol of the generic salt AB is soluble in 1.00 L of water. What is the ?spof…

Q: Use the References to access important values if needed for this question. A student determines that…

Q: Bromothymol blue is yellow in acid solutions. HBB is acidic form of the indicator . The indicator…

A: If we go on adding Sodium Hydroxide solution the Hydroxide Ion concentration will increase. this is…

Q: B represents an acid-base indicator and behaves like a base. Its dissociation equilibrium in an…

Q: The solubility equilibrium of iron(II) hydroxide is expressed as: Fe(OH)2 (s) ⇌ Fe2+(aq) + 2OH−(aq)…

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the A of a weak acid she isolated called…

A: Answer: When a weak acid will be added in water, its partial ionization will take place, due to that…

Q: Doc Jill wants to determine the Ao of a weak acid she isolated called Xcitingpartic acid (HXp). She…

A: Hii there, As there are multiple sub parts posted. we are answering first-three sub parts . If you…

Q: Given the equilibrium equation for the ionization of silver chloride below. What would happen to…

A: The equilibrium equation for ionisation of AgCl given is AgCl (s) ⇌ Ag+ (aq) + Cl- (aq) The…

Q: An aqueous solution of Ag(CN)2− is made by combining 0.0100 moles AgNO3 with 1.00 mole NaCN and…

A: The constant used for the formation of complex is known as formation constant (Kf)

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

Which of the following reactions does not have a Solubility Product (Ksp)?

	AgCl(s)←→Ag⁺(aq) + Cl^-(aq)
	MgCO₃(s)←→MgO(s) + CO₂(g)
	PbCl₂(s)←→Pb²⁺(aq) + 2Cl^-(aq)
	BaSO₄(s)←→Ba²⁺(aq) + SO₄^2-(aq)

Would it be AgCl since it is a very insoluble compound? It appears that they all do have a ksp.

Any help is appreciated. Thank you so much!!

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

Cite microscopic evidence to support that no chemical change took place in silver solid in aqueous hydrochloric acid.
B represents an acid-base indicator and behaves like a base. Its dissociation equilibrium in an aqueous solution can be written as: B(ac) + H2O(l) <-> +BH(ac) + OH(ac) If B (ac) is yellow +BH is red. Using Le Châtelier's principle, predict the color of the indicator by adding a few drops of the indicator to an aqueous solution of HCl and an aqueous solution of NaOH. Write the corresponding chemical reactions.
One student, when experiencing a headache, decided to ingest a solution of acetylsalicylic acid (ASA). So he prepared a 0,1 mol/L solution. Knowing that acetylsalicylic acid is monoprotic and that it has a Ka equal to 5,6x10^-4, we can say that the molar concentration of H+ in the solution will be approximately equal to: 0,0075 mol/L 0,0057 mol/L 0,0032 mol/L 0,0010 mol/L 0,0179 mol/L
1) The equation below represents the equilibrium process of a saturated solution of Ca(OH)2 If the following changes are made to a saturated solution, what will be the effect on the [Ca2+]? Ca(OH)2 (s) <--> Ca2+(aq) + 2 OH- (aq) ΔH = -16.6 kJ A strong base is added to the solution (Decrease, Increase, No change) More solid Ca(OH)2 is added to the container (Decrease, Increase, No change) The solution is raised to a higher temperature (Decrease, Increase, No change) A strong acid is added to the solution (Decrease, Increase, No change) Ca(NO3)2 (s) is added. Ca(NO3)2 is very soluble (Decrease, Increase, No change)
A buffer solution is prepared in such a way that the concentration of propanoic acid is 8.0 × 10−1 M and the concentration of sodium propanoate is 8.4 ×10−1 M. The buffer equilibrium is described by C2H5COOH(aq) + H2O(l) ⇌ H3O+(aq) + C2H5COO−(aq) propanoic acid proponate ion with Ka = 1.34 ×10−5 . If the concentration of the sodium propanoate were doubled while the acid concentration remained the same, calculate the pH of the resulting solution.
Use the References to access important values if needed for this question. A student determines that an aqueous solution that contains 0.176 M sodium fluoride and 0.499 M hydrofluoric acid, also has an H3O+ concentration of 2.94x10-3 M. Based on these data, calculate the value of the equilibrium constant K for the equilibrium: HF(aq) + H₂O2H30+ (aq) + F(aq) Calculate K as is usually done, omitting the solvent, water, from the expression for K: K = Submit Answer Retry Entire Group 2 more group attempts remaining Previous Email Instructor Ne
A buffer solution is prepared in such a way that the concentration of propanoic acid is 8.5 × 10−1 M and the concentration of sodium propanoate is 2.0 × 10−1 M. The buffer equilibrium is described by C2H5COOH(aq) + H2O(l) ⇌ H3O+(aq) + C2H5COO−(aq) propanoic acid propanoate ion with Ka = 1.34 × 10−5. If the concentration of the sodium propanoate were doubled while the acid concentration remained the same, calculate the pH of the resulting solution. pH=________
The solubility equilibrium of iron(II) hydroxide is expressed as: Fe(OH)2 (s) ⇌ Fe2+(aq) + 2OH−(aq) (A) Calculate the molar solubility of iron(II) hydroxide, Fe(OH)2, given that its Ksp is 12.0×10-16. (B) Calculate the molar solubility of Fe(OH)2 in a 0.40 M solution of NaOH(aq). show all of your work including the ICE Tables .
Please explain why this is wrong, thank you for explaining
Calculate the volume of 4.0 M KOH necessary to dissolve 1.0 g of Al metal according to Al(s) + 2 KOH(aq) + 6 H2O -> 2 K+ + 2 Al(OH)4- + 3 H2(g)
Given the equilibrium equation for the ionization of silver chloride below. What would happen to the amount of solid silver chloride if sodium chloride (NaCl) is added to the solution? Explain. AgCl (s) ⇌ Ag+1 (aq) + Cl -1 (aq)
The solubility (denoted as s) of CaSO4 in pure water at 40o C is 1.09 grams per liter. What is the value of the solubility product of CaSO4?

SEE MORE QUESTIONS

Recommended textbooks for you

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning