What is the solubility of AgCN(s) (Ksp = 2.2 x 10-16) in a solution containing 0.19 M H? (Ka for HCN is 6.2 × 10-¹0.) X

Q: Calculate the molar solubility of Ag2 CrO4 in a solution that is 0.01 M in AgNO3.

A: We need to calculate the molar solubility of Ag2CrO4

Q: Calculate the molar solubility of Ag2CrO4 in a solution that is 0.01 M in AgNO3. Ksp of Ag2 CrO4 =…

A: Molar solubility is defined as the number of moles of compound is dissolved in one litre of…

Q: To an aqueous solution originally containing 1.0 x 10^-4 mol/L Ag+ was added enough of the weak acid…

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Q: What is the pH of a buffer that is 0.307 M HF and 0.417 M LiF? The Ka for HF is 3.5 x 10-4.

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Q: What is the solubility of PbF₂ in a solution that contains 0.0700 M Pb²⁺ ions? (Ksp of PbF₂ is 3.60…

A: The objective of this question is to find the solubility of PbF2 in a solution that already contains…

Q: What is the molar solubility of a hypothetical compound AB in pure water given a Ksp = 6.1 x 10-2?…

A: Let the molar solubility is s M.  AB(s) = A^+(aq) + B^-(aq)    s             s                s…

Q: What is the molar solubility of Ca(OH)2Ca(OH)2? Ksp=8.0x10−6

A: Note: As per our guidelines, we are supposed to answer only one question when multiple questions are…

Q: What is the molar solubility of BaSO4 (molar mass=233.4g/mol, Ksp=1.1*10^-10) in a 0.050 M solution…

A: Given : Concentration of BaCl2 = 0.050 M And Ksp of BaSO4 = 1.1 X 10-10

Q: The solubility of Ni(OH)2 in a pH = 10.64 solution is___. Ksp Ni(OH)2 = 1.6 × 10-16

A: Hence Solubility is 8.4×10-10 MExplanation:

Q: What is the solubility of PbF₂ in a solution that contains 0.0500 M Pb²⁺ ions? (Ksp of PbF₂ is 3.60…

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Q: What is the molar solubility of a hypothetical compound AB in pure water given a Ksp = 6.2 x 10-2?…

A: Given the molar solubility of a hypothetical compound AB in pure water given a Ksp = 6.2 x 10-2…

Q: What is the molar solubility of a hypothetical compound AB in pure water given a Ksp = 5.3 x 10-2?…

A:

Q: Calculate the molar solubility of BaCrO4. Ksp of BaCrO4 = 1.2 x 10-10

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Q: What is the pH of a buffer that is 0.307 M HF and 0.417 M LiF? The Ka for HF is 3.5 x 10-4.

A:

Q: What is the solubility of magnesium hydroxide in a solution buffered at pH 9.25?…

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Q: Calculate the molar solubility of Ag2 CrO4 in a solution that is 0.01 M in AgNO3. Ksp of Ag2 CrO4 =…

A: Given,  The solubility product of Ag2CrO4 = 1.2 × 10-12  The solubility of Ag2CrO4 in 0.01 M of…

Q: What is the solubility of AgCN(s) (Ksp = 2.2 × 10⁻¹⁶) in a solution containing 0.39 M H⁺? (Ka for…

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Q: What is the solubility of magnesium hydroxide in a solution buffered at pH 8.45?…

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Q: What is the minimum mass of Mg(NO₃)₂ that must be added to 1.00 L of a 0.460 M HF solution to begin…

A: Given   The volume of solution is 1.00 L. The concentration of HF solution is 0.460 M. The Ksp for…

Q: What is the solubility of AgCN(s) (Ksp = 2.2 × 10⁻¹⁶) in a solution containing 0.55 M H⁺? (Ka for…

A: At Equilibrium       AgCN+  H+  ⇋ HCN +  Ag +

Q: Calculate the solubility of AgCN(s) (Ksp = 2.2 x 10-12) in a solution containing 0.50 M H*. (Ka for…

A: Given that, Ksp = 2.2 × 10-12  [H+] = 0.50 M Ka = 6.2 × 10-10

Q: How do the concentrations of Ag+ and CrO4 2− in a saturated solution above 1.0 g of solid Ag2CrO4…

A: When the maximum amount of solute is dissolved in the solvent is called solubility.

Q: molar solubility

A:

Q: What is the molar solubility of Pb(OH)2 in a solution that is 0.10 M NaOH? The Ksp for Pb(OH)2 is…

A: The reaction involved is:                     Pb (OH)2→Pb+2 + 2OH-Time=0        s                 0…

Q: At a certain temperature, the solubility of strontium arsenate, Sr3 (AsO4)2, is 0.0550 g/L. What is…

A: Given, solubility of strontium arsenate, Sr3(AsO4)2 = 0.0550 g/L Ksp = ? Note: molar mass of…

Q: To an aqueous solution originally containing 1.0 x 10^-4 mol/L Ag+ was added enough of the weak acid…

A: Precipitation of AgCN occurs when the product of concentrations of ions formed equals Ksp. Ksp is…

Q: What is the molar solubility of Ca(OH)2 in a 0.340 M NaOH solution? The Ksp of Ca(OH)2 is 6.5 x…

A:

Q: What would the molar solubility of Mg(OH)2 (s) be in a 3.0 M solution of NaOH? Ksp=7.1*10^-12? What…

A: The solubility product of a sparingly soluble salt is defined as the product of molar concentrations…

Q: You add 50.0 mL of 0.150 M HCl to 50.0 mL of 0.150M AgNO,. What are the final concentrations of H30…

A: The chemical reaction between HCl and AgNO3, AgCl is formed and the concentration of Cl- is only due…

Q: What is the molar solubility of lead(II) fluoride in 0.20 M NaF? The Ksp of lead(II) fluoride…

A: Here we have to determine the solubility of PbF2 in presence of 0.2M of NaF solution.  Data- Ksp…

Q: ature, the solubility of stront his salt at this temperature?

A: The solubility reaction for Sr>3(AsO4)2 is given by Sr3(AsO4)2 (s) -----> 3 Sr2+ (aq) + 2…

Q: How many moles of Mg(OH)2 can dissolve in one liter of solution with pH = 10. Ksp Mg(OH)2 = 8.9 x…

A: The expression for the solubility product is given as:Ksp = [Mg2+] [OH-]2 Given: Ksp = 8.9×10-12pH…

Q: What is the molar solubility of Sn(OH)4 if Ksp = 1.20 x 10-57

A: Given data set: Ksp of Sn(OH)4 = Ksp = 1.20 x 10^-57 We need to determine the molar solubility.

Q: What is the solubility of Mg(OH)₂ at a pH of 12.70? (Ksp Mg(OH)₂ is 1.6 × 10⁻¹³)

A: Dear student since you have posted multiple questions, As per our company QnA guidelines We are…

Q: 4.) A solution contains 7.84 x 10 8 M of copper ion (Cu2*) and has a pH of 9.118. Does copper(II)…

A: Given that:  [Cu2+] = 7.84×10-8M pH = 9.118  Ksp of Cu(OH)2 = 1.10×10-15 Using: pH + pOH = 14 pOH =…

Q: What is the molar solubility lead(II) bromide when it is added to pure water, if the Ksp (PbBr2) is…

A: Given: The Ksp of PbBr2 = 6.60 × 10-6 We have to calculate the molar solubility lead(II) bromide…

Q: An ionic compound with the generic formula "AB 2" has a K sp = 4.67 x 10 -6. What is the molar…

A: When AB2 Dissociates - AB2 <===> A2+ + 2B-   Then, Ksp solubility Product is written as - Ksp…

Q: What

A: Ksp is the solubility product which is defined for solid

Q: Consider a buffer made by adding 132.8 g of NaC, H₂O₂ to 300.0 mL of 1.41 M HC,HO2 (Ka = 6.3 x 10-5)…

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Q: What is the minimum mass of Mg(NO₃)₂ that must be added to 1.00 L of a 0.710 M HF solution to begin…

A: Given, Ka for HF= 7.2 x 10-4 Ksp for MgF2 = 7.4 × 10⁻⁹

Q: Given a 1.00 L solution containting 1.00 x 10^-2 M each of Ca2+ and Ag+. A 1.00 M Na2CO3 solution is…

A: Given that Concentration of Ca+2 = 1.00 × 10–2 M Concentration of Ag+1 = 1.00 × 10–2 M Ksp of CaCO3…

Q: What is the solubility of Fe(OH)2 (Ksp = 7.9 × 10–15) in a solution that has a pH of 9.55?

A: Given that p H =9.55. Thus, p OH = 14-9.55 = 4.45 pOH=4.45pOH= -logOH-OH-=10-4.45=3.55×10-5 M

Q: What will be the pH of a buffer

A: Given :-  Concentration of weak acid i.e. HCN = 0.65 M  Concentration of conjugate base i.e. CN- =…

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.