What is the molar solubility of NiS in 0.40 M NH3? The Ksp for NiS is 3.0 × 10-19. The K₁ for Ni(NH3)62+ is 5.6 × 108. Molar solubility = M

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: f 27.5 mL of 1.63x10-9M of FeCl3 is added to 98.6mL of 2.58x10-9 M NaOH, will a precipitate of…

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

Q: What is the molar solubility of PbSO4 in 0.19 M MgSO4? Ksp = 1.0 ✕ 10-8 for PbSO4. (in M)

A: The given data contains, Mg2+=SO42-=0.19 M. Ksp for PbSO4=1.0×10-8

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: An analytical chemist has been given the task of precipitating lead cation (Pb2+) out of solution…

A: Given,  Molar concentration of Pb2+ ion = [Pb2+] = 0.424 M  Solubility product constant of PbI2 =…

Q: What is the molar solubility of Mg(OH)2, Ksp is 5.6 x 10^-12 for Mg(OH)2 in the following aqueous…

A:

Q: What is the molar solubility of barium oxalate(BaC2O4) in a solution buffered to a pH of 6.65? The…

A: Let the molar solubility of Barium oxalate be "s" mol/L.On dissolution into the…

Q: The solubility product of Ni(OH)2 at 25 oC is Ksp = 1.6 x 10-16. Calculate the molar solubility of…

A: In this question, we want to determine the value of molar solubility of Ni(OH)2  You can see details…

Q: Calculate the molar solubility  of Mg(OH)2 Ksp=8.9×10^-12

A: The dissociation reaction of Mg(OH)2 is given below.

Q: The solubility of AgCl in 0.010 M NH3 is equal to the Ksp1/2 of AgCl. True or False?

A: Answer: In this question we have to establish the fact that whether the presence of NH3 affects the…

Q: ト juIH Calculate the pH for each of the cases in the titration of 25.0 mL of 0.120 M pyridine, C, H,…

A:

Q: What is the maximum concentration of Ag⁺ that can be added to a 0.00730 M solution of Na₂CO₃ before…

A: Ag+ was added to a 0.00730 M solution of Na2CO3 to form a precipitate . The Ksp of Ag2CO3 is8.10 ×…

Q: Kf for the complex ion Ag(NH3)2+ is 1.7 x 107. Ksp for AgCl is 1.6 x 10-10. Calculate the molar…

A: Given : The equilibrium constants for the complex formation Ag(NH3)2+, is 1.7 X 107 and the Ksp of…

Q: If 10.0mL of 2.0x10^-3 M Cr(NO3)3 is added to 10.0mL of a pH = 10.0 NaOH solution, will a…

A: The number of moles of a substance is given as the mass of a substance upon its molar mass. The pH…

Q: A HCN / NaCN buffer system is to be constructed that is also 0.039 M in Mg2+. What is the minimum…

A: In the given question we have to calculate the ratio of HCN to CN- by using the henderson…

Q: What is the molar solubility of AgCl (Ksp = 1.80 × 10⁻¹⁰) in 0.570 M NH₃? (Kf of Ag(NH₃)₂⁺ is 1.7 ×…

A: Given: Ksp of AgCl=1.80×10-10Molarity of NH3=0.570 MKf of Ag(NH3)2+=1.7×107

Q: A chemistry graduate student is given 100. ml. of a 0.10M pyridine (C,H,N) solution. Pyridine is a…

A:

Q: Calculate the molar solubility of CaF2 at 25 °C in a solution that is 0.010 M in Ca(NO3)2

A: CaF2 dissociates as                     CaF2 (s)  →  Ca+  +  2F- Initial…

Q: What is the molar solubility of AgCl (Ksp = 1.80 × 10⁻¹⁰) in 0.390 M NH₃? (Kf of Ag(NH₃)₂⁺ is 1.7 ×…

A:

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: What is the molar solubility of AgCl (Ksp = 1.80 × 10⁻¹⁰) in 0.740 M NH₃? (Kf of Ag(NH₃)₂⁺ is 1.7 ×…

A:

Q: Calculate the molar solubility of silver iodate in 0.12 M sodium iodate. Ksp= 3.2 x 10-8

A: Given that ,  Solubility product of silver iodate , Ksp = 3.2×10-8 Molar solubility of silver iodate…

Q: A chemistry graduate student is given 100. mL of a 1.50 M benzoic acid (HC H,CO,) solution. Benzoic…

A: Given : Concentration of weak acid HC6H5CO2 = 1.50 M Volume of solution = 100 mL = 0.100 L…

Q: An analytical chemist has been given the task of precipitating lead cation (Pb2+) out of solution…

A: Concept based on the solubility product of the sparingly soluble salts.

Q: Calculate the molar solubility of Ag2SO4. Ksp = 1.5 × 10–5 Group of answer choices 0.0027 M 0.016 M…

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

Q: A chemistry graduate student is given 100. mL of a 0.30M diethylamine ((C,H;), NH) solution.…

A:

Q: The solubility product constant for Hg(IO3)2 is 3.2 x 10-13. What is the Hg2+ concentration of a…

A: Ksp = 3.2*10-13 Hg(NO3)2 + KIO3 -------> Hg(IO3)2 + KNO3 Ksp = [s]*[s]  3.2*10-13 = s2 = 5.6*10-7…

Q: Suppose 100 mL of 2.0 × 10–4 M Fe(NO3)3is added to 100 mL of 2.0 ×10–5 M KIO3. What is Qsp value?…

A: when Qsp < Ksp and then compound does not precipitated. For precipitation, Qsp > Ksp

Q: Calculate the solubility of Cu(OH)2 in an aqueous solution of KCN 0,10 mol/L.

A:

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- =…

Q: What is the molar solubility of AgCl (Ksp = 1.80 × 10⁻¹⁰) in 0.500 M NH₃? (Kf of Ag(NH₃)₂⁺ is 1.7 ×…

A: Given : Concentration of NH3 = 0.500 M The solubility reaction of AgCl can be written as  => AgCl…

Q: A friend tells you: " The constant K sp of a salt is called the sol ubility product constant and is…

A: Solubility product is used only for those salts that are sparingly soluble and there exists…

Q: What is the molar solubility of AgCl (Ksp = 1.80 × 10⁻¹⁰) in 0.600 M NH₃? (Kf of Ag(NH₃)₂⁺ is 1 ×…

A: Here, AgCl(s) → Ag+(aq) + Cl-(aq)    for this reaction Ksp=1.8×10-10 also, Ksp=[Ag+][Cl-] .... (i)…

Q: Calculate the molar solubility of CdF2 in 0.120 M NaF. The Ksp of CdF2is 6.44× 10-3

A: The solubility equilibrium in this case is represented as,                        CdF2 (s)   ⇌…

Q: What is the solubility (in mol/L) of silver chromate in 1.10 M potassium chromate aqueous solution?…

A: Reaction involved:- Ag2CrO4 = 2Ag+ + CrO42-

Q: Predict the equivalence point that occurs for the following titrations: The when C5HSN (aq) is…

A: Equivalence point is defined as the point when equivalent amount of acid and base react completely…

Q: What is the molar solubility of CaF2 in 0.10 M NaF solution at 25 °C? The Ksp for CaF2 is 3.4 ×…

A:

Q: What is the molar solubility of AgCl (Ksp = 1.80 × 10⁻¹⁰) in 0.420 M NH₃? (Kf of Ag(NH₃)₂⁺ is 1.7 ×…

A: In this question, we have to find out the correct answer of given problem by the help of Equilibrium…

Q: buffer solution is 0.500 M in KF and 0.500 M in HF (KA = 3.5 × 10–4). What is the solution’s pH…

A: Here we have to use Henderson–Hassel Balch equation for determination of pH of solution. Generally…

Q: PbI2 has a molar solubility of 1.52 x 10^-3 M. Calculate the Ksp value for PbI2

A: Solubility product of PbI2 is -  Given PbI2 has molar solubility =1.52 ×10-3

Q: approximately 3.2? O A solution of 6.3 x 104 moles of HNO3. O A solution of 0.100 moles of NH3 (Ko =…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Suppose that we have a solution that is 0.0010 M Cl - and 0.100 M CrO4 2-. If we add 0.100 M AgNO 3,…

A:

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.