For calcium fluoride, CaF2, Ksp = 4.0 x 10-11. What is the minimum concentration of Ca2+needed to precipitate CaF2 from a 0.20 M solution of sodium fluoride, NaF?

Q: Iron(II) hydroxide, Fe(OH)2, has a solubility in water of 6.0 x 10¹ mg/L at a given temperature. (a)…

A: Solubility product is defined as the product of the concentration of the ions which is in…

Q: The Solubility Product Constant for zinc carbonate is 1.5 × 10-¹¹. Solid potassium carbonate is…

A: We will first determine the Ksp expression. and we will get the concentration of Zn2+ from the…

Q: The Ksp of zinc hydroxide, ZN(OH)2 is 3.00 x 10-17. Calculate the solubility of this compound in…

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Q: Determine the molar solubility of CuCl in a solution containing 0.050 M KCl. Ksp (CuCl) = 1.0 ×…

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Q: concentration of phosphate

A: A precipitation reaction refers to the formation of an insoluble salt when two solutions containing…

Q: Lead (II) bromide, PbBr2, has Ksp = 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of…

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Q: A 0.10-M Ba(NO3)2 solution is added to four separate beakers as follows: 50.0 mL of 0.10 M Na2S 50.0…

A: Given question related to the solubility of barium salts in water.

Q: Lead (II) bromide, PbBr2, has Ksp= 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of…

A: (a) The concentration of Pb2+  after mixing = 0.10 M×20.0ml20.0ml +30.0 ml…

Q: A solution contains 7.94×10-3 M sodium phosphate and 1.44×10-2 M sodium chloride. Solid silver…

A: When ionic product is higher than that of the solubility product, the precipitation occurs.

Q: The solubility product constant of silver sulfate, Ag2SO4, is 1.2 x 10-5. Determine the mass of…

A: we are required to find  the mass of Ag2SO4 that can be dissolved in 2.00L of a 0.572 M solution of…

Q: What is the molar solubility of calcium carbonate (Ksp = 9.0 x 10-9) in 0.15 mol/L sodium carbonate?

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Q: What happens when équal Võlumes of 281C M aqueous solutions of calcium nitrate. ca(NO3)2, änd sodium…

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

Q: Will a precipitate (ppt) form when 300.0 mL of 5.0 x 10 M AgNO, are added to 300.0 mL of 2.5 x 10-´M…

A: Given: The volume of AgNO3 is 300.0 mL The molarity of AgNO3 is 5.0 x 10-5 M The volume of NaBr is…

Q: A solution contains 8.73x10-3 M potassium iodide and 9.62x10-3 M ammonium bromide. Solid lead…

A: The concentration of ammonium Bromide = 9.62 × 10–3 M The concentration of potassium iodide = 8.73 ×…

Q: The solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C 1.) A 50.0…

A: First we need to calculate the molar solubility of Fe(OH)2 using the given solubility in g/L and its…

Q: At a certain temperature MgF2 has Ksp = 2.34 x 10-10. Calculate the minimum concentration of Mg2+…

A: Given , Ksp of MgF2 = 2.34×10-10 Concentration of NaF = 0.0125 M As NaF is a strong electrolyte , it…

Q: A solution contains 1.42×10-2 M ammonium sulfate and 5.66×10-3 M ammonium chromate. Solid barium…

A: Given :  Concentration of ammonium sulfate = 1.42 x 10-2 M  Concentration of ammonium chromate =…

Q: The Ksp of magnesium hydroxide, Mg(OH)2, is 5.61 × 10-¹2. Calculate the solubility of this compound…

A: The Ksp expression for a salt is the product of the concentrations of the ions, with each…

Q: The solubility product, Ksp, of PbCl2 is 1.6 × 10-5. What mass of KCl(s) must be dissolved in 150.00…

A: Given: Ksp of PbCl2 = 1.6 x 10-5 Qsp = [Pb2+] [Cl-]2 now, Qsp = Ksp, [Pb2+] x [Cl-]2 = 1.6 x 10-5…

Q: What is the molar solubility of MgF2 in 0.36 M NaF? For MgF2, Ksp = 8.4 x 10–8. 7.1 x 10–4 1.0 x…

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Q: For the following, please answer all the questions. Suppose the Ksp value for lead sulfide (PbS) is…

A: Let S be the solubility of PbS  in water.It is a AB2 type of salt. Hence the formula of solubility…

Q: If the concentration of Mg2+ ion in seawater is 1.35 x 10³ mg/L, what OH concentration is required…

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Q: The solubility of Fe(OH)3 is measured and found to be 2.30×10-8 g/L. Use this information to…

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Q: Calculate the maximum solubility of zinc(II) carbonate (Ksp = 1.46 x10-10) in a solution of 0.1M…

A: Ksp of ZnCO3= 1.46×10-10 concentration of Na2CO3= 0.1M Molar mass of ZnCO3= 125.4g/mol We need to…

Q: A student titrates 20.0 mL of 1.0 M NaOH with 2.0 M formic acid, HCOOH (K, = 1.8 x 10 4).…

A: The equivalence point is the theoretical value of the volume of acid required to titrate the base,…

Q: The solubility-product constants, Ksp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and…

A: Given :  Concentration of Fe+2 = 1.02 x 10-2 M  Concentration of Cd+2 = 1.48 x 10-2 M

Q: What is the molar solubility of calcium fluoride, CaF2, in a solution of 0.25 M calcium nitrate,…

A: Given:- Ksp for CaF2 is 3.45×10-11  Concentration of Ca(NO3)2 is 0.25 M We have to calculate…

Q: What is the solubility (in grams per liter) of strontium sulfate, SrSO4, in 0.26 M sodium sulfate,…

A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…

Q: The solubility-product constants, Kp, at 25 °C for two compounds [iron(II) carbonate, FeCO3, and…

A: Step 1: FeCO3FeCO3 → Fe2+ + CO32-Ksp = [Fe2+][CO32-]2.10 x 10-11 = [1.03 x 10-2][CO32-][CO32-] =…

Q: Lead (II) chloride, PbCl2, has Ksp = 1.6 x 10–5. (a) Determine the solubility of PbCl2 expressed in…

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Q: What is the solubility of Ag2CO3 (s) in moles per liter (mol/L) in pure water? O 2.0 x 10-4 O 1.3 x…

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Q: Complete the following solubility constant expression for ZnCO3. K = 0 sp X 0 9 3

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Q: Which of the following compounds will have the highest molar solubility in pure water? O MgCO3, Ksp…

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Q: The solubility product constant for CaCO3 (s) in water is Ksp = [Ca+2] [CO3 -2] = 4.8 x 10^-9…

A: Solution -

Q: Consider iron(II) hydroxide (Fe(OH)2, Ksp = 4.87 × 10-17). Write out the chemical equation for its…

A: The equilibrium reaction for solubility is given by  Fe(OH)2 (s) ----> Fe2+ (aq)+ 2 OH- (aq) Ksp…

Q: The Ksp of magnesium hydroxide, Mg(OH)2, is 5.61 x 10-12. Calculate the solubility of this compound…

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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.