determine the molar solubility oc Cucl in a solution containing 0.050 M KCL. KSP FOR CUCL =1.0X10^-6

Q: Complete the following solubility constant expression for SrCO 3.

A: SrCO3 ionises as : SrCO3 ----------> Sr2+ + CO32- Solubility product Ksp = [Sr2+][CO32-] Let the…

Q: When 25.0 mL of a 2.43×10-4 M manganese(II) acetate solution is combined with 12.0 mL of a 9.49×10-4…

A: In a chemical reaction; the substance which involves in conversion is said to be reactant whereas…

Q: Calculate the solubility of the following compounds in water. (Use internet or tables in the…

A:

Q: The solubility product, Ksp, for AgI is 8.3 x 1017. What is the concentration of iodide ion (I') in…

A: The solubility reaction of AgI is  AgI (s) --------> Ag+ (aq) + I- (aq)

Q: The solubility product of MgF, is 10-8.2. (A) What is the solubility of Mg* at equilibrium with…

A: Given: Ksp of MgF2 = 10-8.2 = 6.31 X 10-9 approx.

Q: When 12.0 mL of a 7.72×10-4 M silver nitrate solution is combined with 15.0 mL of a 6.93×10-4 M…

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Q: The Solubility Product Constant for zinc cyanide is 8.0 × 10-¹2 The molar solubility of zinc cyanide…

A:

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

A:

Q: the solubility of pure gallium iodide Ga (IO3) 3 in water with Kpt = 2.5 × 10-¹¹ is: a) 6.27 g b)…

A: According to the question,  Ksp of Ga(IO3)3 = 2.5*10-11 we need to calculate the solubility of…

Q: 3. The solubility product constant (Ksp) of iron (III) chloride is 1.7 x 10-6. Calculate the molar…

A: Solubility product of iron (III) chloride = The solubility product ( Ksp ) of a sparingly soluble…

Q: The Solubility Product Constant for aluminum phosphate is 1.3 × 10-2⁰. The maximum amount of…

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

Q: What is the concentration of Fe²+ in a saturated solution of Fe(OH)₂ if its solubility is 1.59x10-5…

A: Answer:- This question is answered by using the simple concept of calculation of concentration using…

Q: The solubility of copper(I) chloride is 3.91 mgmg per 100.0 mLmL of solution.   Part A…

A:

Q: O Define molar solubility and solubility. O The solubility product, Ksp of silver chloride, AgCl is…

A: Given solubility product of AgCl is 1.0×10-10  Molar mass of AgCl is 143.3 g/mol.

Q: 1. What is the molar solubility of Ag2SO4? KS= 1.52 x 10-5 b. What is the molar solubility of…

A: Given : compund and their solubility product

Q: Will a precipitate form when 100.0 mL of 4.0 × 10 −4 M Mg(NO3 )2 is added to 100.0 mL of 2.0 × 10 −4…

A: Given data contains, Volume of Mg(NO3 )2 is 100.0 mL. Molarity of Mg(NO3 )2 is 4.0 × 10-4 M. Volume…

Q: When 15.0 mL of a 6.01×10-4 M silver acetate solution is combined with 12.0 mL of a 6.40×10-4 M…

A: The balanced chemical equation for the reaction between silver acetate and sodium hydroxide can be…

Q: 5. In a certain experiment, 750.0 mL of water at 25°C is needed to prepare a solution of AgaCrO4.…

A: Answer: For a sparingly soluble salt, at saturation point ionic product becomes equal to solubility…

Q: ?locator%3Dassignment-take The solubility of silver cyanide, AgCN, in water is 1.0 x 10° gL.…

A: The solubility of silver cyanide is = 1.0×10-6 g/L The solubility product constant for silver…

Q: The Ksp of calcium fluoride (CaF2) for the reaction: CaF2(s) = Ca2+ (aq) + 2F¯(aq)is given that its…

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Q: AgCl has a solubility of 2.2E0 mg/L at room temperature. Based on this information, what is the K…

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Q: When 12.0 mL of a 1.51×10-4 M copper(II) chloride solution is combined with 15.0 mL of a 7.02×10-4 M…

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Q: The molar solubility of silver chromate, Ag2CrO4, in water at a certain temperature is 6.9 x 105 M.…

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Q: À CHM 122 student determines that the molar solubility of AGCI(s) in pure water is 1.3 x 10 mol/L.…

A: The Ksp for a salt is be expressed as: AxBy → x Ay+ + y Bx- Ksp = [Ay+]x [Bx-]y

Q: When 15.0 mL of a 4.72×10-ª M iron(II) bromide solution is combined with 12.0 mL of a 9.07×10-4 M…

A: Ionic product (Kip) Ionic product is the product of concentrations of ions in the solution. It is…

Q: What is the molar solubility for Mg(OH)2 if the Ksp= 2.06x10^-13 A. S=2.27x10^-7 B. S=3.72x10^-5…

A:

Q: Calculate the solubility of silver chloride (AgCl) in g/L. Ksp = 1.6 x 10-10 MM of Ag: 107.8 g/mol;…

A: Given-> Ksp = 1.6 × 10-10 Atomic mass of Ag = 107.8 g/mole Atomic mass of Cl = 35.4 g/mole

Q: The molar solubility of Mt(CO3)2 is 2.7x10^-7 mol L -1. What is its Ksp?

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Q: The solubility of tin(ll) sulfide is 2x10^-14 mol/L. Calculate the Ksp of tin (ll) sulfide.

A: Tin(II) sulfide is a sparingly soluble salt and it dissolves in very low quantity in the aquoeous…

Q: Determine the molar solubility for barium fluoride (BaF2). Ksp = 1.8 x 10-7

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Q: The Solubility Product Constant for magnesium carbonate is 4.0 x 10-5. The maximum amount of…

A: Given,Molarity of magnesium nitrate = 0.270 MThe solubility product of magnesium carbonate = 4.0 x…

Q: Choose the correct solubility constant expression for iron(II) hydroxide in water: Ksp =…

A:

Q: Determine the molar solubility of CuCl in a solution containing 0.060 M KCl. ksp(CuCl)=1.0x10^-6

A: Given;

Q: What is the molar solubility (in M to two decimal places) of copper(II) hydroxide in water (at 25…

A:

Q: The solubility of magnesium oxalate, MgC₂04, n water is 0.0093 mol/L. Calculate Kp.

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Q: e solubility of an ionic compound MX (molar mass = 436 is 6.43 x 103 g/L. What is the Ksp ?

A: Given, molar mass of ionic compound MX = 436 g.mol-1 Solubility of the compound = 6.43 ×10-3 g/L

Q: the

A: Solubility Product constant value Ksp for Barium chromate ( BaCrO4 ) is 2.2 • 10^-10  Ksp = 2.2 •…

Q: What is the molarity of a saturated solution of Ag,S? Ag₂S has a ksp of 1.6 X 10-4⁹ and it has a…

A: Gives us Ksp for Ag2S = 1.6 * 10-19Molar mass of Ag2S = 247.9 g/molmolarity of saturated solution of…

Q: When 18.0 mL of a 2.79×104 M potassium phosphate solution is combined with 18.0 mL of a 7.38×104 M…

A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…

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.