Calculate Ksp for calcium hydroxide if a saturated solution contains 0.20M of calcium hydroxide.

Q: Calculate the concentrations of sodium ions and sulfate ions in a saturated aqueous solution of…

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Q: Calculate the molar solubility of solid zinc hydroxide, Zn(OH)2 (s), with a Ksp of 5.0 x10^-17 .

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Q: Define the term selective precipitation?

A: Given term,           Selective precipitation

Q: What is the solubility of MgCO, in a solution that contains 0.080 M Mg2 ions? (Ksp of MgCO, is 3.5 x…

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Q: Which of the following has the largest molar solubility? A) BaSO4, Ksp = 1.1 × 10-10 B) AgCl, Ksp =…

A: The Molar solubility and the Ksp (solubility product) are directly proportional to each other .…

Q: Calculate the molarity of AgCl in 0.102 M NaCl solution. The Ksp for Silver Chloride is: 1.83 x…

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

Q: Calculate the Ksp value for a solution of magnesium fluoride. The molar solubility of magnesium…

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Q: The molar solubility of mercury (II) sulfide is below. What is the Ksp ? Molar solubility = 2.9 x…

A: given data from question -  molar solubility = 2.9 x 10-25 g/L Ksp = ?

Q: The molar solubility of SrF2 is 2.5 x 10-9 M. Calculate the Ksp of SrF2.

A: The dissociation of the magnesium hydroxide takes place as follows: SrF2s ⇌ Sr2+aq + 2F-aq

Q: What is the pH at 25degrees Celsius of a saturated solution of silver hydroxide? (Ksp value for…

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Q: Given the equilibrium reaction  MgF2(s) ↔ Mg+2(aq) + 2F-(aq)                      Ksp = 7.4x10-11…

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Q: The solubility of barium chromate at 25 degrees C is 0.279 mg/ 100 mL. Calculate the Ksp of barium…

A: Solubility = 0.279 mg / 100 ml  Solubility = 2.79  mg / L  Solubility = 2.79 / 253 = 0.011 m moles…

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: The solubility of lithium fluoride (LiF) is 0.13g per 100mL. Calculate the Ksp for LiF.

A: Given, Mass of LiF = 0.13 g Volume of solution = 100 mL = 0.1 L Molar mass of LiF = 25.9 g/mol

Q: Determine the solubility of AgBr in A. Water B. 6.0x10^-2M AgNO3 C. 0.20M NaBr

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Q: Cite one example where precipitation titration could be applied in food technology.

A: It is used for the determination of halide ions in the solution. It is used to measure salt content…

Q: Mn(OH), has a molar solubility of 2.2 x 10-5 M. Calculate the Ksp value for Mn(OH),.

A: Molar solubility of Mn(OH)2 = 2.2 × 10-5 M  Ksp value for the Mn(OH)2 = ?

Q: The molar solubility of nickel(II) sulfide in a 0.193 M ammonium sulfide solution is

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Q: Complete the following solubility constant expression for BaSO . K = 0 sp

A: Solubility product constant is equilibrium constant when solid dissolves in aqueous solution.…

Q: The molar solubility of magnesium hydroxide in a water solution is 3.72x10^-5 М.

A: Given that, The solubility product (Ksp) of magnesium hydroxide is 1.5 * 10-11 We have to calculate…

Q: Determine the Ksp for iron (III) hydroxide if Fe(OH)3 has a molar solubility of 1.3 × 10-¹0 mol/L at…

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Q: The molar solubility of silver chloride (AGCI) is 4.2 x 106 M. What is Ksp for this compound? O 4.2…

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Q: Hi, I need help with this step-by-step please. Thank you

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Q: The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp  for CuCl.

A: The solubility of copper (I) chloride is 3.91 mg per 100.0 mL of solution. Ksp  for CuCl is to be…

Q: Q-4- calculate the molar solubility of Barium iodate 1- in distilled water 2- in Barium nitrate…

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Q: Determine the molar solubility for Sr3(PO4)2 (Ksp = 1.0 x 1031).

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Q: The value of Ksp for Cd(OH)2 is 2.5 * 10-14. What is the molar solubility of Cd(OH)2?

A: The solubility product of a particular compound is the product of the molarities of the ions present…

Q: . The Ksp for copper (II) hydroxide is 1.6 x 10-19; calculate the molar solubility and concentration…

A: In this question, we want to determine the Concentration of Cu2+ ion and molar solubility of its…

Q: What is the molar solubility of mercury (I) fluoride?  Ksp = 3.1 x 10-6.

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Q: Complete the following solubility constant expression for Ag,CO3. K - 0 sp

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Q: The molar solubility of Ca(OH)2 was experimentally determined to be 0.019 M. Based on this value,…

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Q: Complete the following solubility constant expression for Co (OH),. sp =

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Q: The molar solubility of Mg(CN)2 is 1.4 x 10-5 M at a certain temperature. Determine the value of Ksp…

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Q: How many grams of Silver carbonate are required for 540 mL of its saturated solution? Its Ksp is 8.1…

A: Recall the dissociation of silver carbonate in aqueous solution Ag2CO3 ---> 2Ag+ + CO32-  Given…

Q: If the molar solubility of CaF2 at 35 °C is 1.24 * 10-3 mol/L, what is Ksp at this temperature?

A: Molar solubility of CaF2 is 1.24x10-3 mol/L CaF2 (s)→ Ca2+ (aq)+2F- (aq) S = 1.24x10-3 mol/L

Q: At a particular temperature the [Ba2+] in a saturated solution of barium sulfate is 1.04x10-5 M.…

A: Since the dissolution reaction of barium sulfate is  BaSO4 (s) ----> Ba2+ (aq)+ SO42- (aq) Hence…

Q: bility of barium Florida i

A: Molar solubility gives the number of moles that are dissolved in 1L of solution.

Q: solubility equilibrium for CaBr2 is 4.8x10-8.

A: CaBr2 ⇋  Ca+2 +  2Br -1     t=0       a                -             -     t=t      a-S…

Q: 5. Calculate the solubility of compounds. Assume T=25° C. a) Mg(OH)2(s) b) FeSts)

A: a) Mg(OH)2 b) FeS

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

A: Given;

Q: If Nickel(2)Carbonate has a solubility of 4.3 mg/100 mL at 25.0°C, determine Ksp

A: It is given that the solubility of NiCO3 is 4.3 mg/100ml and it is required to calculate the Ksp.

Q: If 600 mL of some Pb(NO3)2 solution is mixed with 350 mL of 1.80 x 10−2 M NaCl solution, what is the…

A: First, the reaction between Pb(NO3)2 and NaCl is shown below, From given molarity value of NaCl the…

Q: If 100.0 g calcium phosphate (Ksp= 1.3 x 10^-32) are placed in enough water to generate 750.0 mL of…

A: Given : Mass of calcium phosphate given = 100.0 g Volume of solution given = 750.0 mL = 0.750 L…

Q: Determine the molar solubility for Sr₃(PO₄)₂ (Ksp = 1.0 × 10⁻³¹). (ICE table)

A: S=1.25×10-10M

Q: Complete the following solubility constant expression for CaF2. K sp

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Q: Arrange the following in order of increasing molar solubility: Fes (Ksp - 3.7 x 10°19): Caco3 (Ksp -…

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Q: A saturated solution of AB2 contains 8.60 x 10.4 moles AB2 per liter. Determine Ksp.. 2.54 x 10-⁹…

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Q: The molar solubility of iron(II) hydroxide in a water solution is  M. ksp for iron hydroxide is…

A: GIVEN:  ksp for iron hydroxide is 7.9x10-15 To Determine: Molar solubility of iron(II) hydroxide in…

Q: Calculate the molar solubility of Barium Sulfate. (Ksp 1.1 x 10 10) O 1.3 x 10^(-6) M O 1.2 x…

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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.