The ksp of CaF2 is 3.9 x 10 -11 at 25o C. Assuming that CaF2 dissociate completely upon dissolving and that there are no other important equilibria affecting the solubility. Calculate the solubility of CaF2 in grams per liter.    ( mwt CaF2  = 78.1 g/mol)

Q: The Ksp of iron (II) hydroxide is 8.65 x 104 iron (III) hydroxide? -20 What is the molar solubility…

A: The solubility of iron (III) hydroxide can be expressed as: Ksp = Fe3+OH-3Ksp = s3s3Ksp = 27s4

Q: Will a precipitate form when 25 mL of 0.20M Ba(NO3)2 is mixed with 15 mL of 0.20M NaOH? (Ksp Ba(OH)2…

A:

Q: What is the molar solubility of lead chloride (PbCl2) in a solution that is also 0.117 M in sodium…

A:

Q: 1. 150.0 mL of 0.0100 M Mg(NO3), is added to 250.0 mL of 0.100 M NaF. Will MgF₂ precipitate? (Ksp of…

A: Solubility product quotient, Qsp is the product of the concentrations of the products, each raised…

Q: Determine the molar solubility of MgCO3 in pure water. Ksp (MgCO3) =6.82•10-6

A:

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: 9. If 50.0 mL of a 0.0010 M CaCl₂ solution were added to 50.0 mL of 0.010 M Na₂SO4 solution, would a…

A: 9.) Answer:

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

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Q: The solubility of CuCO3 can be enhanced in the presence of CN- according to the equation below. What…

A:

Q: If the Ksp of Ag3AsO4 at 25 oC is 1.03e-22 , what is the molar solubility of Ag3AsO4 at this…

A:

Q: Given that the Ksp for CaF2 at 25 °C is 3.9 × 10–11, will a precipitate form when 0.10 L of 2.3 x…

A: Given information: Ksp for CaF2 at 25 °C is 3.9 × 10–11 Concentration of CaCl2 = 2.3 x 10–4 M Volume…

Q: If 0.235 L of 1.48 x 10-2 M of Ca(NO3)2 is added to 0.688L of 3.25 x 0-2 M of Na2SO4, will a…

A: We have 0.235 L of 1.48 x 10-2  M of Ca(NO3)2 ,0.688L of 3.25 x 10-2 M of Na2SO4 .Ksp as 9.1*10-6 .…

Q: The kps for calcium carbonate (CACO3) is 8.7 x 10-9. X If in 2 L of solution there are 0.1 moles of…

A:

Q: = Ksp of lead(II) carbonate, PbCO3, is 7.40 x 10-¹4. Calculate the molar solubility, S, of this…

A: Solubility product constant (Ksp) is equilibrium constant of solid substance dissolve in aqueous…

Q: A 25.0-mL sample of 0.00200 M AgNO3 is added to 25.0 mL of 0.0100 M NaIO3. What is the + equilibrium…

A: The balanced net ionic reaction is:

Q: If 50.0 mL of a 0.0010 M CaCl2 solution were added to 50.0 mL of 0.010 M Na2SO4 solution, would a…

A: The reaction between calcium chloride (CaCl2) and sodium sulfate (Na2SO4) is represented as follows:…

Q: For BaF2 (Ksp = 1.7 × 10–6), will a precipitate of BaF2 form when 0.10 L of 6.0 × 10–2 M Ba(NO3)2 is…

A:

Q: Determine the molar solubility for Ag.CrO. (Ksp = 1.2 x 10 12). PREV 2 3 sed on your ICE table and…

A:

Q: Consider three different sparingly soluble ionic compounds, YX, ZX2, and AX3, with the same Ksp…

A: Ksp is known as solubility product. Higher the value of solubility product higher will be the…

Q: Which expression best describes the relationship between solubility product, Ksp, and the…

A: Solubility product is denoted by Ksp and it is defined as it is an equilibrium constant for the…

Q: The Ksp of Ag2CO3 (MM = 275.81 g/mol) at 25°C is 8.1 x 10-12 a. Calculate the molar solubility of…

A:

Q: What is the solubility (in g/L) of BaF2 at 25°C? The solubility product constant for BaF2 is 1.0 x…

A: Solubility product constant Ksp = 1.0 * 10-6 For BaF2 ,  BaF2 (s) <=> Ba2+ (aq) + 2 F- (aq)…

Q: What is the solubility (in mol/L) of PbCl2 given that the Ksp is 1.69⋅10-13.

A:

Q: The Ksp for Ag2CO3 at a certain temperature is equal to 8.59x10-12. What is the molar solubility of…

A: Sparingly soluble salt are dissolved is water partially.

Q: The molar solubility of palladium (II) thiocyanate at 25°C is 2.22 x 10-8 M. What is its Ksp value?…

A: molar solubility=S=2.22×10-8M KSP=?

Q: a) The concentration of Mg2+ in seawater is 0.052 M. If the Ksp for Mg(OH)₂ is 8.9 × 10-¹2, at what…

A: (a)The concentration of Mg2+ that can remain in sea water is (100-99.9)% =0.1% Our target is that…

Q: What is the solubility (M) of PbCl2 in 0.12 M of HCL?Ksp for PbCl2 is 1.6*10-5?

A:

Q: 4. Tap water contains the sulfate ion 50 at about 0.00400 mol/L. If 15 mL of 0.00100 of barium…

A:

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 CaF2 is 3.9 x 10-11 at 25 °C. Assuming equilibrium is established between solid and…

A: The solubility reaction is  CaF2 (s) -------> Ca2+ (aq) + 2 F- (aq) Hence the equilibrium…

Q: When 200.0 mL of 5.15 x 10-4 M Ba(NO3)2 is added to 150.0 mL of 8.25 x 10-4 M Na2SO4. Ksp(BaSO4) =…

A: We know if Ionic product is more than solubility product then precipitate forms. if ionic product is…

Q: Does precipitate form if we mix equal volumes of solutions BaCl2 0.008 M and Na2SO4 0.002M? During…

A: Solubility product It is an equilibrium constant where each of the concentration term is multiplied…

Q: a) The concentra=on of Mg2+ in seawater is 0.052 M. If the Ksp for Mg(OH)2 is 8.9 × 10–12, at what…

A: (a)The concentration of Mg2+ that can remain in sea water is (100-99.9)% =0.1% Our target is that…

Q: One way to reduce the presence of lead in water is to add a phosphate corrosion inhibitor, which…

A:

Q: Sodium carbonate, Na2CO3, is added dropwise to a solution that contains 1.0 X 10-2 M Ag+ and 5.0 X…

A: NOTE : I assume that in question  5.0 X 10-2 M Cd2+ has been typed incorrectly instead of  5.0 X…

Q: Use the Ksp values to calculate the molar solubility of CaCO3 and MgCO3. What mass of CaCO3 (in…

A: The Ksp value of CaCO3 is 0.5 × 10-8. The solubility of CaCO3 can be determined as: Ksp = Ca2+CO32-…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for