6- what is the solubility of Pb(0H)2 if Ksp at 20c0 = 2. 5x10-16 ? 3.9 x10-6 0.039 x10-6

Q: Calcium hydroxide is "sparingly soluble" with a Ksp value of 6.5 x 10-6 . Which substance can be…

A: Answer:Le Chatalier's principle states that on changing any parameter of the system that is in…

Q: What is the solubility of Pb3(PO4)2 if it's Ksp is 3.000e-44?

A: Ksp = 3.00e-44 Solubility =?

Q: What is the solubility of Agl(s) in 0.050 M Nal(aq)? Agl(s) Ag+(aq) + 1-(aq) Ksp = 8 x 10-17

A:

Q: Calculate the molar solubility of SrC₂O4 in a solution that has a fixed H3O+ concentration of (Ksp…

A: Answers: (a) Molar solubility = 6.42 x 10-7 M (b) Molar solubility = 6.55 x 10-8 M (c) Molar…

Q: - 1. The Ksp of Cu3(ASO4)2 at 25 °C is 7.6 x 10-36. What is the molar solubility (s) of Cu₂(ASO4)2…

A: Given,1. The Ksp of Cu3AsO42 at 25 °C = 7.6 × 10-36 .2. Concentration of PbNO32 solution = 0.10 M…

Q: Calculate the solubility (in g/L) of silver chromate in water at 25°C if the Ksp for Ag3PO4 is 1.75…

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Q: Equal volumes of a 5.28 x 10-4 M nickel (II) nitrate solution and a 3.18 x 10-3 M sodium carbonate…

A:

Q: 18. Calculate Qsp when 100.0 mL of 0.00250 M BaCl2 are mixed with 200.0 mL of 0.00500 M K2SO4. Will…

A: The concentrations of Ba2+ and SO42- has to be first calculated. Due to mixing of two solutions, the…

Q: Hg₂ Cl₂ (s) Hg2 (aq) + 2Cl(aq) = Ksp = 1.20 × 10–18 Determine the concentrations of Hg2+ and Cl¯ in…

A: To determine the concentration of  Hg22+ and Cl- in pure water and at ionic strength of 0.010 M and…

Q: Q2) Q1) what is the concentration of Sr2 in PPm for the solution in equilibrium with the precipitate…

A: Pksp od SrO4 = 6.55 MW of Sr = 87.6 g/mol We have to find the concentration of Sr2+ in ppm

Q: What is the molar solubility of Pb²+ in the following equilibrium (to 2 significant digits)?…

A:

Q: What is the molar solubility of CuCl (Ksp=1.7 x 10-7) in a solution of 0.023 M FeCl2?

A:

Q: The  Ksp for  BaCrO4 is  1.2×10−10.1.2×10−10. Will BaCrO4 precipitate upon mixing 10 mL of…

A:

Q: The Ksp of PbCl2 is 4.37⋅10−164.37⋅10-16 M.  Calculate the solubility of each ion in a saturated…

A:

Q: How would I solve this problem? 1) Calculate the molar solubility of Cd(OH)2 (Ksp = 1.2 x 10-14)…

A: Given: Ksp=1.2×10-14Molarity of Cd3(PO4)2=0.05 M To find: Molar solubility of Cd(OH)2

Q: A solution contains 0.0480 M Ca²+ and 0.0940 Agt. If solid Na3PO4 is added to the mixture, what is…

A:

Q: Use the reaction quotient to predict whether a precipitate will form. If 15.0 mL of 3.74×104 M Cal2…

A: The objective of the question is to predict whether the precipitate will occur or not.

Q: Calculate the molar solubility of SrC2O4 in a solution that has a fixed H3O+ concentration of (Ksp…

A: The objective of the question is to calculate the molar solubilty of .

Q: What is the solubility of Pb3(PO4)2 if it's Ksp is 3.000e-44?

A: The solubility of a sparingly soluble salt is determined by the equilibrium constant.

Q: The concentration of OH in a saturated solution of Mg(OH)2 is 3.62 × 10 M. The Ksp of Mg(OH)2 is 4.7…

A:

Q: A buffer solution contains 0.10M benzoic acid (C6H5COOH, Ka= 6.3 x 105) and 0.10M potassium benzoate…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: I need help on question 1

A: Let x be the concentration of Ca2+ and SO42-. The Ksp expression for CaSO4 is shown as follows,

Q: CaC2O4 (calcium oxalate) has a Ksp of 2.32 x 10-9. Solve for its molar solubility if its pH is 3.

A: Formula used:  X (s) -----> aA+  + bB-  Ksp = [A+]a [B-]b  Where  A+  and B- are relative cation…

Q: Calculate the solubility of BaSO4 with the Ksp = 1.08 x 10-10 ,in an aqueous solution with I =…

A: The solution is having BaSO4 and I-  The solubility reaction of BaSO4 is  BaSO4 (s) ------> Ba2+…

Q: When 25.0 mL of a 6.89 × 10-4 M potassium sulfide solution is combined with 18.0 mL of a 3.42 x 10-4…

A:

Q: Calculate the molar solubility of LizPO4 (Ksp = 2.37 x 10-") in a %3D 0.0379 M lithium nitrate…

A: Molar solubility is the number of moles of solute that can be dissolved in a litre of solution. It…

Q: Knowing that Ksp of PbI2 = 10-⁷ find out if precipitate will form when mixing 100ml of 0.01 N Pb…

A: The reaction between lead nitrate and sodium iodide is given by Pb(NO3)2 + 2 NaI → PbI2 + 2 NaNO3…

Q: Solid aluminum hydroxide (Ksp = 1.3 x 10-33) is added to 3.50 mM Al(NO3)3 solution until there are…

A:

Q: What is the molar solubility of PbI2 in

A: PbI2 is a sparingly soluble salt                                            PbI2    ⇔   Pb+2       +…

Q: You prepare a solution by mixing 400.0 mL of 1 x 10-4 M Mg(NO3)2  and 500.0 mL of 1.00 x 10-4 M NaF.…

A: Solubility product for MgF2 can be writte as Ksp =Mg2+F-2 Now, to determine weather precipitate…

Q: Determine the molar solubility for Sr3(PO4)2 by constructing an ICE table, writing the solubility…

A: Answer:Sparingly soluble salts are the ionic compounds that are very less soluble in water and all…

Q: Will a precipitate form if a mixture contains (Ag+) = 1.2 x 10-4 M and (C2O4-2) = 4.7 x 10-3 M?…

A:

Q: What is the concentration of Ca2+ that can be found in a saturated solution of CaF2 (s) at 25 °C ?…

A: Ksp is the solubility product constant. It is an equilibrium constant for a solid substance…

Q: if the ksp value of PbF2 is 3.3x10-8 what will be its solubility

A:

Q: what is the solubility of magnesium hydroxide in 0.0050 M MgCl2? Ksp= 6.0x10-12.

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

Q: 5-ksp When 15.0 mL of a 9.75×104 M calcium bromide solution is combined with 12.0 mL of a 4.62×104 M…

A:

Q: hat percent of Ba2+ ions remain  when CaSO4 begins to precipitate from asolution that is 0.05M in…

A: To determine the percent of Ba2+ ions remain when CaSO4 begins to precipitate from the solution.…

Q: If the solubility product of CaF2 is 1.46 x 10 ^-10 mol3 dm^-9, what mass of calcium fluoride will…

A: CaF2 dissociates to give Ca2+ and F- ions as follows: CaF2 <----> Ca2+ + 2F- Now, sodium…

Q: P Chemical eg X P Chemical eq X P Chemical ec X P Chemical ec X P Chemical ec x P Chemi…

A: Given: The molar solubility of BaCrO4 is 1.08*10-5 M.

Q: What is the molar solubility (in mol L-1) of a salt with general molecular formula MX (where M is a…

A: Given data :  1.Initial solubility of M+ = 0.534 mol-1 2. Ksp of MX = 2.1 x 10-8

Q: At 30 °C the Ksp of Pbl2 is 3.2 x 10-8. What is the molar solubility? (Hint, to make this math you…

A: Ksp of PbI2 = 3.2 x 10-8

Q: What is the molar solubility of Ag2SO4 (Ksp = 1.2 x 10-5) in a 0.10 M solution of Na₂SO4? 5.48 x…

A: The solubility product constant, Ksp of Ag2SO4 = The concentration of Na2SO4 solution= 0.10…

Q: Will a precipitate form if a mixture contains (Ag+) = 1.2 x 10-4 M and (C2O4-2) = 4.7 x 10-3 M?…

A: Here, Concentration of [Ag+] = 1.2 x 10-4 M. Concentration of [C2O4-2] = 4.7 x 10-3 M. Ksp = 3.5 x…

Q: What is the molar solubility of barium oxalate at pH of 8? Ksp=10-6

A: The equation for the dissociation of barium oxalate, BaC2O4(s) is: BaC2O4(s) ⇌ Ba2+(aq) + C2O42-(aq)…

Q: 100.0 mL sample of 0.020 M NiCl2 and a 100.0 mL ample of 0.025 M NalO3 are combined at 298 K. You…

A:

Q: Calculate the solubility of PbCl4 in a .2 Moles solution of CaCl2 Ksp for PbCl4 = 8.7 x 10-75

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.