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A solution has Ag 7.7 10 5 and Cl 2.5 10 3 If Ksp for AgCl is 1.8 10 10 what is true about this solution?
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∙ 14y ago
The solution is supersaturated.
Wiki User
∙ 14y ago
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What is the solubility of AgCl if it has Ksp equals 3.2 10-10?
From the definition of Ksp, the product of the concentrations of Ag+ and Cl- can be no more than (1.8 X 10-10)/0.35 = 5.1 X 10-10. Since the only named material that is a source of silver ions is AgCl and the concentrations are molar, this is the maximum possible solubility of AgCl.
If AgNO3 solution is added to a solution containing Br ions until the silver ion concentration is 1.3x10-6 what is the Br ion concentration The ksp for AgBr is 5.2x10-23?
To determine the concentration of Br ions, we can use the solubility product constant (Ksp) expression for AgBr, which is equal to [Ag+][Br-]. Given that the [Ag+] is 1.3x10-6 and the Ksp for AgBr is 5.2x10-23, we can rearrange the equation to solve for [Br-]. Thus, [Br-] = Ksp/[Ag+] = (5.2x10-23) / (1.3x10-6) = 4x10-17. Therefore, the Br- ion concentration is 4x10-17.
What is the solubility of BaCO3 if it has Ksp equals 6.3 10-9?
7.9 10-5
A solution has OH- 3.5 x 10-6 Based on that what must be true about this solution?
It is a basic solution.
Which silver halide is most soluble?
Solubility of the silver halides decreases down the group.The solubilities of silver halides decreases down the periodic table:AgF :Ksp=205AgCl:Ksp=1.8×10−10AgBr:Ksp=5.2×10−13AgI :Ksp=8.3×10−17
What is the solubility of AgCl in a 0.35 M solution of NaCl?
(AgCl has Ksp = 1.8 x 10-10)-5.1 x 10-10
A solution has Ag plus equals 7.7 x 10-5 and Cl- equals 2.5 x 10-3 If Ksp for AgCl is 1.8 x 10-10 what is true about this solution?
The solution is supersaturated
What is the solubility of AgCl if it has Ksp equals 3.2 10-10?
From the definition of Ksp, the product of the concentrations of Ag+ and Cl- can be no more than (1.8 X 10-10)/0.35 = 5.1 X 10-10. Since the only named material that is a source of silver ions is AgCl and the concentrations are molar, this is the maximum possible solubility of AgCl.
A solution has Cu 6.8 10 5 and Cl 1.9 10 3 If Ksp for CuCl is 1.9 10 7 what is true about this solution?
The solution is unsaturated.
A solution has Cu 4.5 10 5 and Br 3.4 10 5 If Ksp for CuBr is 5.3 10 9 what is true about this solution?
The solution is unsaturated.
A solution has Cu plus equals 6.8 x 10-5 and Cl- equals 1.9 x 10-3 If Ksp for CuCl is 1.9 x 10-7 what is true about this solution?
The solution is unsaturated.
A solution has Cu plus equals 4.5 x 10-5 and Br- equals 3.4 x 10-5 If Ksp for CuBr is 5.3 x 10-9 what is true about this solution?
The product of the ion concentrations is (in mol/L) [Cu+] * [Br-] = [4.5*10-5] * [3.4*10-5] = 1.53*10-9 This is LOWER than its solubility product Ksp 5.3*10-9, so the solution is UNDERsaturated.
What is the solubility of BaSO4 in a 0.15 M solution of Na2SO4?
(BaSO4 has Ksp = 1.1 x 10-10)-7.3 x 10-10
What is argentimetric titration?
In analytical chemistry, argentometry is a type of titration involving the silver(I) ion. Typically, it is used to determine the amount of chloride present in a sample. The sample solution is titrated against a solution of silver nitrate of known concentration. Chloride ions react with silver(I) ions to give the insoluble silver chloride:Cl− (aq) + Ag+ (aq) → AgCl (s) (Ksp = 1.70 × 10−10)
What is the molar solubility of CaC2O4 Ksp 2.3 x 10 -9 in a 0.15 M Ca2 solution?
1.5 x 10^-8
What is the solubility of AuCl in a 0.2 M solution of NaCl?
(AuCl has Ksp = 2.0 x 10-13)-1.0 x 10-12
What is the solubility of AuCl in a 0.2 M solution of NaCl AuCl has Ksp equals 2.0 x 10-13?
1.0 x 10-12
