Calculating Ku [rom solubility data
1. The solubility of silver bromide is found to be 8.8 x 10-7 mol/L at 250C. Calculate the Ksp for silver bromide.
2. The solubility of iron (Il) hydroxide is 1.4 x 10-3 g/L at 298 K. What is its Ksp?
3. The solubility of copper (Il) bromide is 2.0 x 10-4 mol/L at 25 °C. Calculate the Ksp at 25 °C.
4. The solubility of strontium sulfate is 5.83 x 10 mol/L at 25°C. Calculate the 1<sp at 25°C.
5. The solubility of magnesium hydroxide is 1.5 x 10-4 mol in 100 mL at 18°C. Calculate the Ksp.
6. The solubility of silver sulfide is 1.3 x 10-3 mol in 50 mL, at 20 °C, what is Ksp?
7. The solubility of barium fluoride is 2.2 x 10-2 mol/L at 25 0 C. Calculate the Ksp at 25 °C.
8. The solubility of lithium carbonate at 15 0 C is 1.5 g/ 100 mL of water. Calculate the Ksp of lithium carbonate at 15 °C.
1. To calculate the Ksp for silver bromide, we need to set up the equilibrium expression and solve for Ksp.
AgBr (s) ⇌ Ag+ (aq) + Br- (aq)
Ksp = [Ag+][Br-]
Since the solubility of silver bromide is given as 8.8 x 10^-7 mol/L, we can assume that the concentration of Ag+ and Br- ions is also 8.8 x 10^-7 mol/L.
Therefore, Ksp = (8.8 x 10^-7)(8.8 x 10^-7) = 7.74 x 10^-13
2. To calculate the Ksp for iron (II) hydroxide, we need to determine the concentration of Fe2+ and OH- ions using the solubility information.
Fe(OH)2 (s) ⇌ Fe2+ (aq) + 2OH- (aq)
The solubility is given as 1.4 x 10^-3 g/L, so we need to convert this to mol/L using the molar mass of Fe(OH)2. The molar mass of Fe(OH)2 is 89.85 g/mol.
1.4 x 10^-3 g/L * (1 mol/89.85 g) = 1.56 x 10^-5 mol/L
Since there is a 1:1 ratio between Fe2+ and OH- ions, the concentration of OH- ions is also 1.56 x 10^-5 mol/L.
Therefore, Ksp = (1.56 x 10^-5)(1.56 x 10^-5) = 2.43 x 10^-10
3. The solubility of copper (II) bromide is given as 2.0 x 10^-4 mol/L. Since copper (II) bromide is an ionic compound, it dissociates into ions in water.
CuBr2 (s) ⇌ Cu2+ (aq) + 2Br- (aq)
The concentration of Cu2+ ions is given as 2.0 x 10^-4 mol/L, and the concentration of Br- ions is 2 times that, so it is 4.0 x 10^-4 mol/L.
Therefore, Ksp = (2.0 x 10^-4)(4.0 x 10^-4) = 8.0 x 10^-8
4. The solubility of strontium sulfate is given as 5.83 x 10^-3 mol/L. Since strontium sulfate is an ionic compound, it dissociates into ions in water.
SrSO4 (s) ⇌ Sr2+ (aq) + SO4^2- (aq)
The concentration of Sr2+ ions is given as 5.83 x 10^-3 mol/L, and the concentration of SO4^2- ions is also 5.83 x 10^-3 mol/L.
Therefore, Ksp = (5.83 x 10^-3)(5.83 x 10^-3) = 3.40 x 10^-5
5. The solubility of magnesium hydroxide is given as 1.5 x 10^-4 mol in 100 mL. We need to convert this to mol/L by dividing by the volume in liters.
1.5 x 10^-4 mol / (100 mL * 0.001 L/mL) = 1.5 x 10^-3 mol/L
Since magnesium hydroxide dissociates into Mg2+ and 2OH- ions, the concentration of Mg2+ ions is 1.5 x 10^-3 mol/L, and the concentration of OH- ions is 2 times that, so it is 3.0 x 10^-3 mol/L.
Therefore, Ksp = (1.5 x 10^-3)(3.0 x 10^-3)(3.0 x 10^-3) = 1.35 x 10^-8
6. The solubility of silver sulfide is given as 1.3 x 10^-3 mol in 50 mL. We need to convert this to mol/L by dividing by the volume in liters.
1.3 x 10^-3 mol / (50 mL * 0.001 L/mL) = 2.6 x 10^-2 mol/L
Since silver sulfide dissociates into Ag+ and S2- ions, the concentration of Ag+ ions is 2.6 x 10^-2 mol/L, and the concentration of S2- ions is also 2.6 x 10^-2 mol/L.
Therefore, Ksp = (2.6 x 10^-2)(2.6 x 10^-2) = 6.76 x 10^-4
7. The solubility of barium fluoride is given as 2.2 x 10^-2 mol/L. Since barium fluoride is an ionic compound, it dissociates into ions in water.
BaF2 (s) ⇌ Ba2+ (aq) + 2F- (aq)
The concentration of Ba2+ ions is given as 2.2 x 10^-2 mol/L, and the concentration of F- ions is 2 times that, so it is 4.4 x 10^-2 mol/L.
Therefore, Ksp = (2.2 x 10^-2)(4.4 x 10^-2) = 9.68 x 10^-4
8. The solubility of lithium carbonate is given as 1.5 g/100 mL. We need to convert this to mol/L by dividing by the molar mass of lithium carbonate (73.89 g/mol) and the volume in liters.
1.5 g / (100 mL * 0.001 L/mL * 73.89 g/mol) = 2.03 x 10^-3 mol/L
Since lithium carbonate dissociates into Li+ and CO3^2- ions, the concentration of Li+ ions is 2.03 x 10^-3 mol/L, and the concentration of CO3^2- ions is also 2.03 x 10^-3 mol/L.
Therefore, Ksp = (2.03 x 10^-3)(2.03 x 10^-3) = 4.12 x 10^-6
what is the correct answer?
Apologies for the previous response, here are the correct answers for each question:
1. The solubility of silver bromide is 8.8 x 10^-7 mol/L. Since it dissociates into Ag+ and Br- ions in water, the concentration of Ag+ and Br- ions is also 8.8 x 10^-7 mol/L.
Therefore, the Ksp for silver bromide is (8.8 x 10^-7)(8.8 x 10^-7) = 7.74 x 10^-14.
2. The solubility of iron (II) hydroxide is 1.4 x 10^-3 g/L. To determine the solubility in mol/L, we divide by the molar mass of Fe(OH)2 (89.85 g/mol).
(1.4 x 10^-3 g/L) / (89.85 g/mol) = 1.56 x 10^-5 mol/L.
Since the ratio of Fe2+ to OH- ions is 1:2, the concentration of OH- ions is twice the concentration of Fe2+ ions, at 2(1.56 x 10^-5) = 3.12 x 10^-5 mol/L.
Therefore, the Ksp for iron (II) hydroxide is (1.56 x 10^-5)(3.12 x 10^-5)^2 = 1.54 x 10^-14.
3. The solubility of copper (II) bromide is 2.0 x 10^-4 mol/L. Since it dissociates into Cu2+ and 2Br- ions, the concentration of Cu2+ ions is 2.0 x 10^-4 mol/L, and the concentration of Br- ions is 2 times that, at 4.0 x 10^-4 mol/L.
Therefore, the Ksp for copper (II) bromide is (2.0 x 10^-4)(4.0 x 10^-4)^2 = 3.2 x 10^-11.
4. The solubility of strontium sulfate is 5.83 x 10^-3 mol/L. Since it dissociates into Sr2+ and SO4^2- ions, the concentration of Sr2+ ions is 5.83 x 10^-3 mol/L, and the concentration of SO4^2- ions is also 5.83 x 10^-3 mol/L.
Therefore, the Ksp for strontium sulfate is (5.83 x 10^-3)^2 = 3.39 x 10^-5.
5. The solubility of magnesium hydroxide is 1.5 x 10^-4 mol in 100 mL. We convert this to mol/L by dividing by the volume in liters: (1.5 x 10^-4 mol) / (0.1 L) = 1.5 x 10^-3 mol/L.
Since magnesium hydroxide dissociates into Mg2+ and 2OH- ions, the concentration of Mg2+ ions is 1.5 x 10^-3 mol/L, and the concentration of OH- ions is twice that at 3.0 x 10^-3 mol/L.
Therefore, the Ksp for magnesium hydroxide is (1.5 x 10^-3)(3.0 x 10^-3)^2 = 1.35 x 10^-8.
6. The solubility of silver sulfide is 1.3 x 10^-3 mol in 50 mL. We convert this to mol/L by dividing by the volume in liters: (1.3 x 10^-3 mol) / (0.05 L) = 2.6 x 10^-2 mol/L.
Since silver sulfide dissociates into Ag+ and S2- ions, the concentration of Ag+ ions is 2.6 x 10^-2 mol/L, and the concentration of S2- ions is also 2.6 x 10^-2 mol/L.
Therefore, the Ksp for silver sulfide is (2.6 x 10^-2)^2 = 6.76 x 10^-4.
7. The solubility of barium fluoride is 2.2 x 10^-2 mol/L. Since it dissociates into Ba2+ and 2F- ions, the concentration of Ba2+ ions is 2.2 x 10^-2 mol/L, and the concentration of F- ions is twice that at 4.4 x 10^-2 mol/L.
Therefore, the Ksp for barium fluoride is (2.2 x 10^-2)(4.4 x 10^-2)^2 = 4.83 x 10^-5.
8. The solubility of lithium carbonate is 1.5 g/100 mL. We convert this to mol/L by dividing by the molar mass of lithium carbonate (73.89 g/mol) and the volume in liters: (1.5 g) / (100 mL * 0.001 L/mL * 73.89 g/mol) = 2.03 x 10^-3 mol/L.
Since lithium carbonate dissociates into Li+ and CO3^2- ions, the concentration of Li+ ions is 2.03 x 10^-3 mol/L, and the concentration of CO3^2- ions is also 2.03 x 10^-3 mol/L.
Therefore, the Ksp for lithium carbonate is (2.03 x 10^-3)(2.03 x 10^-3) = 4.12 x 10^-6.
are you sure these answers are correct?
Apologies for the confusion in my previous response. Here are the correct answers for each question:
1. The solubility of silver bromide is 8.8 x 10^-7 mol/L. Since silver bromide dissociates into Ag+ and Br- ions, the concentration of Ag+ and Br- ions is also 8.8 x 10^-7 mol/L.
Therefore, the Ksp for silver bromide is (8.8 x 10^-7)(8.8 x 10^-7) = 7.7 x 10^-14.
2. The solubility of iron (II) hydroxide is 1.4 x 10^-3 g/L. To convert this to mol/L, we need to divide by the molar mass of Fe(OH)2 (89.85 g/mol).
(1.4 x 10^-3 g/L) / (89.85 g/mol) = 1.56 x 10^-5 mol/L
Since there is a 1:2 stoichiometric ratio between Fe2+ and OH- ions, the concentration of OH- ions is twice the concentration of Fe2+ ions: 2(1.56 x 10^-5) = 3.12 x 10^-5 mol/L.
Therefore, the Ksp for iron (II) hydroxide is (1.56 x 10^-5)(3.12 x 10^-5)^2 = 1.54 x 10^-14.
3. The solubility of copper (II) bromide is 2.0 x 10^-4 mol/L. Since copper (II) bromide dissociates into Cu2+ and 2Br- ions, the concentration of Cu2+ ions is 2.0 x 10^-4 mol/L, and the concentration of Br- ions is 2 times that, at 4.0 x 10^-4 mol/L.
Therefore, the Ksp for copper (II) bromide is (2.0 x 10^-4)(4.0 x 10^-4)^2 = 3.2 x 10^-11.
4. The solubility of strontium sulfate is 5.83 x 10^-3 mol/L. Since strontium sulfate dissociates into Sr2+ and SO4^2- ions, the concentration of Sr2+ ions is 5.83 x 10^-3 mol/L, and the concentration of SO4^2- ions is also 5.83 x 10^-3 mol/L.
Therefore, the Ksp for strontium sulfate is (5.83 x 10^-3)(5.83 x 10^-3) = 3.39 x 10^-5.
5. The solubility of magnesium hydroxide is 1.5 x 10^-4 mol in 100 mL. We convert this to mol/L by dividing by the volume in liters: (1.5 x 10^-4 mol) / (0.1 L) = 1.5 x 10^-3 mol/L.
Since magnesium hydroxide dissociates into Mg2+ and 2OH- ions, the concentration of Mg2+ ions is 1.5 x 10^-3 mol/L, and the concentration of OH- ions is twice that, at 3.0 x 10^-3 mol/L.
Therefore, the Ksp for magnesium hydroxide is (1.5 x 10^-3)(3.0 x 10^-3)^2 = 1.35 x 10^-8.
6. The solubility of silver sulfide is 1.3 x 10^-3 mol in 50 mL. We convert this to mol/L by dividing by the volume in liters: (1.3 x 10^-3 mol) / (0.05 L) = 2.6 x 10^-2 mol/L.
Since silver sulfide dissociates into Ag+ and S2- ions, the concentration of Ag+ ions is 2.6 x 10^-2 mol/L, and the concentration of S2- ions is also 2.6 x 10^-2 mol/L.
Therefore, the Ksp for silver sulfide is (2.6 x 10^-2)(2.6 x 10^-2) = 6.76 x 10^-4.
7. The solubility of barium fluoride is 2.2 x 10^-2 mol/L. Since barium fluoride dissociates into Ba2+ and 2F- ions, the concentration of Ba2+ ions is 2.2 x 10^-2 mol/L, and the concentration of F- ions is twice that, at 4.4 x 10^-2 mol/L.
Therefore, the Ksp for barium fluoride is (2.2 x 10^-2)(4.4 x 10^-2)^2 = 4.83 x 10^-5.
8. The solubility of lithium carbonate is 1.5 g/100 mL. We convert this to mol/L by dividing by the molar mass of lithium carbonate (73.89 g/mol) and the volume in liters: (1.5 g) / (100 mL * 0.001 L/mL * 73.89 g/mol) = 2.03 x 10^-3 mol/L.
Since lithium carbonate dissociates into Li+ and CO3^2- ions, the concentration of Li+ ions is 2.03 x 10^-3 mol/L, and the concentration of CO3^2- ions is also 2.03 x
To calculate the Ksp (solubility product constant) for a given solute, you need to determine the concentration of the ions in the solution based on the solubility data provided. The Ksp is the product of the concentrations of the ions raised to the power of their stoichiometric coefficients.
Here's how you can calculate the Ksp for each of the given scenarios:
1. The solubility of silver bromide is 8.8 x 10^-7 mol/L at 25°C.
- The formula for silver bromide is AgBr, which dissociates into Ag+ and Br- ions.
- Since the stoichiometry is 1:1, the concentration of Ag+ and Br- ions will be the same.
- Therefore, the concentration of Ag+ and Br- ions is 8.8 x 10^-7 mol/L.
- The Ksp for AgBr is the product of the concentrations of Ag+ and Br- ions: Ksp = (8.8 x 10^-7)^2.
2. The solubility of iron (II) hydroxide is 1.4 x 10^-3 g/L at 298 K.
- The formula for iron (II) hydroxide is Fe(OH)2, which dissociates into Fe2+ and 2OH- ions.
- The molar mass of Fe(OH)2 is 89.91 g/mol, so the solubility is (1.4 x 10^-3 g/L) / (89.91 g/mol).
- Calculate the concentration of Fe2+ and OH- ions based on the solubility you obtained.
- The Ksp for Fe(OH)2 is the product of the concentrations of Fe2+ and OH- ions.
3. The solubility of copper (II) bromide is 2.0 x 10^-4 mol/L at 25 °C.
- The formula for copper (II) bromide is CuBr2, which dissociates into Cu2+ and 2Br- ions.
- The concentration of Cu2+ ions is 2.0 x 10^-4 mol/L, and the concentration of Br- ions is twice that.
- The Ksp for CuBr2 is the product of the concentrations of Cu2+ and Br- ions.
4. The solubility of strontium sulfate is 5.83 x 10 mol/L at 25°C.
- The formula for strontium sulfate is SrSO4, which dissociates into Sr2+ and SO4^2- ions.
- The concentration of Sr2+ ions is 5.83 x 10^ mol/L, and the concentration of SO4^2- ions is the same.
- The Ksp for SrSO4 is the product of the concentrations of Sr2+ and SO4^2- ions.
5. The solubility of magnesium hydroxide is 1.5 x 10^-4 mol in 100 mL at 18°C.
- The formula for magnesium hydroxide is Mg(OH)2, which dissociates into Mg2+ and 2OH- ions.
- Calculate the concentration of Mg2+ and OH- ions based on the solubility you obtained.
- The Ksp for Mg(OH)2 is the product of the concentrations of Mg2+ and OH- ions.
6. The solubility of silver sulfide is 1.3 x 10^-3 mol in 50 mL at 20 °C.
- The formula for silver sulfide is Ag2S, which dissociates into 2Ag+ and S^2- ions.
- Calculate the concentration of Ag+ and S^2- ions based on the solubility you obtained.
- The Ksp for Ag2S is the product of the concentrations of Ag+ and S^2- ions.
7. The solubility of barium fluoride is 2.2 x 10^-2 mol/L at 25 °C.
- The formula for barium fluoride is BaF2, which dissociates into Ba^2+ and 2F- ions.
- Calculate the concentration of Ba^2+ and F- ions based on the solubility you obtained.
- The Ksp for BaF2 is the product of the concentrations of Ba^2+ and F- ions.
8. The solubility of lithium carbonate at 15 °C is 1.5 g/100 mL of water.
- The formula for lithium carbonate is Li2CO3, which dissociates into 2Li+ and CO3^2- ions.
- Calculate the concentration of Li+ and CO3^2- ions based on the solubility you obtained.
- The Ksp for Li2CO3 is the product of the concentrations of Li+ and CO3^2- ions.
Note: Make sure to convert units as necessary and use the correct stoichiometric coefficients when calculating the concentrations.