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The minimum volume of water required to dissolve 0.1g lead (II) chloride to get a saturated solution (Ksp of PbCl2 = 3.2 x 10-8; atomic mass of Pb= 207 u) is:
- a)018 L
- b)0.36 L
- c)17.98 L
- d)1.798 L
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
The minimum volume of water required to dissolve 0.1g lead (II) chlori...
Ksp of PbCl2 is 3.2 × 10-8
PbCl2 is 3.2 × 10−8
Pbcl2(s) ⇌ Pb2+(aq) + 2Cl−(aq)
t = 0 1 0 0.
At equilibrium 1 – S S 2S.
Ksp = [S] [2S]2
3.2 × 10−8 = 4s3
S3 = 0.8 × 10−8
S3 = 8 × 10−9
S = 2 × 10−3
Solubility = W/V
∴ Solubility of PbCl2 in gL−1 = 2 × 10−3 × 278
= 556 × 10−3gL−1
0.556 gL−1
x = 0.1/0.556
= 0.18L
PbCl2 is 3.2 × 10−8
Pbcl2(s) ⇌ Pb2+(aq) + 2Cl−(aq)
t = 0 1 0 0.
At equilibrium 1 – S S 2S.
Ksp = [S] [2S]2
3.2 × 10−8 = 4s3
S3 = 0.8 × 10−8
S3 = 8 × 10−9
S = 2 × 10−3
Solubility = W/V
∴ Solubility of PbCl2 in gL−1 = 2 × 10−3 × 278
= 556 × 10−3gL−1
0.556 gL−1
0.556/0.1 = 1/x
x = 0.1/0.556
= 0.18L
Most Upvoted Answer
The minimum volume of water required to dissolve 0.1g lead (II) chlori...
To determine the minimum volume of water required to dissolve 0.1g of lead (II) chloride (PbCl2) and obtain a saturated solution, we can use the solubility product constant (Ksp) of PbCl2.
Given data:
Mass of PbCl2 = 0.1g
Ksp of PbCl2 = 3.2 x 10^-8
Atomic mass of Pb = 207 u
To solve this problem, we need to follow these steps:
1. Calculate the number of moles of PbCl2:
Number of moles = Mass / Molar mass
Number of moles of PbCl2 = 0.1g / (207g/mol + 2 x 35.5g/mol) = 0.1g / 278g/mol = 0.000359 moles
2. Write the balanced chemical equation for the dissociation of PbCl2:
PbCl2 (s) ⇌ Pb2+ (aq) + 2Cl- (aq)
3. Use the stoichiometry of the balanced equation to determine the concentration of ions in the saturated solution:
Pb2+ concentration = 0.000359 moles / V (L)
Cl- concentration = 2 x 0.000359 moles / V (L)
4. Apply the solubility product constant expression for PbCl2:
Ksp = [Pb2+] x [Cl-]^2
Substituting the concentrations from step 3:
3.2 x 10^-8 = (0.000359 / V) x (2 x 0.000359 / V)^2
Simplifying the equation:
3.2 x 10^-8 = 4 x (0.000359 / V)^3
(0.000359 / V)^3 = (3.2 x 10^-8) / 4
(0.000359 / V)^3 = 8 x 10^-9
Taking the cube root of both sides:
0.000359 / V = 2 x 10^-3
V = 0.000359 / (2 x 10^-3)
V = 0.0001795 L
5. Convert the volume from liters to milliliters:
V = 0.0001795 L x 1000 mL/L = 0.1795 mL
Therefore, the minimum volume of water required to dissolve 0.1g of PbCl2 and obtain a saturated solution is approximately 0.1795 mL, which is equivalent to 0.018 L (option A).
Given data:
Mass of PbCl2 = 0.1g
Ksp of PbCl2 = 3.2 x 10^-8
Atomic mass of Pb = 207 u
To solve this problem, we need to follow these steps:
1. Calculate the number of moles of PbCl2:
Number of moles = Mass / Molar mass
Number of moles of PbCl2 = 0.1g / (207g/mol + 2 x 35.5g/mol) = 0.1g / 278g/mol = 0.000359 moles
2. Write the balanced chemical equation for the dissociation of PbCl2:
PbCl2 (s) ⇌ Pb2+ (aq) + 2Cl- (aq)
3. Use the stoichiometry of the balanced equation to determine the concentration of ions in the saturated solution:
Pb2+ concentration = 0.000359 moles / V (L)
Cl- concentration = 2 x 0.000359 moles / V (L)
4. Apply the solubility product constant expression for PbCl2:
Ksp = [Pb2+] x [Cl-]^2
Substituting the concentrations from step 3:
3.2 x 10^-8 = (0.000359 / V) x (2 x 0.000359 / V)^2
Simplifying the equation:
3.2 x 10^-8 = 4 x (0.000359 / V)^3
(0.000359 / V)^3 = (3.2 x 10^-8) / 4
(0.000359 / V)^3 = 8 x 10^-9
Taking the cube root of both sides:
0.000359 / V = 2 x 10^-3
V = 0.000359 / (2 x 10^-3)
V = 0.0001795 L
5. Convert the volume from liters to milliliters:
V = 0.0001795 L x 1000 mL/L = 0.1795 mL
Therefore, the minimum volume of water required to dissolve 0.1g of PbCl2 and obtain a saturated solution is approximately 0.1795 mL, which is equivalent to 0.018 L (option A).
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The minimum volume of water required to dissolve 0.1g lead (II) chloride to get a saturated solution(Ksp of PbCl2 = 3.2 x 10-8; atomic mass of Pb= 207 u) is:a)018 Lb)0.36 Lc)17.98 Ld)1.798 LCorrect answer is option 'A'. Can you explain this answer?
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