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Travka [436]
3 years ago
12

The solubility of lead (ii) chloride (pbcl2) is 1.6 ⋅ 10-2 m. what is the ksp of pbcl2? the solubility of lead (ii) chloride (pb

cl2) is 1.6 10-2 m. what is the ksp of pbcl2? 3.1 ⋅ 10-7 5.0 ⋅ 10-4 1.6 ⋅ 10-5 1.6 ⋅ 10-2 4.1 ⋅ 10-6
Chemistry
2 answers:
Yakvenalex [24]3 years ago
8 0
According to the equilibrium equation for this reaction:

PbCl2(s)  ↔ Pb2+(aq)   +  2Cl-(aq)

So when Ksp is the solubility product constant for a solid substance when it

dissolved in the solution. and measure how a solute dissolves in the solution 

So, Ksp expression = [Pb2+] [Cl-]^2

and when the solubility is the maximum quantity of solute which can dissolve in a certain solute.
 
So, we assume the solubility = X 

∴[Pb2+] = X = 1.6 x 10^-2 M

[Cl-] = 2X = 2 * 1.6 x 10^-2 = 0.032 M

by substitution:

∴ Ksp = (1.6 x 10^-2) * (0.032)^2

           = 1.64 x 10^-5  
DedPeter [7]3 years ago
8 0

Answer:The Solubility product of PbCl_2 is 1.63\times 10^{-5}.

Explanation;

Solubility of PbCl_2,S=1.6\times 10^{-2} M

                         PbCl_2\rightleftharpoons Pb^{2+}+2Cl^-

                                                 S        2S

The expression of K_{sp} is given as:

K_{sp}=S\times (2S)^2=4S^3

K_{sp}=4\times (1.6\times 10^{-2})^3=1.63\times 10^{-5}

The Solubility product of PbCl_2 is 1.63\times 10^{-5}.

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(b)ΔS_{sys}  = 2.881 J/K; ΔS_{sur}  = 0 ; total change in entropy = 2.881 J/K

(c) ΔS_{sys}  = 0 ; ΔS_{sur}  = 0 ; total change in entropy = 0

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In the given problem, we need to calculate the change in the entropy of the system and also the change in the entropy of the surroundings, and the resulting total change in entropy, when a sample of nitrogen gas of mass 14 g at 298 K and 1.00 bar doubles its volume. We have the following variable:

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1 ) Δs ( entropy change for hot block ) = - Q / th  ( -ve shows heat lost to cold block )

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<u>1) To show that heat flows spontaneously from high temperature to low temperature </u>

example :

Pick two(2) solid metal blocks with varying temperatures ( i.e. one solid block is hot and the other solid block is cold )

Place both blocks for time (t ) in an insulated system to reduce heat loss or gain to or from the environment

Check the temperature of both blocks after time ( t ) it will be observed that both blocks will have same temperature after time t ( first law of thermodynamics )

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Δs ( entropy change for cold block ) = Q / tc

∴ Total Δs = ΔSc + ΔSh

                 = Q/tc - Q/th

<u>2) Entropy change for Decomposition of mercuric oxide </u>

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there is transition from solid to liquid and the melting point of mercury ( the point at which reaction will take place ) = 500⁰C

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Δh of reaction = 181.6 KJ

Temp = 500 + 273 = 773 k

hence ΔSdecomposition = Δh / Temp = ( 181.6 * 10^3 / 773 ) = 234.928 J/k

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