use the following data, as appropriate, to estimate the molarity of a saturated aqueous solution of Sr(IO3)2.
Molarity of a saturated aqueous solution of Sr(IO3)2
Sr(IO3)2(s)
delt h kJ/mol=-1019.2
delta G kJ/mol=-855.1
delta S= 234 J mol-1K-1
Sr^2+(aq)
delta h= -545.8 kJ/mol
delta G= -599.5
delta s= -32.6 j /mol*k
IO3^-(aq)
delta h= -221.3 kj/mol
delta g= -128.0 kj/mol
delta s= 118.4 J/mol*k
To estimate the molarity of a saturated aqueous solution of Sr(IO3)2, we need to use the given data and apply the appropriate equations.
First, let's find the molar entropy change, delta Sprime, for the dissolution of Sr(IO3)2 using the entropy of formation for the reactants and products:
delta Sprime = nSr^2+(aq) * delta S(Sr^2+) + 2 * nIO3^-(aq) * delta S(IO3^-)
Plugging in the values:
delta Sprime = (1 * (-32.6 J/mol*K)) + (2 * 118.4 J/mol*K)
delta Sprime = -32.6 J/mol*K + 236.8 J/mol*K
delta Sprime = 204.2 J/mol*K
Now we can calculate the standard free energy change, delta G°, for the dissolution of Sr(IO3)2:
delta G° = -RTln(Ksp)
Where:
R = gas constant (8.314 J/mol*K)
T = temperature in Kelvin (assumed to be 298 K for standard conditions)
Ksp = solubility product constant (unknown)
Since we don't have the value for Ksp, we can use the given data to calculate it:
delta G° = delta H° - T * delta Sprime
Plugging in the values:
-855.1 kJ/mol = (-1019.2 kJ/mol) - (298 K * (204.2 J/mol*K / 1000))
-855.1 kJ/mol = -1019.2 kJ/mol - 61.5976 kJ/mol
-855.1 kJ/mol = -1080.7976 kJ/mol
Now, we can solve for Ksp:
Ksp = e^(delta G° / (R * T))
Plugging in the values:
Ksp = e^((-1080.7976 kJ/mol) / (8.314 J/mol*K * 298 K))
Ksp = e^(-4.06759)
Ksp ≈ 0.017
Finally, we can calculate the molarity (M) of the saturated aqueous solution of Sr(IO3)2 using the molar solubility (s):
Ksp = [Sr^2+][IO3^-]^2
M = s = [Sr^2+] ≈ [IO3^-]
Therefore, the molarity of a saturated aqueous solution of Sr(IO3)2 is approximately 0.017 M.