You have a 2.0 Molar solution of an unknown acid, “HX”. Given the (25°C) thermodynamic data below, calculate Keq given that Keq = exp.[-ΔG/RT] and R is the gas constant 8.314 J/mol K
Another useful equation : ΔG = ΔH - TΔS
HX —> H+ + X- all aqueous
Enthapies of formation Entropy of formation
In KJ/mole in J/mole K
HX 200 300
H+ 10 0
X- 250 175
Do you have to multiply the enthaply and entropy values by 2 because it is a 2.0 molar solution when calculating delta G and K eq? If you do, would the answer be incorrect ?
You have a 2.0 Molar solution of an unknown acid, “HX”. Given the (25°C) thermodynamic data...
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Please help with solving Question 1 (A-C) Thank you! Unless otherwise specified in the problem, you may assume that all solutions are at 25°C. 1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. Carbonic acid: Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857...