Which of the following is the pH of a 0.0295 M NaOH solution? 3.39 times 10^-13

Question

Which of the following is the pH of a 0.0295 M NaOH solution? 3.39 times 10^-13 7.00 12.47 1.53 None of the above A reaction is found to have a change in enthalpy of -8.67 kJ/mol and a change in entropy of 29.87 J/mol. The reaction is: Spontaneous at all T Nonspontaneous at all T Spontaneous at high T and nonspontaneous at low T Spontaneous at low T and nonspontaneous at high T Cannot be determined with the information given. Acetone has a freezing point of -139 degree C and a molar entropy of fusion is 32.3 J/molK. What is the enthalpy of fusion for acetone?? -4489 J/mol -4.303 J/mol 4.149 J/mol 4328 J/mol 0.241 J/mol All of the following are strong acids except HF HCl HI HBr They are all strong acids In an equilibrium constant expression: The pressures of pure liquids are included The concentrations of aqueous solutions are included The concentration of solids are included All of the above None of the above

Explanation / Answer

Q11.

pH of NaOH

[OH-] = [NaOH] = 0.0295 M

so

pOH = -log(OH) = -log(0.0295 ) = 1.53017

pH = 14-pOH = 14-1.53017 = 12.46

Q12

dHrn = -8.67 kJ/mol

dS = 29.87 J/mol

so..

d G = dH - T*dS

this will be always negative, so always spontaneous

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