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please check my answers for 1 and 2 and then answer #3 in detail A 10.0...

please check my answers for 1 and 2 and then answer #3 in detail

  1. A 10.0 mL sample of Ba(OH)2 at 0°C is titrated with 0.230 M HCl, and 5.22 mL of the acid are used to reach the yellow endpoint.
  1. Calculate the concentration of OH⁻ in the 10.0 mL sample of Ba(OH)2 at 0°C.
    1. .12 M
  2. Calculate the molar solubility (S) and from that the Ksp of Ba(OH)2 at 0°C.
    1. 8.64*10^-4
  3. Calculate the ∆G° for the dissolution of Ba(OH)2 from the Ksp calculated in part b, at 0°C.

16010.47

2. A second 10.0 mL sample of Ba(OH)2 is obtained at a temperature of 50°C. This solution required 47.99 mL of 0.230 M HCl to reach the yellow endpoint.

  1. Calculate the concentration of OH⁻ in the 10.0 mL sample of Ba(OH)2 at 50°C.

1.1

  1. Calculate the molar solubility (S) and from that the Ksp of Ba(OH)2 at 50°C.
    1. .6655
  2. Calculate ∆G° for the dissolution of Ba(OH)2 from the Ksp calculated in part b, at 50°C.

1093.54

3. Using the values of ∆G° at 0°C and 50°C, calculate ∆H° and ∆S° for this reaction.

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