If 200 ml of aqueous 0.862 m hcl is mixed with 20. ml of aqueous 0.431 m ba(oh)2 in a constant-pressure calorimeter of negligible heat capacity, the initial temperature of both solutions is the same at 20.48ºc. the neutralization reaction h+(aq) + oh–(aq) → h2o(l) has a δhº = –56.2 kj/mol.

what is the final temperature of the mixed solution? (assume all solutions have a density of 1.00 g/cm3 and a specific heat capacity of 4.184 j/g•ºc)

The final temperature of the mixed solution is 26.26 °C.

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the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.