Chemistry, 25.09.2019 23:00 patrickfutrell2537

Solve an equilibrium problem (using an ice table) to calculate the ph of each solution: part a a solution that is 0.195 m in hc2h3o2 and 0.125 m in kc2h3o2

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To determine the pH of a solution which has 0.195 M hc2h3o2 and 0.125 M kc2h3o2, we use the ICE table and the acid dissociation constant of hc2h3o2 to determine the concentration of the hydrogen ion present at equilibrium. We do as follows:

HC2H3OO = H+ + C2H3OO-
KC2H3OO = K+ + C2H3OO-

Therefore, the only source of hydrogen ion would be the acid. We use the ICE table,
HC2H3OO H+ C2H3OO-
I 0.195 0 0.125
C -x +x +x

E 0.195-x x 0.125 + x

Ka = 1.8*10^-5 = (0.125 + x) (x) / 0.195 -x
x = 2.81x10^-5 M = [H+]

pH = - log [H+]
pH = -log 2.81x10^-5
pH = 4.55

Therefore, the pH of the resulting solution would be 4.55.

Answer from: Quest

10.063g / 10.00 ml = 1.0063 g/ml which rounds off to 4 sig figs as: 1.006 g/ml

Answer from: Quest

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.

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