A100.0 ml sample of 0.10 m ca(oh)2 is titrated with 0.10 m hbr. determine the ph of the solution after the addition of 300.0 ml hbr. a) 2.62 b)2.00 c) 1.7 d) 12.52

Answer : The correct option is, (C) 1.7

Explanation :

First we have to calculate the moles of and .

The balanced chemical reaction will be:

0.01 mole of dissociate to give 0.01 mole of ion and 0.02 mole of ion

and

0.03 mole of dissociate to give 0.03 mole of ion and 0.03 mole of ion

That means,

0.02 moles of ion  neutralize by 0.02 moles of ion.

The excess moles of ion = 0.03 - 0.02 = 0.01 mole

Total volume of solution = 100 + 300 = 400 ml = 0.4 L

Now we have to calculate the concentration of ion.

Now we have to calculate the pH of the solution.

Therefore, the pH of the solution is, 1.7

answer: the figure is attached herewith.

step-by-step explanation:   we are given to sketch a unit circle and label the terminal points corresponding to

in the attached figure, we have drawn a unit circle, with centre at o(0,0) and radius 1 unit. we have labelled the points a, b, c, d and e corresponding to the angles below

∠aox = 60°,

∠box = 120°,

∠cox = 180°,

∠dox = 240°,

∠eox = 300°.

and the coordinates are a(0.5,1), b(-0.5,1), c(-1,0), d(-0.5,-1) and e(0.5,-1).

thus, the answer is complete.

pure substance: iron,copper

impure substance: water,charcoal