If 0.500 mol of each of the following solutes is dissolved in 2.0 l of water, which will cause the greatest increase in the boiling point of the solution? a. nacl b. ki c. co2 d. na2so4

D.

Explanation:

= change in boiling point

i= vant hoff factor = no of ions produced on complete dissociation

= boiling point constant

m= molality = =same for all solutes

1. For NaCl:

i=2

2. For ,

i=2

3. , i= 1 as it does not dissociate

4. For ,

i=3

Thus elevation in boiling point will be highest in solution.

the grams   of   barium that   are in   2.3 x 10^23   atoms of barium   is   52.4 g (answer c)

    calculation

mass = moles   of ba   x molar   mass of ba

  molar mass of ba from periodic table=   137.3 g/mol

  use the   avogadro's law   constant   to   calculate the moles of barium

  that   is     1 mole =   6.02   x 10^23 atoms

                    ? moles = 2.3 x 10^23   atoms

by cross   multiplication

=(1 mole   x 2.3x 10^23 atoms)   / 6.02   x10^23 atoms)=   0.382   moles

mass   is therefore = 137.3   g/mol x 0.382 mol = 52.4 ( answer c)

explanation:

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