which of the following concentration measures willchange in value as the tempera

Question

which of the following concentration measures willchange in value as the temperature of a solution change? mass percent mole fraction molality molarity or all of these please explain thank you 2)question 2 which of the following favors thesolubility of an ionic solid in a liquid solvent a large magnitude of the solvation energy of the ions a small magnitude of the lattice energy of the solute a large polarity of the solvent all of these or none of these please explain thankyou 3) in a 0.1 molar solution of Nacl in water which one of thefollowing will be closest to 0.1? mole fraction of Nacl or mass fraction, mass percent ofnacl or molality or all of these are about 0.1 pleaseexplain thank you which of the following concentration measures willchange in value as the temperature of a solution change? mass percent mole fraction molality molarity or all of these please explain thank you 2)question 2 which of the following favors thesolubility of an ionic solid in a liquid solvent a large magnitude of the solvation energy of the ions a small magnitude of the lattice energy of the solute a large polarity of the solvent all of these or none of these please explain thankyou 3) in a 0.1 molar solution of Nacl in water which one of thefollowing will be closest to 0.1? mole fraction of Nacl or mass fraction, mass percent ofnacl or molality or all of these are about 0.1 pleaseexplain thank you

Explanation / Answer

1) molarity, because this is concentration per volume. Volumeusually increases with temperature mass percent is mass/total mass, total mass stays the same mole fract is mole/total moles; moles is contant molality is moles/ mass solvent 2) all, large magnitude of solvation energy => favorable change inenergy potentially small magnitude of the lattice energy means the solid form is notfavored polar solvents can dissolve ionic compounds readily by stabilizingthe ions with polar-ion interactions 3) molality: 0.1 M = 0.1 mol/ L solution 1L solution ~ 1 kg water b/c water has density 1 kg/1L So 0.1 mol in 1L solution is about 0.1 mol in 1kg water molality = 0.1 mol/1kg water= 0.1 molal 0.1 mol NaCl in 1 kg water => 1 kg water is 1kg *(1000g/1kg) *(1 mol / 18g) = 55.56 mol water Thus mol frac of NaCl: 0.1 mol /(55.56 + 0.1) = 0.00179, so molfraction is not true 0.1 mol NaCl has mass of 0.1 mol *(58.4 g /mol) = 5.84 g NaCl      in 1 kg water mass percent NaCl: 5.84/(1000 + 5.84) = 0.055 = 5.5%, so not0.1

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