What is the molality of a solution consisting of 2.66 mL of carbon tetrachloride

Question

What is the molality of a solution consisting of 2.66 mL of carbon tetrachloride (CCl_4; d = 1.59 g/mL) in 76.5 mL of methylene chloride (CH_2Cl_2; d = 1.33 g/mL)? When substances are dissolved in a given solvent, Hess's law can be applied to find the Delta H What three AH terms are needed, and what does each describe? When ionic compounds are dissolved in water, what does the Delta H account for? In other words, what two terms are equivalent to Delta H ? Given that Delta H_solute = Delta H_lattake, rewrite Delta H_solin in terms of Delta H_ and Delta H_hydr.

Explanation / Answer

density of CCl4=1.56g/ml

V=2.66mL

Mass of CCl4 =d×v=1.59×2.66=4.229g

d of CH2Cl2=1.336g/mL

V=76.5 mL

Mass=1.33×76.5=101.745g

Molar mass of CCl4=154g

Molarity=mass×1000/molar mass×mass of solvent

=4.229×1000/154×101.745=0.269=0.27

20)A) The 3 terms needed are...

a)breaking solute solute attraction that is lattice enthalpy

b)breaking solvent solvent attraction that is hydrogen bonding

c)formin solute solvent attraction that is solvation enthalpy

B)enthalpy of solution and lattice enthalpy

C)enthalpy of solution=lattice enthalpy+ enthalpy of hydration

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