For each solute (i) complete the following table where %i= the percent of the so
ID: 718095 • Letter: F
Question
For each solute (i) complete the following table where %i= the percent of the solute in the solutioin, Mi = molarity, mi= molality, and Xi = mole fraction of “i” .For each solute (i) complete the following table where %i= the percent of the solute in the solutioin, Mi = molarity, mi= molality, and Xi = mole fraction of “i” .
fo achsolute completethefollow ngt blewhere %i the percent of thesolute inthese u in Me molarity, me molality, and X,- mole fraction of "You should show how you arrived at your answers show your work on a separate piece of paper s) Remember to circle your answers when you show your lute in the solutioin work Solute (olgsolute lehto volume Density %1 M Xi of Sofutionsolution of the HC,HO 5.00g 95.0g KNO CH0 54.0 1.007 /cm 1001.120 0.03764 cm 36.0 69.8 mi 100 miL 50.0% H5034.875
Explanation / Answer
Part a
For HC2H3O2
Total mass = mass of solute + Mas of H2O
= 5.00 + 95.0
= 100.0 g
Volume of solution = mass/density
= (100.0g) / (1.007 g/cm3)
= 99.3 cm3 = 99.3 mL = 0.0993 L
%i = mass of HC2H3O2 x 100 / mass of solution
= 5 x 100 / (5 + 95)
%i = 5 %
moles of HC2H3O2 = mass / molecular weight
= 5g / 60g/mol
= 0.08333 mol
Moles of water = 95g / 18g/mol = 5.27777 mol
Molarity = moles of HC2H3O2 / volume of solution
= 0.08333 mol / ( 0.0993 L)
Mi = 0.839 M
Molality = moles of HC2H3O2 / Mass of water in kg
= 0.08333 mol / ( 95 g x 1 kg/ 1000 g)
mi = 0.877 m
Total Moles = 0.08333 + 5.27777 = 5.3611 mol
Mol fraction of HC2H3O2 = moles of HC2H3O2 / total moles
= 0.08333 / 5.3611
Xi = 0.0155
Part b
For KNO3
Mass of solution = volume x density
= 1.00 L x 1000 cm3/L x 1.120 g/cm3
Mass of KNO3 + mass of water = 1120 g
w1 + w2 = 1120
w1 = 1120 - w2 ........... Eq1
Mol fraction of KNO3 = moles of KNO3 / (moles of KNO3 + moles of water)
0.03764 = n1 / (n1 + n2)
0.03764 n1 + 0.03764 n2 = n1
0.03764 n2 = 0.96236 n1
n1/n2 = 0.039112
(w1/M1) /(w2/M2) = 0.039112
(w1M2) / (w2M1) = 0.039112
(w1 x 18) / (w2 x 101.10) = 0.039112
w1/w2 = 0.21968
w1 = w2 x 0.21968 .......... Eq2
From Eq1 and eq2
w2 x 0.21968 = 1120 - w2
w2 = 918.27 g = mass of water
w1 = 1120 - 918.27 = 201.73 g = mass of KNO3
%i = mass of KNO3 x 100 / mass of solution
= 201.73 x 100 / (1120)
%i = 18.01 %
moles of KNO3 = mass / molecular weight
= 201.73g / 101.10g/mol
= 1.99535 mol
Molarity = moles of KNO3 / volume of solution
= 1.99535 mol / ( 1 L)
Mi = 1.995 M
Molality = moles of KNO3 / Mass of water in kg
= 1.99535 mol / ( 918.27 g x 1 kg/ 1000 g)
mi = 2.173 m
Part c
For C12H22O11
Density of solution = mass of solution / volume of solution
= (54 + 36) g / 69.8 mL
= 1.29 g/mL = 1.29 g/cm3
Moles of C12H22O11 = Mass / molecular weight
= 54g / 342.2965 g/mol
= 0.157757 mol
Moles of water = 36/18 = 2 mol
Mass of water in kg = 36 g x 1kg/1000g = 0.036 kg
%i = mass of C12H22O11 x 100 / mass of solution
= 54 x 100 / (54 + 36)
= 60 %
Molarity = moles of C12H22O11 / volume of solution
= 0.157757 mol / ( 69.8 mL x 1L/1000 mL)
Mi = 2.26 M
Molality = moles of C12H22O11 / Mass of water in kg
= 0.157757 mol / ( 0.036 kg)
mi = 4.38 m
Total Moles = 0.157757 + 2 = 2.157757 mol
Mol fraction of C12H22O11 = moles of C12H22O11 / total moles
= 0.157757 / 2.157757
Xi = 0.07311
Part d
For H2SO4
Mass of H2SO4 = 34.875 g
%i = 50% = mass of H2SO4 x 100 / mass of solution
0.50 x mass of solution = 34.875
Mass of solution = 69.75 g
Mass of water = 69.75 - 34.875 = 34.875 g
Volume of solution = 100 mL
Density of solution = mass of solution / volume of solution
= 69.75 g / 100 mL
= 0.6975 g/mL = 0.6975 g/cm3
Moles of H2SO4 = Mass / molecular weight
= 34.875 g / 98.079 g/mol
= 0.35558 mol
Moles of water = 34.875 g / 18 g/mol = 1.9375 mol
Mass of water in kg = 34.875 g x 1kg/1000g = 0.034875 kg
Molarity = moles of H2SO4 / volume of solution
= 0.35558 mol / ( 100 mL x 1L/1000 mL)
Mi = 3.56 M
Molality = moles of H2SO4 / Mass of water in kg
= 0.35558 mol / ( 0.034875 kg)
mi = 10.2 m
Total Moles = 0.35558 + 1.9375 = 2.29308 mol
Mol fraction of H2SO4 = moles of H2SO4 / total moles
= 0.35558 / 2.29308
Xi = 0.1551
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