Question

An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114...

An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114 g/mL; M = 62.07 g/mol) and water (d = 1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as

(a) volume percent % v/v

(b) mass percent % w/w

(c) molarity M

(d) molality m

(e) mole fraction

Homework Answers

Answer #1

Solution-

Let us assume 10 mL of ethylene glycol and 10 mL of water

mass ethylene glycol = 10 mL x 1.114 g/mL = 11.14 g
mass water = 10 mL x 1.00 g/mL = 10.0 g
mass solution = 11.14 + 10.0= 21.14 g

mass percent = 11.14 x 100/ 21.14 = 52.7

volume solution = 21.14 g / 1.070 g/mL=19.8 mL

volume percent = 10 x 100/ 19.8=50.5

moles ethylene glycol = 11.14 / 62.07 =0.179
M = 0.179/ 0.0198 L=9.06

m = 0.179/ 0.010 Kg = 17.9

moles water = 10.0 g/ 18.02 g/mol=0.555
mole fraction = 0.179/0.179 + 0.555 =0.244

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Different Ways of Expressing Concentration An aqueous antifreeze solution is 35.5% ethylene glycol (C2H6O2) by mass....
Different Ways of Expressing Concentration An aqueous antifreeze solution is 35.5% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.045 g/cm3. Calculate the molality of the ethylene glycol. 8.87 m Calculate the molarity of the ethylene glycol. Calculate the mole fraction of ethylene glycol
Ethylene glycol (62.1 g/mol), a nonvolatile organic compound, is commonly used in antifreeze. If you buy...
Ethylene glycol (62.1 g/mol), a nonvolatile organic compound, is commonly used in antifreeze. If you buy pure ethylene glycol and mix your own radiator fluid by pouring 2.5L of the ethylene glycol in a bucket with 2.5L of water, what will be the freezing point (°C)? van ’t Hoff factor of ethylene glycol = 1 density of ethylene glycol = 1.11 g/mL density of water = 1.00 g/mL Kf for water = 1.86°C kg/mol
To what minimum temperature would a radiator be protected if equal volumes of ethylene glycol (permanent...
To what minimum temperature would a radiator be protected if equal volumes of ethylene glycol (permanent antifreeze) (density 1.11 g/mL) and water were mixed. Assume that ethylene glycol does not dissociate and has a formula, C2H6O2.
Be sure to answer all parts. Ethylene glycol [CH2(OH)CH2(OH)] is a common automobile antifreeze. Calculate the...
Be sure to answer all parts. Ethylene glycol [CH2(OH)CH2(OH)] is a common automobile antifreeze. Calculate the freezing point and boiling point of a solution containing 253 g of ethylene glycol and 1095 got water.(Kb and Kf for water are 0.52°C/m and 1.86°C/m, respectively.) freezing point   °C boiling point   °C
A solution is prepared by mixing 25 mL pentane (C5H12, d = 0.63 g/cm3) with 30...
A solution is prepared by mixing 25 mL pentane (C5H12, d = 0.63 g/cm3) with 30 mL hexane (C6H14, d = 0.66 g/cm3). Assuming that the volumes add on mixing, calculate the mass percent, mole fraction, molality, and molarity of the pentane.
1. Ethylene glycol [CH2(OH)CH2(OH)] is a common automobile antifreeze. Calculate the freezing point and boiling point...
1. Ethylene glycol [CH2(OH)CH2(OH)] is a common automobile antifreeze. Calculate the freezing point and boiling point of a solution containing 323 g of ethylene glycol and 1025 g of water. (Kb and Kf for water are 0.52°C/m and 1.86°C/m, respectively.) freezing point ___  °C boiling point ___°C 2. Calculate the molar mass of naphthalene, the organic compound in mothballs, if a solution prepared by dissolving 10.0 g of naphthalene in exactly 200 g of benzene has a freezing point 2.0°C below...
An aqueous ethylene glycol (HOCH2CH2OH, FW = 62.07 g/mol) solution with a mass of 279.1 mg...
An aqueous ethylene glycol (HOCH2CH2OH, FW = 62.07 g/mol) solution with a mass of 279.1 mg is titrated with 42.9 mL of 0.0939 M Ce4 in 4 M HClO4. The solution is held at 60°C for 15 minutes to oxidize the ethylene glycol to formic acid (HCO2H) and carbon dioxide. The excess Ce4 is titrated with 11.89 mL of 0.0417 M Fe2 to a ferroin end point. What is the mass percent of ethylene glycol in the unknown solution?
A sodium hydroxide solution is made by mixing 13.64 g NaOH with 100 g of water....
A sodium hydroxide solution is made by mixing 13.64 g NaOH with 100 g of water. The resulting solution has a density of 1.131 g/mL. a. What is the molarity of this solution? b. What is the molality of the solution? c. What is the mass fraction of NaOH in the solution? d. What is the mole fraction of NaOH in the solution?
± Introduction to Units of Concentration The composition of a solution can be expressed in several...
± Introduction to Units of Concentration The composition of a solution can be expressed in several different ways. Four of the most common concentration units are defined as follows:. mass %=mass of componenttotal mass of solution×100% mole fraction (X)=moles of componenttotal moles of solution molarity (M)=moles of soluteliters of solution molality (m)=moles of solutemass of solvent (kg) A solution was prepared by dissolving 33.0 g of KCl in 225 g of water. Part A Calculate the mass percent of KCl...
A solution was prepared by dissolving 26.0 g of KCl in 225 g of water. The...
A solution was prepared by dissolving 26.0 g of KCl in 225 g of water. The composition of a solution can be expressed in several different ways. Four of the most common concentration units are defined as follows:. mass %=mass of componenttotal mass of solution×100%; mole fraction (X)=moles of componenttotal moles of solution; molarity (M)=moles of soluteliters of solution; molality (m)=moles of solutemass of solvent (kg) Part A Calculate the mass percent of KCl in the solution. Part B Calculate...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT