- Amal Augustine
- January 27, 2026
Essential Guide: Toxicity and Safety of Ethylene Glycol Explained
Ethylene glycol is a widely used organic compound in chemistry and industry, especially as an antifreeze and coolant. Despite its usefulness, understanding its health risks is extremely important. This article focuses on toxicity and safety of ethylene glycol explained in a clear and practical way, helping aspirants and readers understand both its dangers and safe handling practices.
Ethylene glycol is a colorless, odorless, sweet-tasting liquid, which unfortunately makes accidental ingestion more likely. The phrase toxicity and safety of ethylene glycol explained becomes crucial because even small amounts can cause severe poisoning in humans and animals. Once ingested, ethylene glycol is metabolized in the liver into toxic compounds such as glycolic acid and oxalic acid, which are responsible for its harmful effects.
From a chemical and medical perspective, toxicity and safety of ethylene glycol explained begins with understanding how it affects the body. Initially, symptoms may resemble alcohol intoxication, including dizziness, nausea, and confusion. As metabolism progresses, severe metabolic acidosis occurs, leading to kidney failure, respiratory distress, and potentially death. This delayed toxicity makes early diagnosis difficult, reinforcing why toxicity and safety of ethylene glycol explained is an important topic.
In laboratory and industrial environments, toxicity and safety of ethylene glycol explained emphasizes strict handling protocols. Ethylene glycol should always be stored in properly labeled containers and kept away from food or drink containers to prevent accidental ingestion. Protective equipment such as gloves, safety goggles, and lab coats should be used when handling it to minimize skin contact.
Another key aspect of toxicity and safety of ethylene glycol explained is its environmental impact. Spills can contaminate soil and water sources, posing risks to wildlife. Although ethylene glycol is biodegradable, high concentrations can still be toxic to aquatic organisms. Therefore, disposal must follow environmental safety regulations, which is an essential part of toxicity and safety of ethylene glycol explained.
In households, antifreeze products containing ethylene glycol are a common source of poisoning, especially in pets. The sweet taste attracts animals, making accidental ingestion common. Veterinarians stress the importance of pet-safe antifreeze alternatives. This real-life relevance highlights toxicity and safety of ethylene glycol explained beyond textbooks.
Medical treatment also falls under toxicity and safety of ethylene glycol explained. Antidotes such as ethanol or fomepizole are used because they inhibit the enzyme alcohol dehydrogenase, preventing formation of toxic metabolites. In severe cases, hemodialysis is required. Awareness of treatment options reinforces why toxicity and safety of ethylene glycol explained is vital for emergency response.
From a chemistry education standpoint, toxicity and safety of ethylene glycol explained is often included in topics like alcohols, industrial chemicals, and environmental chemistry. Aspirants must understand not only reactions and properties but also health hazards and safety symbols associated with ethylene glycol.
Toxicity and Safety of Ethylene Glycol Explained MCQs
1.
Which one of the following 0.06 M aqueous solutions has the lowest freezing point?
A. C₆H₁₂O₆
B. Al₂(SO₄)₃
C. K₂SO₄
D. KI
Answer: B
2.
A solute dimerizes in water. The boiling point of a 2 molar solution of A is 100.52°C. The percentage association of A is (nearest integer):
(Use Kb = 0.52 K kg mol⁻¹, bp of water = 100°C)
A. 25
B. 50
C. 75
D. 100
Answer: D
3.
2 molal solution of weak acid HA has freezing point of -3.885°C. Degree of dissociation is ____ ×10⁻³ (nearest integer).
(Kf = 1.85, fp of water = 0°C)
A. 25
B. 30
C. 50
D. 3
Answer: C
4.
40 g glucose (M=180) is mixed with 200 mL water. Freezing point is ____ K (nearest integer).
(Kf = 1.86, density water = 1 g/mL, fp water = 273.15 K)
A. 271.09 K
B. 270.99 K
C. 270.69 K
D. 270.49 K
Answer: A
5.
1 kg of 0.75 molal aqueous sucrose solution can be cooled up to -4°C before freezing. Ice separated (in g) is ____ (nearest integer).
(Kf(H₂O)=1.86)
A. 180 g
B. 204 g
C. 256 g
D. 518 g
Answer: D
6.
Solutions:
P₁: 10 g glucose in 250 mL water
P₂: 10 g urea in 250 mL water
P₃: 10 g sucrose in 250 mL water
Decreasing order of osmotic pressure is:
A. P₁ > P₂ > P₃
B. P₂ > P₁ > P₃
C. P₃ > P₂ > P₁
D. P₂ > P₃ > P₁
Answer: B
7.
1.22 g organic acid dissolved in 100 g benzene (Kb=2.6) and 100 g acetone (Kb=1.7). Acid dimerises in benzene, monomer in acetone. Boiling point rise in acetone = 0.17°C. Rise in benzene = x×10⁻¹. x is (nearest integer):
A. 10
B. 2
C. 13
D. 4
Answer: C
8.
Which 0.10 M aqueous solution shows largest freezing point depression?
A. Hydrazine
B. Glucose
C. Glycine
D. KHSO₄
Answer: D
9.
12.2 g benzoic acid in 100 g water gives fp = -0.93°C. Kf = 1.86. Number of molecules associated (100% association) is:
A. 1
B. 2
C. 3
D. 4
Answer: B
10.
83 g ethylene glycol dissolved in 625 g water. Freezing point is ____ K (nearest integer).
(Kf=1.86, fp water = 273 K)
A. 269 K
B. 279 K
C. 267 K
D. 277 K
Answer: A
11.
1 molal aqueous electrolyte A₂B₃ is 60% ionised. Boiling point at 1 atm is ____ K (nearest integer).
(Kb = 0.52)
A. 370 K
B. 375 K
C. 376 K
D. 377 K
Answer: B
12.
Which graph correctly represents change in freezing point with solute concentration? (image options)
A. Option 1
B. Option 2
C. Option 3
D. Option 4
Answer: B
13.
On mixing urea, bp of water becomes 100.5°C. Freezing point of solution is:
(Kf=1.87, Kb=0.52)
A. -0.5°C
B. 0°C
C. -1.8°C
D. -1°C
Answer: C
14.
Match:
(A) Ebullioscopic constant → (III) Elevation of boiling point
(B) Cryoscopic constant → (I) Depression in freezing point
(C) Henry’s law → (IV) Solubility of gas in liquid
(D) Dalton’s law → (II) Total pressure sum of partial pressures
Correct option is:
A. Option 1
B. Option 2
C. Option 3
D. Option 4
Answer: C
15.
AB₂ is 10% dissociated to A²⁺ and B⁻. Boiling point of 10.0 molal aqueous AB₂ is ____ °C (nearest integer).
(Kb=0.5, bp water=100°C)
A. 100.5°C
B. 101.0°C
C. 106°C
D. 102.0°C
Answer: C
16.
During which processes does entropy decrease?
(i) Freezing at 0°C
(ii) Freezing at -10°C
(iii) N₂ + 3H₂ → 2NH₃
(iv) Adsorption of CO₂ on lead
(v) Dissolution of NaCl
Correct option:
A. (i, ii, iii, iv)
B. (i, iii, v)
C. (i, v)
D. (ii, iii)
Answer: A
17.
At 298 K, ΔHfusion = 2.8 kJ/mol and ΔHvap = 98.2 kJ/mol. ΔHsublimation is (nearest integer):
A. 101 kJ mol⁻¹
B. 126 kJ mol⁻¹
C. 56 kJ mol⁻¹
D. 70 kJ mol⁻¹
Answer: A
18.
2 g non-electrolyte (M=500) dissolved in 57.3 g xylene. Kf(xylene)=4.3. Depression in fp is:
A. 57.3 K
B. 0.3 K
C. 4.3 K
D. 0.002 K
Answer: B
19.
Which forms an ideal solution?
A. C₂H₅OH & H₂O
B. HNO₃ & H₂O
C. CHCl₃ & CH₃COCH₃
D. C₆H₆ & C₆H₅CH₃
Answer: D
20.
72.4 g maltose (M=342.3) in 1000 g ethanol. Depression in fp of ethanol is ____ K.
(Kf=1.23)
A. 0.26
B. 0.42
C. 0.47
D. 0.2
Answer: A
21.
Elevation in bp of 10 g binary electrolyte (M=100) in 100 g water is ΔTb. Then Kb of water is:
A. ΔTb/2
B. 10
C. 10ΔTb
D. ΔTb/10
Answer: A
22.
Which aqueous solution has highest boiling point? (Identical conditions)
A. 1% Glucose
B. 1% Sucrose
C. 1% Urea
D. 1% Phenol
Answer: C
23.
Calculate molal depression constant of a solvent freezing at 15°C. Latent heat fusion = 180.7 J/g.
A. 3.81 K molal⁻¹
B. 0.381 K molal⁻¹
C. 1.90 K molal⁻¹
D. 0.19 K molal⁻¹
Answer: A
24.
Which condition is not satisfied by an ideal solution?
A. Both ΔmixH = 0 and ΔmixS = 0
B. Obeyance of Raoult’s law
C. Both ΔmixH = 0 and ΔmixV = 0
D. ΔmixH = 0
Answer: A
25.
Urea solution (M=60) boils at 100.20°C. Kf=1.86, Kb=0.512. Freezing point is:
A. -0.654°C
B. 0.654°C
C. -0.726°C
D. 0.726°C
Answer: C
26.
Kf(water)=1.86. Ice begins to separate from 10 mass% ethylene glycol at:
A. -1.86°C
B. -3.3°C
C. -2.3°C
D. -3°C
Answer: B
27.
Kf of benzene = 5.12. For molality 0.078 m, ΔTf (rounded to 2 decimals) is:
A. 0.20 K
B. 0.40 K
C. 0.60 K
D. 0.80 K
Answer: B
28.
Potassium ethyl xanthate in froth flotation makes ore:
A. Lighter
B. Hydrophobic
C. Hydrophilic
D. Heavier
Answer: B
29.
ΔTb of 0.10 m CrCl₃·xNH₃ solution is twice that of 0.05 m CaCl₂. Find x.
(Assume 100% ionisation, coordination no. Cr = 6, all NH₃ in coordination sphere)
A. 4
B. 5
C. 10
D. 15
Answer: B
30.
How much NaCl to add to 600 g water to lower freezing point to -0.2°C? (Kf = 2 K kg mol⁻¹)
A. 1.76 g
B. 2.34 g
C. 0.94 g
D. 1.02 g
Answer: A
Conclusion on Toxicity and Safety of Ethylene Glycol Explained
In conclusion, toxicity and safety of ethylene glycol explained is essential knowledge for chemists, students, healthcare professionals, and the general public. While ethylene glycol plays an important role in industry and daily life, improper handling can have fatal consequences. Repeating the core idea of toxicity and safety of ethylene glycol explained ensures awareness, prevention, and responsible use of this chemical.Understanding toxicity and safety of ethylene glycol explained ultimately bridges the gap between chemistry theory and real-world responsibility.
Amal Augustine is the founder of ExQuizMe, a dynamic learning and quiz platform built to make education engaging, competitive, and fun. A passionate learner and an academic achiever, Amal completed his schooling at Government HSS Manjapra, graduating with 92.5% in Computer Science. He later earned his degree from St. Stephen’s College, University of Delhi, one of India’s most prestigious arts and science institutions.
Currently, Amal is pursuing his Master’s degree at National Sun Yat-sen University, Taiwan, where he continues to deepen his interest in research and technology. Throughout his school and college years, he won 50+ national-level interschool and collegiate quiz competitions, was
Beyond academics, Amal Augustine is an avid reader of science journals, a dedicated research student, and a technology enthusiast who loves programming and exploring the world of Computer Science. Through ExQuizMe, he aims to make learning accessible, enjoyable, and empowering for students across the globe.