How many liters of the antifreeze ethylene glycol [ch2(oh)ch2(oh)] would you add to a car radiator containing 6.50 l of water if the coldest winter temperature in your area is -10.°c? (the density of ethylene glycol is 1.11 g/ml. assume the density of water at -10.°c is 1.00 g/ml.)

Around 2.0 L of ethylene glycol needs to be added to the car radiator

Explanation:

The depression in freezing point ΔTf of a solution is directly proportional to its molality (m), i.e.

From the given information:

= freezing pt of solution = -10.0 C

= freezing pt of pure solvent = 0 C

Kf = freezing pt depression constant = 1.86 C/m

i = 1 for ethylene glycol antifreeze

Volume of water = 6.50 L = 6500 ml

Density of water = 1.00 g/ml

Therefore mass of water =

Molar mass of ethylene glycol = 62 g/mol

Mass of ethylene glycol needed =

Density of ethylene = 1.11 g/ml

Therefore, volume needed =

plasma is the state of matter where the substance is ionized and has no definite shape or volume. the fact of being ionized makes the substance a good electrical conductor.

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.