What mass of salt (nacl) should you add to 1.48 l of water in an ice cream maker to make a solution that freezes at -13.4 ∘c ? assume complete dissociation of the nacl and density of 1.00 g/ml for water?

311.6g NaCl you should add

Explanation:

When you add a solute (NaCl) to solvent (Water), the freezing point of the solution decreases with regard to pure solvent following the equation:

ΔT = Kf × m × i

Where ΔT is change in temperature(From 0°C to -13.4°C), Kf is freezing point depression constant (1.86°C/m for water), m is molality of solution (Moles solute / 1.48 kg solvent -Because 1.48L≡1.48kg; density 1.00g/mL-) and i is Van't Hoff factor (2 for NaCl because in water, NaCl dissociates as Na⁺ and Cl⁻ ions, 2 ions).

Replacing:

13.4°C = 1.86°C/m × moles NaCl / 1.48kg × 2

5.33 = moles NaCl

As molar mass of NaCl is 58.44g/mol, mass in 5.33moles are:

5.33mol NaCl × (58.44g /mol) = 311.6g NaCl you should add

altitude, density, pressure

air gets less dense the higher the altitude and also the air pressure is less as altitude rises.

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.