Consider the solubilities of common solids shown in the graph below. Determine which substance will have a greater molar solubility at 50°C: NH₄Cl or KBr.

Identify the compound that would be more soluble in n-octane, C₈H₁₈ from the following pair: ethylene glycol, HOCH₂CH₂OH or toluene, C₆H₅CH₃.

Given the strength of attraction for solutions X, Y, and Z. Arrange them from most endothermic to most exothermic.

The following are some sulfate salts with their solubility (mass%) in water at 25°C

Ag₂SO₄ = 0.830

PbSO₄ = 0.00443

BaSO₄ = 0.245

SrSO₄ = 0.0135

If a saturated solution was created individually for each of the sulfate salts given above, what will be their molality?

What is the molality of a solution produced by diluting 278 g of KCl in distilled water that resulted in a total solution volume of 2.00 L? (density of solution = 1.03 g/mL)

An aqueous solution is 23.0% acetic acid (CH₃COOH) by mass. Calculate the mole fraction of the solute and the molality of the solution.

Air is enclosed in a container and exerts a total pressure of 2 atm. Find the concentration of carbon dioxide in parts per million if its partial pressure is 2.7×10^-4 atm, assuming that the average molar mass of air is 29 g/mol.

Determine which has the higher molarity in water, 30 ppm NaCl or 40000 ppb NaF.

WHO guidelines recommend that the amount of residual chlorine in drinking water should not be higher than 5 parts per million (ppm). The amount of chlorine can be determined by back titration with potassium iodide:
Cl₂(aq) + 2 I⁻(aq) → 2 Cl⁻(aq) + I₂(aq)
The iodine formed as a result of the reaction above is then titrated with a solution of sodium thiosulfate:
2 Na₂S₂O₃(aq) + I₂(aq) → 2 NaI(aq) + Na₂S₄O₆(aq)
A 350.0 mL water sample was added with excess solid sodium iodide and the resulting solution was then titrated against a 2.25×10⁻³ M sodium thiosulphate solution. The solution required 14.5 mL of Na₂S₂O₃ to reach the equivalence point. How many grams of chlorine are there in the water sample?

The average amount of methane (CH₄) in the atmosphere is 1.87 ppm. If a sample of air has a total pressure of 760 mmHg, what is the partial pressure of methane in the sample?

38.9 g of lactose (C₁₂H₂₂O₁₁) is dissolved in 483 g of water to a final volume of 496 mL. Determine the concentration of this solution in the following units.

a. Molarity

b. Molality

c. Percent by mass

d. Mole fraction

e. Mole percent

The following are temperature independent except which unit?