Why would buffered solution tests be compared to distilled water?

Why do proteins form precipitates under some conditions and gels under others?

A solute is a minor component of a solution. For example, if a small amount of benzoic acid is dissolved in diethylether, the benzoic acid is considered to be the solute. If you had 2 solutes (like napthalene and sodium bicarbonate), in which layer would you find each solute? Why?

Explain the difference between a. a colloidal and a crystalline precipitate b. precipitation and coprecipitation c. peptization and coagulation of a colloid d. occlusion and mixed-crystal formation e. nucleation and particle growth

Suppose you are recrystallizing a compound and boil the solution for so long that a substantial amount of liquid evaporates. What is likely to happen to some of the solute? What should you do if this occurs?

Use the solubility graph to answer the following question. Which of the listed salts is the most soluble at 20 °C? Solubility (g/L of solvent) OKCI NaCl OKNO3 O KI NH4CI 1400 1300 1200 1100 1000 900 800 700 600 500 400 300 200 100 0 Solubility Curves ZKI -HCI SO₂ NaNO3 -KNO3 NHẠCH KCI -KCIO3 NaCl NH₂ 10 20 30 40 50 60 70 80 90 100 Temperature (°C)

Why do two layers form when solutions containing water are added to the extracted dichloromethane (CH2CI-2) solution?

QUESTION 26 It is a type of coprecipitation in which a normally soluble compound is carried out of solution on the surface of a coagulated colloid. mechanical entrapment occlusion mixed crystal formation surface adsorption

Provide a flow chart analogous to separate a diethyl ether solution containing benzoic acid, 2-naphthol (a weak acid), 4-nitroaniline (a weak base), and naphthalene