Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column next to the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution 1.1 g of hydrobromic acid (HBr) dissolved in 350. mL of water 1.1 g of potassium chloride (KCI) dissolved in 350. mL of water 1.1 g of glycerin (C3H8O3) dissolved in 350. mL of water 350. mL of pure water freezing point (choose one) ✓ (choose one) (choose one) ✓ (choose one) boiling point (choose one) (choose one) ✓ (choose one) ✓ (choose one)
States of Matter
The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).
Chemical Reactions and Equations
When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
Colligative properties :
Colligative properties are the properties that are depends on the number of molecules present in the solution instead of nature of molecules present in solution.
Elevation in the boiling point :
Due to the number of molecules present in the solution, the boiling point of the solution increases.
Lowering in the freezing point :
Due to the number of molecules present in the solution, the freezing point of the solution decreases.
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