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Unit 1 - Chapter 1 - Integrated Sciences for Grade 10 (First Year of Secondary School) - First Semester شرح علوم متكاملة لغات الصف الاول الثانوي لغات - الفصل الدراسي الأول شرح علوم متكاملة اولي ثانوي لغات - ترم أول In This Lesson : The Effects of Chemical Reactions on Water Quality ▌Water's unique properties make it vital for life. Its ability to dissolve substances and exist in different states is crucial for life processes. Water is essential for all living things, from tiny microbes to large animals. It moves into cells, providing nutrients and removing waste. ▌Water, covering approximately 70% of Earth's surface, sets our planet apart from others in the solar system. This vast amount of water, known as the hydrosphere: Divided into: Salty water existing in oceans, seas, and saltwater lakes. Freshwater Only a small portion is freshwater found in rivers, lakes, and underground. Water vapor contributes to the atmosphere, while frozen water, is found in polar regions and glaciers Hydrological cycle ▌The water cycle is a continuous process that moves water around Earth. Water evaporates from bodies of water and land, rises into the atmosphere, condenses to form clouds, and falls back to Earth as precipitation. This cycle is influenced by various processes, including transpiration from plants, infiltration into the ground, and chemical reactions that can lead to acid rain. Chemical Composition of Water Water is composed of two elements: hydrogen and oxygen. By volume hydrogen and oxygen combine in a 2:1 ratio By mass oxygen accounts for approximately 88.89% of a water molecule, while hydrogen constitutes about 11.11%. Chemical Properties of Water Water, as found on Earth, is rarely pure. It typically contains various ions and chemical substances that interact with it in numerous ways. Let's explore three of water's primary chemical properties: ❶ Polarity of Water: the oxygen atom in a water molecule has a much higher electronegativity than the hydrogen atoms. This causes the electrons in the covalent bonds to be pulled more strongly towards the oxygen atom. As a result, the oxygen atom carries a partial negative charge (δ-), while the hydrogen atoms carry partial positive charges (δ+). This uneven distribution of charge gives the water molecule a polar character. It allows water to dissolve a wide range of substances, transport nutrients, and participate in numerous biological processes. Example: Salt (NaCl) dissolves in water because the positive sodium ions are attracted to the negative oxygen end of water molecules, while the negative chloride ions are attracted to the positive hydrogen end. The ability of water molecules to form hydrogen bonds with each other is a primary reason for the high boiling point of pure water, which reaches 100 degrees Celsius under standard atmospheric pressure. This is in contrast to compounds with similar structures, such as hydrogen sulfide, which boils at -61 degrees Celsius. ❷ Hydrolysis: A small percentage of water molecules exist as hydrogen ions (H⁺) and hydroxide ions (OH⁻). Chemical reactions with various compounds can cause hydrolysis of certain salts present in natural water, affecting the balance of these ions and resulting in the acidity or alkalinity of the water. Practical Example: ▌When table salt (NaCl) is added to water, it dissociates into sodium ions (Na⁺) and chloride ions (Cl⁻). These ions remain in the solution without interacting with water ions, making the solution neutral because the concentration of hydrogen ions (H⁺) is equal to the concentration of hydroxide ions (OH⁻). ▌However, in the case of sodium bicarbonate (NaHCO₃), hydrolysis occurs, leading to a decrease in the concentration of hydrogen ions (H⁺) and an increase in the concentration of hydroxide ions (OH⁻) making the salt solution basic. HCO₃⁻ + H₂O → H₂CO₃ + OH⁻ ▌The opposite occurs when ammonium chloride (NH₄Cl) is dissolved in water, which undergoes hydrolysis and causes a decrease in the concentration of hydroxide ions and an increase in the concentration of hydrogen ions, making the salt solution acidic. NH₄⁺ + H₂O → NH₃ + H₃O⁺ ❸ Acid-base balance: - The acid-base balance in water depends on the relationship between the concentration of hydrogen ions (H+) and hydroxide ions (OH⁻). This relationship can be determined by measuring the pH of the solution. pH is a scale ranging from 0 to 14. If the concentration of H⁺ ions increases, the water becomes acidic and the pH value is less than 7. - Conversely, if the concentration of OH⁻ ions increases, the water becomes basic and the pH value is greater than 7. - When the concentrations of H⁺ and OH⁻ ions are equal, the water is neutral and the pH value is 7.

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