Arrhenius Acids: HF: It releases H+ ions in water, acting as an acid. H2 SO3 : It is dissociate to give H+ ions, making it an acid. H2 S It increases H+ ionsin aqueous solution. Other compounds do not fulfill this criterion.
The reaction of calcium metal with dilute H2 SO4 (likely meant H2 SO4) is : Ca + H2 SO4 → Ca SO4 + H2 Calcium react reacts with dilute sulfuric acid to produce calcium sulfate and hydrogen gas. This reaction is vigorous.
When HCL reacts with BaCO3 the salt formed is BaCL2 (barium chloride) Reaction: BaCO3 + 2HCL → BaCL2+ H2 O +CO2
Soap is chemically named as a sodium or potassium salt or of a long – chain fatty acid. Example: Sodium stearate ( C17 H35 COONa) is a common soap. It is formed by the reaction of facts with alkalis ( saponification)
HSO4 is a bronsted –lowery acid because it denotes a proton (H+) Reaction : HSO4 → SO42- + H+ This ability to release H+ ions confirms its acidic nature.
HCL is not edible because, is pure form it is a highly corrosive acid. In the stomach, it is present in a diluted form to aid digestion. It helps break down food and activates digestive enzymes like pepsin. However, concentrated HCI can cause burns and severe tissue damage. This makes it unsafe for consumption in its pure form In the presence of a drop of an acid, water is known to ionize as follows: H₂O →← H+ + OH-
Water is both an acid and a base, making it amphoteric. Explanation: Water donates H* ions, acting as an acid: H2 O→ H+ + OH- It also accepts H+ ions, acting as a base: H2 O + H+→H3 O This dual behavior classifies water as amphoteric.
Ans. Sodium carbonate (Na2CO3) behaves like a base in water because it hydrolyzes to produce hydroxide (OH-) ions: Na 2CO 3 + H2 O → 2Na+ + HCO3 + ОН". Sodium carbonate (behaves like a base in water because it dissociates into sodium ion (Na+ ) and carbonate ions (CO32- ) carbonate ion reacts with water to form bicarbonate (HCO3- ) hydroxide ions (OH). This the concentration of OH" in the solution, making it basic. The ability of carbonate to accept a proton (H") from water classifies Na2 CO3 as a basic compound. This property’s why solutions of sodium carbonate turn red litmus paper blue.
Sodium bicarbonate (NaHCO 1 ) is amphoteric, meaning it can act as both an acid and a base As an acid: NaHCO→, Na+ HCO3 (donates H") As a base: HCO3 + H → H₂CO3 (accepts H*) According to equations sodium bicarbonate (NaHCO 3 ) an amphoteric substance, meaning it can act as both a base and an acid, depending on the situation. In water, it usually behaves as a weak base because it reacts with acids to neutralize them, producing carbon dioxide gas. However, it can also act a weak acid in the presence of strong bases, releasing a proton (H*) to form carbonate ions ( CO32-) The dual behavior makes NaHCO3, a versatile compound commonly used in baking and as an antacid.
1 Strong Acid. A strong arid completely ionizes in water, meaning all its molecules dissociate into hydrogen ions (H") and their corresponding anions. Examples include hydrochloric acid (HCI) and sulfuric acid (H2 SO4 ) 2 Concentrated Acid: A concentrated acid has a high amount of acid dissolved in a small amountof water (high concentration of H ions in the solution) Concentration refers to the quantity of acid, not ability to ionize. A strong acid can be dilute, and a weak acid can be concentrated. For example, concentrated acetic acid is still a weak acid because it only partially ionizes in water. 4. Descriptive Questions Explain
The Arrhenius concept defines acids and bases based on their behavior in water: 1 Acids: According to Arrhenius, an acid is a substance that increases the concentration of hydrogen ions (H*) in an aqueous solution. For example, hydrochloric acid (HCI) dissociates in water to produce and Cl ions. 2. Bases: A base is a substance that increases the concentration of hydroxide ions (OH") in aqueous solution For instance, sodium hydroxide (NaOH) dissociates in water to give Na" and OH" ion. This concept is simple and useful but applies only to aqueous solutions and concept explains the behavior of acids and bases in non-aqueous solvents or reactions without water.
The Arrhenius and Bronsted-Lowry concepts of acids and bases differ in their definitions and scope 1 Arrhenius Concept Acids are substances that increase the concentration of H" ions in water while bases increase the concentration of OH ions. It is limited to aqueous solutions and cannot explain acid-base behavior in non-aqueous systems. Bronsted-Lowry Concept Acids are proton (H") donors, and bases are proton (H') acceptors. This concept is broader and applies to reactions in both aqueous and non-aqueous environments. For example, ammonia (NH,) is a base because it accepts a proton, even though it does not produce OH ions directly Thus, the Bronsted-Lowry concept is more versatile compared to the Arrhenius concept.
NH4 CI (Ammonium chloride): H2 SO4 + NH 4CI → NH4 HSO4 +HCL Sulfuric acid reacts with ammonium chloride to form ammonium bisulfate and hydrogen chloride
H2 SO 4, NH4 NO3 →NH4 HSO4 , HNO3 , Ammonium nitrate reacts with sulfuric acid to form ammonium sulfate and nitric acid.
H2 SO4 + MgO→ MgSO4 ,+H₂O Magnesium oxide reacts with sulfuric acid to form magnesium sulfate and water.
H2 SO4,+MgCO3 →MgSO4 , CO2 + H2 O Magnesium carbonate reacts with sulfuric acid to form magnesium sulfate, carbon dioxide, and water
When a base reacts with a non metallic oxide, a salt and water are formed. This is because non-metallic oxides are acidic in nature For example: Ca(OH)2 + CO2 →CaCO3 + H2 O This reaction shows that non metallic oxides, like carbon dioxide (CO₂), behave as acids because they react with bases to neutralize them. Hence, non metallic oxides are considered acidic oxides.
Dry HCI gas does not show acidic properties because it does not ionize in the absence of water. Acidity arises from the presence of hydrogen ions (H"), which are not generated in dry HCl gas However, HCI in water shows acidic properties because it completely ionizes into H" and Ct ions The water facilitates this ionization, releasing H ions that are responsible for the acidic nature. Thus, the acidic character of HCI is observed only when it is dissolved in water, not in its dry form.
An acid and its ronjugate base are related but have distinct roles in a chemical reaction. 1 Acid. An acid donates a proton (H") during a reaction. For example, in water, HCI donates a proton to form C HCI → H +Cl 2 Conjugate Base: The conjugate base is the species that remains after the acid has donated a proton For example, Cl is the conjugate base of RCICI in HCI → H+CI The acid and as conjugate base differ by one proton, Acids are proton donors, while conjugate bases are capable of accepting a proton in the reverse reaction
Acids are crucial for various functions in the human body 1. Hydrochloric Acid (HCI): Found in the stomach, it aids digestion by breaking down food and killing pathogens 2. Amino Acids: Building blocks of proteins essential for growth and repair 3. Fatty Acids. Provide energy and are vital for cell membranes 4. Nucleic Acids Form DNA and RNA, which carry genetic information 5. Carbonic Acid: Helps maintain blood pH balance during respiration These acids support life sustaining processes
Short Duration When CO, is passed through lime water briefly, it turns milky due to the formation of insolutie calcium carbonate Ca(OH)2 + CO2 →CaCO3 + H2 O 2. Long Duration: If CO, is passed for a long time, the milkiness disappears as calcium carbonate reacts with excess CO, to form soluble calcium bicarbonate CaCO3 + CO2 , H₂O→ Ca(HCO3)2
Fruits that contain citric acid include lemons, limes, oranges, and grapefruits These are citra fruits known for their tangy flavour due to the high citric acid content Citric acid is a natural preservative and helps give these fruits their sour taste It also plays a role in maintaining the pH balance in the body
Oxalic acid (H,CO) is the simplest organic diprotic acid its commercial uses include bleach straw and leather and removing rust and ink stains from fabrics
Mineral acids, such as hydrochloric acid, sulfuric acid, and nitric acid, are highly useful in vario ways They are used in industries for manufacturing fertilizers, plastics, and dyes. They play a key role laboratory experiments for chemical analysis and synthesis Additionally, mineral acids are essential refining metals and producing important chemicals
In water, a chloride ion (CI) exists as a negatively charged ion formed when chlorine gains of electron. It is stable and surrounded by water molecules due to the process of hydration, where the positive ends of water molecules (hydrogen) are attracted to the negative chloride ion, keeping it dissolved in the solution HCI + H2 O →← CI + H3 O
Ammonium hydroxide (NH,OH) only partially ionizes in water because it is a weak base. In water it does not completely dissociate into its ions, as the reaction reaches an equilibrium where both the dissociated NH4OH molecules and the ions coexist. This is because the attraction between NH," and OH is strong, preventing complete dissociation The ionization reaction is as follows: NH₂OH→← NH4 + OH Here, the double arrow indicates that the reaction is reversible, and only a small fraction of NH OH molecules dissociate into ions.
Stomach acidity or hyperacidity conditions are common problems. Most often the problem arises when a person takes fatty and spicy foods which cause more acid to produce in the stomach than required Our stomach produces hydrochloric acid to digest the food that we eat. Whenever we eat, cells within the lining of the stomach produce acid Problem occurs when these cells produce more acid than our stomach needs. When it happens the person suffers from stomach acidity The common indication of such a condition is the feeling of burning sensation right below our breast bone. A person may also feel sour taste in mouth and heart burn or pain near the heart area. The uneasy condition may easily be cured by taking weak bases like calcium hydroxide and magnesium hydroxide commonly known as antacids These antacids removed minor stomach disorders by neutralizing the stomach acid, but the concentration of hydroxyl ions in them is too low to harm the throat or stomach
Two examples of Bronsted-Lowry bases that are not Arrhenius bases are ammonia (NH,) and bicarbonate ion (HCO₂) 1 Ammonia (NH,) acts as a Brønsted-Lowry base by accepting a proton (H) NH3 +H₂O→← NH4 + OH Ammonia does not contain OH ions, so it is not an Arrhenius base 2. Bicarbonate ion (HCO,) acts as a Bronsted-Lowry base by accepting a proton: HCO3 + H→← H2CO3 It does not release OH" ions directly, so it is not classified as an Arrhenius base
Blocked drains are one of the most common problems that we face every other day Different blockages require different chemicals to remove them One of way to clean the drains is to pour half a cup of sodium bicarbonate solution into the dram followed by half a cup of vinegar Cover the drain and wait for thirty minutes Four boiling water down the drain Caustic chemical drains cleaners are capable of dissolving grease, hair, food and other common blockages Pour down the caustic cleaner into your drain Wait for half an hour and then flush our drain with water.
An acid is a substance that releases hydrogen ions (H") when dissolved in water. It has a sour tame turns blue litmus paper red, and has a pH less than 7
A base is a substance that releases hydroxide ions (OH) when dissolved in water. It has a bitter taste, slippery feel, turns red litmus paper blue, and has a pit greater than7 .
The pH scale measures the acidity or alkalinity of a solution. It ranges from 0 to 14, with values below 7 indicating acidity, values above 7 indicating alkalinity, and 7 being neutral (like pure water)
When an acid reacts with a base, a neutralization reaction occurs, producing salt and water For example, HCl + NaOH→ NaCl+H₂O.
Acids and bases are important in various daily processes For example, acids are found in food (like vinegar and citrus fruits), and bases are used in cleaning products. Neutralization reactions also help treat indigestion
According to the Arrhenius concept, acids are substances that release hydrogen ions (H") when dissolved in water. For example, hydrochloric acid (HCI) dissociates in water to release H' ions
According to the Arrhenius concept bases are substances that release hydroxide ions (OH") when dissolved in water For example sodium hydroxide (NaOH) dissociates in water to release OH Ions
According to the Bronsted-Lowry theory, an acid is a substance that donates a proton (Hanin a chemical reaction For example, in the reaction between HCI and water, HCI donates a proton to form HO
According to the Bronsted Lowry theory, a base is a substance that accepts a proton (H* ion) in chemical reaction. For example, ammonia (NH3, accepts a proton to form NH,
The Arrhenius definition focuses on the release of H° or OH i`ons in water, while the Bronsted Lowry definition is broader, focusing on proton donation and acceptance, not necessarily in water
In the reaction between ammonia (NH,) and water NH3 + H2 O →NH4+ OH Here, NH, accepts a proton from water, making NH4" and OH.
A conjugate acid-base pair consists of two substances that differ by only one proton For example, in the reaction HCl →H+ CI HCI is the acid and CT is the conjugate base
Water can act as both an acid and a base according to the Bronsted Lowry theory. For example, H2 O+H2 O →H 3O +H one water molecule donates a proton (acting as an acid), and the other accepts a proton (acting as a base)
Yes, according to the Bronsted Lowry theory, substances like water and ammonia can act as both acids and bases, depending on what they are reacting with
The Bronsted Lowry definition is more general because it does not require water for a substance to act as an acid or base it focuses on proton transfer, allowing the concept to apply in a wider range of reactions beyond aqueous solutions. Properties of acids, bases, and salts
Acids have a sour taste and can turn blue litmus paper red. They release hydrogen ions (H") in water, making the solution acidic. For example, when hydrochlornic acid (HCI) is dissolved in water, it dissociates as follows HOIH CI Acids can also react with metals to release hydrogen gas, such as Zn+2HCI ZnCl H
Bases have a bitter taste and slippery feel They turn red litmus paper blue and release hydroxide ions (OH") in water, making the solution basic. For example, sodium hydroxide (NaOH) dissociates in water NaOH →Na+OH Bases can neutralize acids to form salt and water For example NaOH +HCI →NaCl+ H2 O.
Salts are formed when an acid reacts with a base. They are generally neutral, with a pH of around For example, when hydrochloric acid (HCI) reacts with sodium hydroxide (NaOH), sodium chloride (NaCl) is formed as HCI NaOH NaCl HO Salts can conduct electricity when dissolved in water, as they dissociate into ions.
When an acid reacts with a base, a neutralization reaction occurs, producing salt and water. For example, when sulfuric acid (H,SO,) reacts with sodium hydroxide (NaOH), the reaction is H 2SO 4 + 2NaOH→ NaSo4 +2H2O
Acids lower the pH of a solution, making it more acidic, while bases increase the pH, making a more alkaline For example, when hydrochloric acid (HCI) is added to water, the pH drops HCI→H+Cl On the other hand, adding sodium hydroxide (NaOH) to water increases the pH NaOH →Na +OH Acid rain and its effects.
Acid rain is rain that has a pH lower than 5.6 due to the presence of dissolved sulfur dioxide (50) and nitrogen oxides (NO,) in the atmosphere. These gases react with water vapor to form sulfuric acidH2SO4) and nitric acid (HNO,), which then fall as acid rain. The reactions are : SO2+H2O→ H2SO3 H2SO3 +O2 → H2SO4 NOX +H2O → HNO3.
The main causes of acid rain are the burning of fossil fuels like coal and oil, which release sulfur dioxide (SO2) and nitrogen oxides (NOX) into the atmosphere. These gases combine with water vapor forming sulfuric acid and nitric acid, as shown in the following reactions: SO2 +O2 → SO3 SO3 +H2O → H2SO4 NO2 +H2O → HNO3
Acid rain harms plants by lowering the pH of the soil, making it more acidic, which affects nutrient availability and can damage plant roots. The acids in the rain can also directly damage leaves and stems For example, sulfuric acid (H2 SO4.) and nitric acid (HNO3) can cause chemical burns on plant tissues. H2SO4 +H2O → H3SO4 +SO4 2-
Acid rain lowers the pH of rivers, lakes, and streams, making the water more acidic and harmful to aquatic life A decrease in pH can cause the death of fish and other organisms For example, when sulfuric acid dissolves in water, it dissociates into hydrogen ions, lowering the pH. H2SO4 → H++ HSO4 A pH level below 55 can be lethal to many aquatic species
Acid rain can cause the corrosion of buildings and monuments, especially those made of limestone and marble The sulfuric acid in the rain reacts with the calcium carbonate in the stone to form calcium sulfate, carbon dioxide and water For example CaCO 3 + H 2SO4 →CaSO4+ CO2 + H2 O This reaction leads to the erosion of the stone surface over time.
When the temperature is increased in an exothermic reaction, the equilibrium shifts toward the reactants, are the system tries to absorb the added heat by favoring the reverse reaction, which is endothermic.
Decreasing the temperature in an endothermic reaction shifts the equilibrium toward the reactants, as the system tries to release heat by favoring the exothermic reverse reaction
Increasing pressure will shift the equilibrium toward the side with fewer gas molecules. This is because the system will try to decrease the pressure by favoring the side with fewer gas molecules
Increasing pressure shifts the equilibrium toward the side with more gas molecules. The system tries to relieve the pressure by increasing the number of gas molecules.
Adding an inert gas to the system at constant pressure does not affect the equilibrium position, as inert gases do not participate in the reaction and do not change the partial pressures of the reacting gases.
Decreasing pressure in a reaction with gaseous reactants and products shifts the equilibrium toward the side with more gas molecules, as this increases the total volume, counteracting the decrease in pressure
Increasing temperature in an endothermic reaction shifts the equilibrium toward the products, as the system absorbs the added heat to favor the forward reaction, which is endothermic.
Decreasing the temperature in an exothermic reaction shifts the equilibrium toward the products, as the system releases heat to favor the exothermic forward reaction
The equilibrium constant (K) changes with temperature because it is temperature-dependent For endothermic reactions, K, increases with increasing temperature, while for exothermic reactions, K. decreases as temperature rises.
A catalyst speeds up the rate at which equilibrium is reached by lowering the activation energy. However, it does not affect the position of the equilibrium, as it accelerates both the forward and reverse reactions equally
If the concentration of a reactant is increased, the equilibrium shifts toward the products to counteract the change by consuming the added reactant and forming more products
When the concentration of a product is increased, the equilibrium shifts toward the reactants, as the system tries to use up the excess product and form more reactants.
A shift in equilibrium refers to a change in the position of equilibrium in response to a change in conditions such as temperature, pressure, or concentration. The system adjusts to minimize the effect of the disturbance
For exothermic reactions, increasing temperature shifts the equilibrium toward the reactants, while for endothermic reactions; increasing temperature shifts the equilibrium toward the products
In this reaction, the number of gas molecules is fewer on the product side (2 molecules of NH₃) compared to the reactant side (4 molecules: 1 of N2 , and 3 of H2.) Increasing pressure shifts the equilibrium toward the side with fewer gas molecules to reduce the pressure.
