Nitric acid (HNO3) and barium carbonate (BaCO3) are two chemical compounds that are commonly encountered in various industries and laboratory settings. HNO3 is a strong acid that is widely used in the production of fertilizers, explosives, and dyes, as well as in the etching and cleaning of metals. On the other hand, BaCO3 is a white, odorless powder that is primarily used in the manufacturing of ceramics, glass, and pigments. In this article, we will explore the properties, uses, and reactions of HNO3 and BaCO3, shedding light on their significance in different applications. So, let’s dive in and uncover the fascinating world of HNO3 and BaCO3!
Key Takeaways
- HNO3 and BaCO3 are chemical formulas for nitric acid and barium carbonate, respectively.
- Nitric acid is a strong acid commonly used in various industries, including the production of fertilizers, dyes, and explosives.
- Barium carbonate is a white, odorless powder used in the manufacturing of ceramics, glass, and specialty chemicals.
- When nitric acid reacts with barium carbonate, it forms barium nitrate, carbon dioxide, and water.
- The reaction between HNO3 and BaCO3 is a double displacement reaction, also known as a metathesis reaction.
HNO3 + BaCO3 Ionic Equation
Explanation of the ionic equation for the reaction
When nitric acid (HNO3) reacts with barium carbonate (BaCO3), an interesting chemical reaction takes place. This reaction is commonly referred to as an acid-base reaction or a neutralization reaction. Let’s delve into the details of this reaction and understand the ionic equation that represents it.
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In the reaction between HNO3 and BaCO3, the nitric acid acts as the acid, while the barium carbonate acts as the base. The acid donates a proton (H+) to the base, resulting in the formation of water (H2O), carbon dioxide (CO2), and a salt called barium nitrate (Ba(NO3)2).
The balanced chemical equation for this reaction can be represented as follows:
HNO3 (aq) + BaCO3 (s) → Ba(NO3)2 (aq) + H2O (l) + CO2 (g)
Let’s break down this equation to understand the ionic species involved in the reaction.
- BaCO3 (s) + 2H+ (aq) → Ba2+ (aq) + H2O (l) + CO2 (g)
In this equation, the solid barium carbonate (BaCO3) dissociates into its ionic components when it comes into contact with the aqueous nitric acid (HNO3). The acid donates two protons (H+) to the carbonate ion (CO3^2-), resulting in the formation of water, carbon dioxide, and the barium ion (Ba^2+).
The carbonate ion (CO3^2-) is a polyatomic ion that has a charge of -2. When it reacts with the protons from the nitric acid, it forms water (H2O) and carbon dioxide (CO2). The barium ion (Ba^2+), on the other hand, remains in the solution as a spectator ion.
It’s important to note that this reaction is irreversible, meaning it proceeds in one direction only. Once the reaction has occurred, it cannot be easily reversed to regenerate the reactants.
This reaction is also exothermic, meaning it releases heat energy. The enthalpy change for this reaction is negative, indicating that it is an exothermic process.
In summary, the reaction between nitric acid (HNO3) and barium carbonate (BaCO3) results in the formation of barium nitrate (Ba(NO3)2), water (H2O), and carbon dioxide (CO2). The balanced ionic equation for this reaction is BaCO3 (s) + 2H+ (aq) → Ba2+ (aq) + H2O (l) + CO2 (g).
BaCO3 + HNO3 Ionic Equation
When barium carbonate (BaCO3) reacts with nitric acid (HNO3), an interesting chemical reaction takes place. This reaction can be represented by the following ionic equation:
BaCO3 (s) + 2H+ (aq) → Ba2+ (aq) + H2O (l) + CO2 (g)
Explanation of the ionic equation for the reverse reaction
Let’s break down the ionic equation to understand what is happening during this reaction.
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BaCO3 (s): This represents solid barium carbonate, which is the reactant in this equation. Barium carbonate is a white, crystalline compound commonly used in laboratory settings.
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2H+ (aq): The “aq” stands for aqueous, indicating that the nitric acid is dissolved in water. The “2H+” represents two hydrogen ions, which are the acidic component of nitric acid.
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Ba2+ (aq): This represents the barium ions that are formed when barium carbonate reacts with nitric acid. The “2+” indicates that the barium ion has a positive charge of 2.
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H2O (l): This represents liquid water, which is one of the products of this reaction. Water is formed when the hydrogen ions from nitric acid combine with hydroxide ions.
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CO2 (g): This represents carbon dioxide gas, which is another product of this reaction. Carbon dioxide is released when the carbonate ions from barium carbonate combine with hydrogen ions.
In this reaction, barium carbonate reacts with nitric acid to form barium ions, water, and carbon dioxide gas. It is important to note that this reaction is irreversible, meaning it proceeds in one direction only.
The formation of carbon dioxide gas makes this reaction particularly interesting. When the reaction takes place in a closed container, the carbon dioxide gas can build up pressure, causing the container to expand or even burst. Therefore, it is crucial to perform this reaction in a well-ventilated area or under controlled conditions in a laboratory.
To ensure safety, it is also important to wear appropriate protective gear, such as gloves and goggles, when handling chemicals like nitric acid and barium carbonate. Additionally, proper disposal methods should be followed for any waste generated during this reaction.
In summary, the ionic equation for the reaction between barium carbonate and nitric acid shows the formation of barium ions, water, and carbon dioxide gas. This reaction is irreversible and can have safety implications if not performed with caution.
Balanced Equation for HNO3 + BaCO3
When it comes to chemical reactions, balancing the equation is an essential step to ensure accuracy and consistency. In the case of the reaction between nitric acid (HNO3) and barium carbonate (BaCO3), balancing the equation is crucial to understand the stoichiometry and predict the products formed. Let’s take a closer look at the step-by-step process to balance this equation.
Step-by-step process to balance the equation
To balance the equation for the reaction between HNO3 and BaCO3, we need to ensure that the number of atoms of each element is the same on both sides of the equation. Here’s how we can achieve that:
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Start by writing the unbalanced equation: BaCO3 + HNO3 → Ba(NO3)2 + H2O + CO2
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Count the number of atoms for each element on both sides of the equation. In this case, we have:
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Ba: 1 on the left side, 1 on the right side
- C: 1 on the left side, 1 on the right side
- O: 3 on the left side, 5 on the right side
- H: 1 on the left side, 2 on the right side
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N: 1 on the left side, 2 on the right side
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Begin balancing the equation by adjusting the coefficients in front of each compound. Let’s start with the carbon dioxide (CO2) on the right side:
BaCO3 + HNO3 → Ba(NO3)2 + H2O + 1 CO2
- Next, let’s balance the oxygen (O) atoms. Since there are 3 oxygen atoms on the left side and 5 on the right side, we can balance them by adding a coefficient of 3 in front of the water (H2O):
BaCO3 + HNO3 → Ba(NO3)2 + 3 H2O + 1 CO2
- Now, let’s balance the hydrogen (H) atoms. There is 1 hydrogen atom on the left side and 6 on the right side. We can balance them by adding a coefficient of 6 in front of the nitric acid (HNO3):
BaCO3 + 6 HNO3 → Ba(NO3)2 + 3 H2O + 1 CO2
- Finally, let’s balance the nitrogen (N) atoms. There is 1 nitrogen atom on the left side and 2 on the right side. We can balance them by adding a coefficient of 2 in front of the barium nitrate (Ba(NO3)2):
BaCO3 + 6 HNO3 → 2 Ba(NO3)2 + 3 H2O + 1 CO2
And there you have it! The balanced equation for the reaction between nitric acid (HNO3) and barium carbonate (BaCO3) is:
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BaCO3 + 6 HNO3 → 2 Ba(NO3)2 + 3 H2O + CO2
By balancing the equation, we can determine the correct stoichiometry of the reactants and products involved in the reaction. This information is crucial for understanding the chemical properties and behavior of substances.
In the next section, we will explore the products formed in this reaction and their significance.
Properties and Characteristics of HNO3
Nitric acid, commonly known as HNO3, is a highly corrosive and strong acid. It is widely used in various industries and laboratory settings due to its unique properties and characteristics. In this section, we will explore why HNO3 is called nitric acid, discuss its strength compared to HNO2, and explore its applications and uses.
Explanation of why HNO3 is called nitric acid
The name “nitric acid” is derived from the Latin word “nitrum,” which means “native soda” or “niter.” It was first discovered by alchemists in the 13th century, who noticed that it was produced when niter (potassium nitrate) was treated with sulfuric acid. The term “nitric” refers to the presence of nitrogen in the acid.
Nitric acid is composed of one nitrogen atom (N) and three oxygen atoms (O), giving it the chemical formula HNO3. The presence of nitrogen in the compound is what distinguishes it from other acids. Nitric acid is a strong acid, meaning it readily donates a proton (H+) in aqueous solutions.
Discussion on the strength of HNO3 compared to HNO2
When comparing the strength of HNO3 to HNO2, it is important to consider their acid dissociation constants (Ka). The Ka value indicates the extent to which an acid dissociates in water, with a higher Ka value indicating a stronger acid.
HNO3 has a higher Ka value than HNO2, making it a stronger acid. This means that HNO3 dissociates more readily in water, releasing more hydrogen ions (H+) and leading to a more acidic solution. In contrast, HNO2 is a weaker acid and does not dissociate as readily.
Applications and uses of HNO3
Nitric acid has a wide range of applications and uses across various industries. Some of the notable applications include:
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Chemical manufacturing: Nitric acid is used in the production of fertilizers, explosives, dyes, and pharmaceuticals. It is a key component in the manufacturing of ammonium nitrate, which is a common fertilizer.
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Metallurgy: Nitric acid is used for metal etching and cleaning in the metallurgical industry. It is particularly effective in removing rust and corrosion from metal surfaces.
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Laboratory: Nitric acid is commonly used in laboratories for various purposes, such as pH adjustment, chemical analysis, and synthesis of other compounds.
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Cleaning agent: Due to its strong oxidizing properties, nitric acid is used as a cleaning agent for removing stains, mineral deposits, and organic residues.
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Explosives production: Nitric acid is a crucial component in the production of explosives, such as trinitrotoluene (TNT) and nitroglycerin.
It is important to note that nitric acid is highly corrosive and should be handled with caution. Safety precautions, such as wearing protective clothing and working in a well-ventilated area, should be followed when using nitric acid.
In conclusion, nitric acid (HNO3) is a highly corrosive and strong acid with various applications in industries and laboratories. Its name is derived from the presence of nitrogen in the compound, and it is stronger than HNO2. Understanding the properties and characteristics of nitric acid is essential for its safe and effective use in various applications.
Properties and Characteristics of BaCO3
Explanation of where BaCO3 is found
Barium carbonate (BaCO3) is a white, odorless powder that is commonly found in nature as the mineral witherite. It is named after William Withering, an English chemist who first discovered it in 1784. Witherite is primarily found in veins of lead ore, and it is often associated with other minerals such as galena (lead sulfide) and fluorite (calcium fluoride).
Witherite is not a widely available mineral, and its occurrence is relatively rare. It is mainly found in a few locations around the world, including England, Germany, Scotland, and the United States. In the United States, witherite deposits can be found in the states of Missouri, Tennessee, and Kentucky.
Discussion on the properties and uses of BaCO3
BaCO3 possesses several interesting properties that make it useful in various applications. Let’s explore some of these properties and discuss the different uses of BaCO3.
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Solubility: Barium carbonate is sparingly soluble in water, meaning it dissolves only to a limited extent. This property makes it useful in applications where controlled release of barium ions is required, such as in the production of ceramic glazes and specialty glasses.
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Thermal stability: BaCO3 is thermally stable at high temperatures. It does not decompose easily, making it suitable for use in industries that require heat-resistant materials. For example, it is used as a flux in the production of certain types of glass and ceramics.
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Reactivity: Barium carbonate is a weak base and can react with acids to form barium salts. This property is utilized in various chemical reactions and processes. For instance, it is commonly used in the laboratory as a source of barium ions in acid-base titrations.
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Optical properties: BaCO3 has optical properties that make it useful in the manufacturing of optical glasses and lenses. It can be used as a component in the production of optical filters and coatings.
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Radiopacity: Barium carbonate is radiopaque, meaning it is visible under X-ray imaging. This property makes it valuable in medical applications, such as in the diagnosis of gastrointestinal disorders. Barium sulfate, a compound derived from BaCO3, is commonly used as a contrast agent in X-ray examinations of the digestive system.
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Corrosion resistance: BaCO3 exhibits good resistance to corrosion, making it suitable for use in coatings and paints. It can provide protection to metal surfaces, preventing them from rusting or corroding.
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Other uses: BaCO3 is also used in the production of barium chemicals, pigments, and fireworks. It is sometimes employed as a flux in the smelting of certain metals, and it can also be used as a neutralizing agent in wastewater treatment processes.
In summary, BaCO3 is a versatile compound with various properties that make it valuable in different industries. Its solubility, thermal stability, reactivity, optical properties, radiopacity, corrosion resistance, and other characteristics contribute to its wide range of applications. Whether it is used in ceramics, glass manufacturing, medical imaging, or other fields, barium carbonate plays a significant role in numerous industrial processes.
Reaction between HNO3 and BaCO3
Explanation of the reaction process
When nitric acid (HNO3) reacts with barium carbonate (BaCO3), an interesting chemical reaction takes place. Let’s delve into the details of this reaction and understand the process behind it.
The reaction between HNO3 and BaCO3 is a type of acid-base reaction known as a neutralization reaction. In this reaction, the acid (HNO3) reacts with the base (BaCO3) to form a salt, water, and carbon dioxide gas.
Formation of Ba(NO3)2, H2O, and CO2
The balanced chemical equation for the reaction between HNO3 and BaCO3 is as follows:
2HNO3(aq) + BaCO3(s) → Ba(NO3)2(aq) + H2O(l) + CO2(g)
In this equation, two molecules of nitric acid (HNO3) react with one molecule of barium carbonate (BaCO3) to produce one molecule of barium nitrate (Ba(NO3)2), one molecule of water (H2O), and one molecule of carbon dioxide (CO2).
During the reaction, the hydrogen ions (H+) from the nitric acid combine with the carbonate ions (CO3^2-) from the barium carbonate to form water. Simultaneously, the barium ions (Ba^2+) from the barium carbonate combine with the nitrate ions (NO3^-) from the nitric acid to form barium nitrate.
Observation of effervescence and experiments to prove the evolution of CO2
One of the key observations during the reaction between HNO3 and BaCO3 is the effervescence or the release of gas. This gas is none other than carbon dioxide (CO2), which is produced as a byproduct of the reaction.
To prove the evolution of carbon dioxide gas, we can perform a simple experiment. We can collect the gas produced during the reaction in a test tube by inverting it over a beaker filled with water. As the reaction proceeds, we will observe bubbles rising and filling the test tube. These bubbles are a clear indication of the evolution of carbon dioxide gas.
To further confirm the presence of carbon dioxide, we can perform the limewater test. Limewater is a solution of calcium hydroxide (Ca(OH)2) in water. When carbon dioxide gas is passed through limewater, it forms a white precipitate of calcium carbonate (CaCO3). This confirms the presence of carbon dioxide in the gas evolved during the reaction.
In conclusion, the reaction between HNO3 and BaCO3 results in the formation of barium nitrate, water, and carbon dioxide gas. The effervescence observed during the reaction is due to the evolution of carbon dioxide. By conducting simple experiments, we can confirm the presence of carbon dioxide in the gas evolved.
Net Ionic Equation for HNO3 + BaCO3
In chemical reactions, it is often useful to write net ionic equations to focus on the essential species involved. Net ionic equations are simplified representations of reactions that exclude spectator ions, which are ions that do not participate in the reaction. Let’s explore how to derive the net ionic equation for the reaction between nitric acid (HNO3) and barium carbonate (BaCO3).
Explanation of how to derive the net ionic equation
To derive the net ionic equation, we first need to write the balanced chemical equation for the reaction between HNO3 and BaCO3. The balanced equation shows the reactants and products in their proper stoichiometric ratios. In this case, the balanced equation is:
HNO3 (aq) + BaCO3 (s) → Ba(NO3)2 (aq) + H2O (l) + CO2 (g)
Now, let’s break down the equation and identify the spectator ions. The nitric acid (HNO3) dissociates into H+ and NO3- ions in aqueous solution, while barium carbonate (BaCO3) dissociates into Ba2+ and CO3^2- ions. The Ba(NO3)2 formed from the reaction is soluble and dissociates into Ba2+ and NO3- ions as well.
The spectator ions in this reaction are the NO3- ions, which appear on both sides of the equation. Since they do not participate in any net change, we can eliminate them from the equation. This leaves us with the net ionic equation:
BaCO3 (s) + 2H+ (aq) → Ba2+ (aq) + H2O (l) + CO2 (g)
In the net ionic equation, we can see that the barium carbonate reacts with the hydrogen ions to form barium ions, water, and carbon dioxide. This equation focuses only on the species that undergo a chemical change, providing a clearer representation of the reaction.
It is important to note that the net ionic equation does not include the state of the reactants and products. The “(s)” and “(aq)” notations indicate the physical states of the substances (solid and aqueous, respectively) but are not included in the net ionic equation.
In summary, the net ionic equation for the reaction between nitric acid (HNO3) and barium carbonate (BaCO3) is:
BaCO3 (s) + 2H+ (aq) → Ba2+ (aq) + H2O (l) + CO2 (g)
By focusing on the essential species involved, the net ionic equation provides a concise representation of the chemical reaction. This equation is particularly useful in understanding acid-base reactions, precipitation reactions, and gas formation reactions.
HNO3 + BaCO3 as a Titration
Explanation of how HNO3 + BaCO3 can be used in a titration
In chemistry, a titration is a technique used to determine the concentration of a substance in a solution. It involves the gradual addition of a reagent of known concentration to a solution containing the analyte until the reaction between the two is complete. One such titration involves the combination of nitric acid (HNO3) and barium carbonate (BaCO3).
When HNO3 and BaCO3 are mixed together, a chemical reaction occurs. The nitric acid, which is a strong acid, reacts with the barium carbonate, a weak base, resulting in the formation of water, carbon dioxide gas, and a soluble salt called barium nitrate (Ba(NO3)2). The balanced equation for this reaction is as follows:
HNO3 + BaCO3 → Ba(NO3)2 + CO2 + H2O
During the titration, a solution of nitric acid is slowly added to a solution containing barium carbonate. The reaction between the two compounds is monitored using an indicator or pH meter. As the reaction progresses, the pH of the solution changes, indicating the completion of the reaction.
Apparatus and chemicals required
To perform the HNO3 + BaCO3 titration, several apparatus and chemicals are required. Here is a list of the essential items:
- Burette: A long, graduated glass tube with a stopcock at one end, used to accurately measure and dispense the nitric acid solution.
- Pipette: A glass or plastic tube used to measure a precise volume of the barium carbonate solution.
- Conical flask: A glass container with a conical shape, used to hold the barium carbonate solution during the titration.
- Indicator: A substance that changes color to indicate the completion of the reaction. In this titration, phenolphthalein is commonly used as an indicator.
- Nitric acid (HNO3) solution: A solution of known concentration, usually prepared by diluting a concentrated nitric acid solution with distilled water.
- Barium carbonate (BaCO3) solution: A solution of known concentration, prepared by dissolving a known mass of barium carbonate in distilled water.
Procedure for the titration
Performing the HNO3 + BaCO3 titration involves several steps. Here is a step-by-step procedure to carry out the titration:
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Prepare the solutions: Prepare the nitric acid solution and the barium carbonate solution by accurately measuring the required amounts of each chemical and dissolving them in distilled water. Ensure that the solutions are properly labeled to avoid confusion during the titration.
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Set up the apparatus: Set up the burette by filling it with the nitric acid solution. Make sure there are no air bubbles trapped in the burette and that the stopcock is closed. Place the conical flask on a white tile or a piece of white paper to easily observe any color changes during the titration.
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Add the indicator: Add a few drops of phenolphthalein indicator to the barium carbonate solution in the conical flask. The indicator will turn the solution pink.
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Perform the titration: Slowly open the stopcock of the burette to allow the nitric acid solution to flow into the conical flask. Swirl the flask gently to ensure thorough mixing. The pink color of the solution will gradually fade as the nitric acid reacts with the barium carbonate. Continue adding the nitric acid solution until the pink color disappears completely, indicating the completion of the reaction.
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Record the volume of nitric acid used: Note the initial and final readings on the burette to determine the volume of nitric acid solution used in the titration. This information will be used to calculate the concentration of the barium carbonate solution.
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Repeat the titration: Repeat the titration two more times to ensure accuracy and consistency of results. Take the average of the three titrations to obtain a more reliable value for the concentration of the barium carbonate solution.
By following this procedure, scientists and chemists can accurately determine the concentration of barium carbonate using the HNO3 + BaCO3 titration method. This technique is widely used in laboratories to analyze the concentration of various substances and is an essential tool in chemical analysis. Conclusion
In conclusion, the reaction between HNO3 and BaCO3 is a fascinating chemical process that results in the formation of Ba(NO3)2 and CO2. This reaction is commonly known as a double displacement reaction, where the cations and anions of two compounds switch places to form new compounds. HNO3, also known as nitric acid, is a strong acid that is commonly used in various industrial processes, while BaCO3, also known as barium carbonate, is a white crystalline solid. When these two substances come into contact, the nitric acid reacts with the barium carbonate, causing it to decompose and release carbon dioxide gas. The resulting compound, barium nitrate, is soluble in water and forms a clear solution. This reaction is not only interesting from a chemical standpoint, but it also has practical applications in various industries, such as the production of barium nitrate for fireworks and pyrotechnics. Overall, the reaction between HNO3 and BaCO3 is a prime example of the fascinating world of chemical reactions and their importance in our daily lives.
Frequently Asked Questions
Q: What is the chemical reaction between HNO3 and CaCO3?
The chemical reaction between HNO3 and CaCO3 can be represented by the equation HNO3 + CaCO3 → Ca(NO3)2 + CO2 + H2O.
Q: What is the balanced equation for the reaction between HNO3 and CaCO3?
The balanced equation for the reaction between HNO3 and CaCO3 is HNO3 + CaCO3 → Ca(NO3)2 + CO2 + H2O.
Q: What is the net ionic equation for the reaction between HNO3 and CaCO3?
The net ionic equation for the reaction between HNO3 and CaCO3 is H+ + CO3^2- → H2O + CO2.
Q: Why is HNO3 called nitric acid?
HNO3 is called nitric acid because it is an acid that contains the nitrate ion (NO3^-). It is a strong acid commonly used in laboratories and industries.
Q: When HNO3 is dissolved in water, what is it called?
When HNO3 is dissolved in water, it is called nitric acid. It forms a strong acidic solution due to the dissociation of HNO3 into H+ and NO3^- ions.
Q: Where is CaCO3 found?
CaCO3, also known as calcium carbonate, is a common mineral found in various natural sources such as limestone, chalk, and marble. It is also present in the shells of marine organisms.
Q: Why is HNO3 stronger than HNO2?
HNO3 is stronger than HNO2 because it has a higher tendency to donate a proton (H+). The presence of the nitrate ion (NO3^-) in HNO3 makes it more stable and more likely to dissociate in water.
Q: What are the products of the reaction between HNO3 and BaCO3?
The products of the reaction between HNO3 and BaCO3 are Ba(NO3)2, CO2, and H2O. This is a decomposition reaction where BaCO3 breaks down into its constituent ions and compounds.
Q: Does a chemical reaction occur when HNO3 dissolves in water?
Yes, a chemical reaction occurs when HNO3 dissolves in water. It undergoes dissociation, breaking down into H+ and NO3^- ions. This reaction is known as ionization.
Q: What are the safety precautions in handling HNO3 in the laboratory?
When handling HNO3 in the laboratory, it is important to wear appropriate protective equipment such as gloves, goggles, and a lab coat. HNO3 is corrosive and can cause severe burns, so it should be handled with care. It should also be stored in a well-ventilated area away from flammable substances.
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