Experiment 1: A student determined the empirical formula for magnesium by reacting magnesium with hydrochloric acid. The reaction produced hydrogen gas.
Experiment 2: Another experiment was carried out to study the effect of temperature on the rate of reaction between sodium thiosulfate solution and sulfuric acid. Increasing the temperature increased the rate of reaction.
Experiment 3: A student determined the percentage composition of oxygen in copper(II) nitrate through its decomposition reaction. The percentage of oxygen was calculated to be 51.06% based on the relative atomic masses and mole ratios in the balanced equation.
1. The document provides guidance for students taking their board practical exam, outlining 52 important points to remember and topics to study.
2. Students are instructed to show calculations for standard solutions, write balanced equations, describe procedures, record observations, and state results clearly in their exam.
3. The viva questions section lists over 40 topics that may be asked about in the oral exam, including theory, tests, reactions, and applications. Students are told to thoroughly learn the objectives, equations, and inferences related to these topics.
Permanganometry, iodometry in analytical technique, P K MANIP.K. Mani
This document provides information about various redox titration methods including permanganometry, dichromatometry, iodometry, and iodimetry. It discusses the standard redox potentials and reaction equations for potassium permanganate, potassium dichromate, iodine, and other oxidizing agents. The document also describes procedures for standardizing and preparing standard solutions of these titrants. Specific applications discussed include the titration of iron(II), nitrites, and arsenite.
Learning objectives
Introduction
Preparation of a standard solution used for redox titration
Oxidizing and reducing agents used in volumetric analysis
N/10 potassium permanganate preparation
N/10 potassium dichromate preparation
N/10 Iodine solution preparation
Examples of redox titrations
Conclusion
References
Applications of Redox Titrations - Reon SylvesterBebeto G
Redox titrations are used for a variety of applications in organic and inorganic analysis. Some examples include determining chemical oxygen demand to manage industrial wastewaters, determining water content in non-aqueous solvents using Karl Fischer titration, and measuring dissolved oxygen levels through Winkler's method. Iodometric and iodimetric titrations can be used to indirectly or directly determine oxidizing or reducing agents by exploiting the redox reaction between iodine and the analyte. Chlorination of public water supplies is also monitored through an indirect iodometric titration to measure total chlorine residual levels.
Redox titrations involve the oxidation-reduction reaction between an analyte solution and titrant. For example, a permanganometric titration can be used to estimate hydrogen peroxide or ferrous iron by titrating with potassium permanganate, a powerful oxidizer in acidic solutions. At the endpoint, the intensely colored permanganate ion is reduced to colorless manganese ions. An indicator is sometimes needed if the redox ion does not produce a color change at the endpoint. Common redox titrations involve permanganate or dichromate ions as oxidizing agents.
This document discusses various types of redox titrations and indicators used. It describes the preparation and standardization of common redox titrants like potassium manganate(VII), iodine, potassium dichromate, potassium bromate and ceric ammonium sulfate. Examples of titrations included are standardization of KMnO4 with sodium oxalate or sodium thiosulfate, iodine with sodium thiosulfate or arsenic trioxide, and sodium thiosulfate with potassium iodate. The document also covers redox indicators and conditions for iodometric titrations.
The document discusses redox titrations, which are volumetric methods of analysis that rely on the oxidation or reduction of an analyte using redox indicators or potentiometry. It covers changes in solution potential during titration, basic calculations, sample preparation methods, common titrants, and examples of determining the equivalence point potential in redox reactions. The document also provides details on potentiometric titration and using a platinum electrode to monitor the potential during titration instead of an indicator.
Redox titrations involve adjusting the oxidation state of the analyte using an auxiliary oxidizing or reducing agent so that it can be titrated. Common reagents used in redox titrations include potassium permanganate, sodium thiosulfate, cerium sulfate, and potassium dichromate. Redox titrations are used to determine various analytes like ascorbic acid, hydrogen peroxide, iron, and calcium compounds. The document discusses the principles and procedures of important redox titrations like permanganometry, iodimetry, cerimetry, and dichrometry. It also describes the determination of water using the Karl Fischer reagent and reaction.
1. The document provides guidance for students taking their board practical exam, outlining 52 important points to remember and topics to study.
2. Students are instructed to show calculations for standard solutions, write balanced equations, describe procedures, record observations, and state results clearly in their exam.
3. The viva questions section lists over 40 topics that may be asked about in the oral exam, including theory, tests, reactions, and applications. Students are told to thoroughly learn the objectives, equations, and inferences related to these topics.
Permanganometry, iodometry in analytical technique, P K MANIP.K. Mani
This document provides information about various redox titration methods including permanganometry, dichromatometry, iodometry, and iodimetry. It discusses the standard redox potentials and reaction equations for potassium permanganate, potassium dichromate, iodine, and other oxidizing agents. The document also describes procedures for standardizing and preparing standard solutions of these titrants. Specific applications discussed include the titration of iron(II), nitrites, and arsenite.
Learning objectives
Introduction
Preparation of a standard solution used for redox titration
Oxidizing and reducing agents used in volumetric analysis
N/10 potassium permanganate preparation
N/10 potassium dichromate preparation
N/10 Iodine solution preparation
Examples of redox titrations
Conclusion
References
Applications of Redox Titrations - Reon SylvesterBebeto G
Redox titrations are used for a variety of applications in organic and inorganic analysis. Some examples include determining chemical oxygen demand to manage industrial wastewaters, determining water content in non-aqueous solvents using Karl Fischer titration, and measuring dissolved oxygen levels through Winkler's method. Iodometric and iodimetric titrations can be used to indirectly or directly determine oxidizing or reducing agents by exploiting the redox reaction between iodine and the analyte. Chlorination of public water supplies is also monitored through an indirect iodometric titration to measure total chlorine residual levels.
Redox titrations involve the oxidation-reduction reaction between an analyte solution and titrant. For example, a permanganometric titration can be used to estimate hydrogen peroxide or ferrous iron by titrating with potassium permanganate, a powerful oxidizer in acidic solutions. At the endpoint, the intensely colored permanganate ion is reduced to colorless manganese ions. An indicator is sometimes needed if the redox ion does not produce a color change at the endpoint. Common redox titrations involve permanganate or dichromate ions as oxidizing agents.
This document discusses various types of redox titrations and indicators used. It describes the preparation and standardization of common redox titrants like potassium manganate(VII), iodine, potassium dichromate, potassium bromate and ceric ammonium sulfate. Examples of titrations included are standardization of KMnO4 with sodium oxalate or sodium thiosulfate, iodine with sodium thiosulfate or arsenic trioxide, and sodium thiosulfate with potassium iodate. The document also covers redox indicators and conditions for iodometric titrations.
The document discusses redox titrations, which are volumetric methods of analysis that rely on the oxidation or reduction of an analyte using redox indicators or potentiometry. It covers changes in solution potential during titration, basic calculations, sample preparation methods, common titrants, and examples of determining the equivalence point potential in redox reactions. The document also provides details on potentiometric titration and using a platinum electrode to monitor the potential during titration instead of an indicator.
Redox titrations involve adjusting the oxidation state of the analyte using an auxiliary oxidizing or reducing agent so that it can be titrated. Common reagents used in redox titrations include potassium permanganate, sodium thiosulfate, cerium sulfate, and potassium dichromate. Redox titrations are used to determine various analytes like ascorbic acid, hydrogen peroxide, iron, and calcium compounds. The document discusses the principles and procedures of important redox titrations like permanganometry, iodimetry, cerimetry, and dichrometry. It also describes the determination of water using the Karl Fischer reagent and reaction.
The document discusses redox reactions and equations. It provides examples of writing half-ionic equations for redox reactions involving complex ions such as permanganate (MnO4-), dichromate (Cr2O7 2-), and iodate (IO3-). It also discusses using titration to determine the stoichiometry of the reaction between iodine and thiosulfate ions.
Precipitation Titration, Complexometric Titration, Gravimetry and Diazotizati...DRx Rajveer Prajapati
This document discusses different analytical techniques including precipitation titration, complexometric titration, and gravimetry. It provides details on the estimation of sodium chloride through silver nitrate titration and the preparation of reagents. Complexometric titration is introduced as a method using chelating agents to form complex ions with metal ions, replacing solvated molecules. EDTA is commonly used and the document describes the complexation reaction between copper and ammonium ions. References are also included.
Formal potential analytical technique, P K MANIP.K. Mani
This document discusses formal potentials and their importance in redox titrations. It begins by explaining that standard potentials (E°) assume ideal conditions that are rarely present in practice. Formal potentials (E°') account for non-ideal conditions like varying activities of species. The document then provides examples of how complex formation in solutions can affect formal potentials compared to standard potentials. It discusses various redox indicators used in titrations and criteria for their selection, including their formal potentials relative to the analyte. In summary, the document outlines the concept of formal potentials, why they are more practical than standard potentials, and considerations for choosing redox indicators in titration analyses.
This document discusses various redox titration methods including permanganate, cerium, iodine, periodic acid, and sodium nitrite titrations. It provides details on relevant concepts such as redox equivalent weight calculations, types of indicators, and applications of different titration methods. Permanganate titrations can be direct, indirect, or residual and use potassium permanganate as the titrant. Cerium titrations use ammonium ceric sulfate and are advantageous over other methods. Sodium nitrite titration is used to determine primary aromatic amines. Periodic acid titration is used to determine polyhydroxy compounds by oxidation. Iodine titrations can be iodimetric or iod
This document discusses redox titration methods. It describes the Winkler method for determining dissolved oxygen in waste water and determining whether bacteria present are aerobic or anaerobic. The Karl Fischer method for determining water content is also outlined, using iodine, sulfur dioxide, and pyridine dissolved in methanol to quantitatively reduce iodine in the presence of water. Common oxidizing agents used in redox titrations include potassium permanganate, potassium bromate, cerium(IV), and potassium dichromate. Sodium thiosulfate is also described as a moderately strong standard reducing agent often used in indirect iodometric titrations to determine oxidizing agents.
IB Chemistry on Redox Titration, Biological Oxygen Demand and Redox.Lawrence kok
This document discusses titration methods including acid-base titration and redox titration. It provides details on common primary standard acids and bases used in titration as well as indicators. It also discusses the principles and reactions involved in acid-base titration and redox titration. Examples are given of various redox titrations to determine concentrations of substances like copper, iron, chlorine, vitamin C, and more. Procedures and calculations for determining percentage compositions of substances from redox titrations are outlined.
property of Tris(acetylacetonato)manganese(III) MUKULsethi5
this presentation useful for discussing #chemical and #physical property and application of ..
#Manganese(III)acetylacetonate
#Manganicacetylacetonate
#3-Penten-2-one,4-hydroxy-,manganese(3+) salt
#Mangan(3+)tris[(2Z)-4-oxo-2-penten-2-olat]
#3-Penten-2-one,4-hydroxy-,manganese(3+)salt,(3Z)-(3:1)
in this I discuss chemical and physical property, #spectra, application, #harmness etc
Potassium permanganate, potassium dichromate – one of the excellent tools of ...Istiqur Rahman
This document discusses pharmaceutical analysis and different types of titration methods. It focuses on redox titration and provides details about common oxidizing agents used - potassium permanganate and potassium dichromate. Potassium permanganate is highlighted as a stronger oxidizing agent compared to potassium dichromate due to its higher oxidation state of +7 and ability to oxidize a wider range of functional groups. Both oxidizing agents are compared in terms of their toxicity, with potassium dichromate noted as being more hazardous to health.
The document describes procedures for determining the available chlorine content in a bleaching powder sample using iodometric titration. Key steps include:
1. Standardizing a sodium thiosulfate solution by titrating it against a primary standard potassium dichromate solution in the presence of excess potassium iodide.
2. Dissolving a bleaching powder sample in water and liberating chlorine by adding acetic acid.
3. Reacting the liberated chlorine with excess potassium iodide to generate iodine, then titrating the iodine with the standardized sodium thiosulfate solution.
4. Calculating the available chlorine content based on the titration
The document provides information on writing chemical equations, including:
- Types of chemical equations like molecular, ionic, and net ionic equations.
- Common types of chemical reactions like combustion, synthesis, decomposition, single replacement, double replacement, and acid-base reactions.
- Key aspects of oxidation-reduction reactions involving electron transfer between reactants.
Qualitative tests for elements in organic compoundsAbigail Sapico
This document outlines qualitative tests for carbon, hydrogen, oxygen, nitrogen, halogens, and sulfur in organic compounds. Carbon and hydrogen are detected by heating compounds with CuO and observing the formation of calcium carbonate and water droplets. Oxygen is detected using ferrox paper or iron(III) hexathiocyanatoferrate(III) solutions, which turn red in the presence of oxygen. Nitrogen, halogens, and sulfur require sodium fusion to convert them to inorganic ions before qualitative testing, such as using Prussian blue for nitrogen or lead sulfide for sulfur.
This document discusses redox titrations. It begins by defining oxidation and reduction reactions. It then discusses different types of redox titrations including cerimetry, iodimetry, iodometry, bromatometry, dichrometry, and titration with potassium iodate. For each type of titration, the document describes the basic principles and provides some examples of applications. The document is presented by Miss Harshada R. Bafna and contains information on concepts, types, and specific techniques for various redox titration methods.
Learning objectives
Introduction
Types of solvents
Acidimetry in non aqueous medium
Alkalimetry in non aqueous medium
Estimation of Sodium benzoate and Ephedrine HCl
Applications of non aqueous titrations in pharmacy
Conclusion
Reference
Permanganate titration by krishna baokarkrishnabaokar
This document discusses potassium permanganate titration. It begins by outlining the key learning objectives, which include understanding why potassium permanganate is not used as a primary standard and how to prepare and standardize it. It then explains that permanganate behaves differently in acidic, neutral, and basic conditions when used as an oxidizing agent. The document also notes some disadvantages of using permanganate solutions and provides guidance on proper preparation, storage, and applications for titrating various analytes like ferrous ions, nitrites, and hydrogen peroxide.
This document describes how to determine the percentage of iron in a sample through a redox titration with potassium permanganate (KMnO4). It provides background on redox titrations and oxidation-reduction reactions. KMnO4 is first standardized against oxalic acid, since its concentration decreases over time. This allows the moles of KMnO4 used to be determined. The reaction of KMnO4 with Fe2+ is then used to find the moles of Fe2+ in the sample. From this, the mass and percentage of iron can be calculated.
Redox titrations involve the reaction of an oxidizing titrant with a reducing analyte. The document discusses the redox reaction of permanganate (KMnO4) with iron in an ore sample. It also provides the theory behind redox titrations, including Nernst equations that describe the cell potential before, at, and after the equivalence point of the titration reaction. The equivalence point potential can be calculated from the standard reduction potentials of the oxidized and reduced forms of the analyte and titrant.
Types of chemical reactions - Laboratory ActivityNarella Rebullar
These are synthesis, decomposition, combustion, single replacement and double replacement.
Laboratory Report.
University of Makati, Philippines.
III- BSE General Science
#Biochemistry #GeneralChemistry
Quantitative Determination of Total Hardness in Drinking Water by Complexomet...Nathan Nogales
This experiment aims to determine the total hardness of drinking water using a complexometric titration with EDTA. The standardization of EDTA is performed using a calcium carbonate standard. Reactions involving the calcium-EDTA and magnesium-EDTA complexes are discussed. The addition of magnesium chloride is meant to create a sharper titration endpoint but the amount added was insignificant compared to the EDTA. Analysis of a water sample from Viva found it to have a total hardness of 192.49 ppm CaCO3, which is 25.8% lower than the value claimed.
This document describes the precipitation method for determining the chloride ion concentration of a solution by titration with silver nitrate. Silver nitrate is added until all chloride ions are precipitated as silver chloride. Additional silver ions then react with potassium chromate indicator to form a red-brown silver chromate precipitate, signaling the endpoint. The method can be used to analyze water samples. It involves titrating aliquots of the sample with a standardized silver nitrate solution until concordant results are obtained.
Class-10-Chapter-01-Science-Chemistry-Chemical Reactions and Equations.pptxSoftcare Solution
Hello Friends,
Check out our new PowerPoint presentation on "Chemical Reactions and Equations" | Introduction to Chemical Reactions and Equations by softcare solution. We know these things in our daily life. Let’s them understand some concept about Chemical Reactions and Equations. At the end of this video, you will be able to understand the following points on Chemical Reactions and Equations: *******************************************************************
1. Chemical Reaction and Chemical Equation.
2. Types of Chemical Reaction.
3. Redox Reaction..
4. Corrosion and Rancidity.
*******************************************************************
NCERT solutions for Class 10th science.
****************************************************
We cover Complete Syllabus of All subjects
****************************************************
Our Study channel : For Business Enquiry - amitpandey.hrd@gmail.com
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✴️✔️ Do 𝐒𝐔𝐁𝐒𝐂𝐑𝐈𝐁𝐄 to the channel for more updates and hit that like button!
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This document discusses aqueous solutions and their properties. It defines key terms including solute, solvent, solution, electrolyte, and nonelectrolyte. It explains that solutions can be solid, liquid, or gas and describes different types of aqueous solutions. Common examples like sea water, vinegar, and sugar water are provided. The document also discusses solubility, dissociation, hydration, and precipitation reactions.
The document discusses redox reactions and equations. It provides examples of writing half-ionic equations for redox reactions involving complex ions such as permanganate (MnO4-), dichromate (Cr2O7 2-), and iodate (IO3-). It also discusses using titration to determine the stoichiometry of the reaction between iodine and thiosulfate ions.
Precipitation Titration, Complexometric Titration, Gravimetry and Diazotizati...DRx Rajveer Prajapati
This document discusses different analytical techniques including precipitation titration, complexometric titration, and gravimetry. It provides details on the estimation of sodium chloride through silver nitrate titration and the preparation of reagents. Complexometric titration is introduced as a method using chelating agents to form complex ions with metal ions, replacing solvated molecules. EDTA is commonly used and the document describes the complexation reaction between copper and ammonium ions. References are also included.
Formal potential analytical technique, P K MANIP.K. Mani
This document discusses formal potentials and their importance in redox titrations. It begins by explaining that standard potentials (E°) assume ideal conditions that are rarely present in practice. Formal potentials (E°') account for non-ideal conditions like varying activities of species. The document then provides examples of how complex formation in solutions can affect formal potentials compared to standard potentials. It discusses various redox indicators used in titrations and criteria for their selection, including their formal potentials relative to the analyte. In summary, the document outlines the concept of formal potentials, why they are more practical than standard potentials, and considerations for choosing redox indicators in titration analyses.
This document discusses various redox titration methods including permanganate, cerium, iodine, periodic acid, and sodium nitrite titrations. It provides details on relevant concepts such as redox equivalent weight calculations, types of indicators, and applications of different titration methods. Permanganate titrations can be direct, indirect, or residual and use potassium permanganate as the titrant. Cerium titrations use ammonium ceric sulfate and are advantageous over other methods. Sodium nitrite titration is used to determine primary aromatic amines. Periodic acid titration is used to determine polyhydroxy compounds by oxidation. Iodine titrations can be iodimetric or iod
This document discusses redox titration methods. It describes the Winkler method for determining dissolved oxygen in waste water and determining whether bacteria present are aerobic or anaerobic. The Karl Fischer method for determining water content is also outlined, using iodine, sulfur dioxide, and pyridine dissolved in methanol to quantitatively reduce iodine in the presence of water. Common oxidizing agents used in redox titrations include potassium permanganate, potassium bromate, cerium(IV), and potassium dichromate. Sodium thiosulfate is also described as a moderately strong standard reducing agent often used in indirect iodometric titrations to determine oxidizing agents.
IB Chemistry on Redox Titration, Biological Oxygen Demand and Redox.Lawrence kok
This document discusses titration methods including acid-base titration and redox titration. It provides details on common primary standard acids and bases used in titration as well as indicators. It also discusses the principles and reactions involved in acid-base titration and redox titration. Examples are given of various redox titrations to determine concentrations of substances like copper, iron, chlorine, vitamin C, and more. Procedures and calculations for determining percentage compositions of substances from redox titrations are outlined.
property of Tris(acetylacetonato)manganese(III) MUKULsethi5
this presentation useful for discussing #chemical and #physical property and application of ..
#Manganese(III)acetylacetonate
#Manganicacetylacetonate
#3-Penten-2-one,4-hydroxy-,manganese(3+) salt
#Mangan(3+)tris[(2Z)-4-oxo-2-penten-2-olat]
#3-Penten-2-one,4-hydroxy-,manganese(3+)salt,(3Z)-(3:1)
in this I discuss chemical and physical property, #spectra, application, #harmness etc
Potassium permanganate, potassium dichromate – one of the excellent tools of ...Istiqur Rahman
This document discusses pharmaceutical analysis and different types of titration methods. It focuses on redox titration and provides details about common oxidizing agents used - potassium permanganate and potassium dichromate. Potassium permanganate is highlighted as a stronger oxidizing agent compared to potassium dichromate due to its higher oxidation state of +7 and ability to oxidize a wider range of functional groups. Both oxidizing agents are compared in terms of their toxicity, with potassium dichromate noted as being more hazardous to health.
The document describes procedures for determining the available chlorine content in a bleaching powder sample using iodometric titration. Key steps include:
1. Standardizing a sodium thiosulfate solution by titrating it against a primary standard potassium dichromate solution in the presence of excess potassium iodide.
2. Dissolving a bleaching powder sample in water and liberating chlorine by adding acetic acid.
3. Reacting the liberated chlorine with excess potassium iodide to generate iodine, then titrating the iodine with the standardized sodium thiosulfate solution.
4. Calculating the available chlorine content based on the titration
The document provides information on writing chemical equations, including:
- Types of chemical equations like molecular, ionic, and net ionic equations.
- Common types of chemical reactions like combustion, synthesis, decomposition, single replacement, double replacement, and acid-base reactions.
- Key aspects of oxidation-reduction reactions involving electron transfer between reactants.
Qualitative tests for elements in organic compoundsAbigail Sapico
This document outlines qualitative tests for carbon, hydrogen, oxygen, nitrogen, halogens, and sulfur in organic compounds. Carbon and hydrogen are detected by heating compounds with CuO and observing the formation of calcium carbonate and water droplets. Oxygen is detected using ferrox paper or iron(III) hexathiocyanatoferrate(III) solutions, which turn red in the presence of oxygen. Nitrogen, halogens, and sulfur require sodium fusion to convert them to inorganic ions before qualitative testing, such as using Prussian blue for nitrogen or lead sulfide for sulfur.
This document discusses redox titrations. It begins by defining oxidation and reduction reactions. It then discusses different types of redox titrations including cerimetry, iodimetry, iodometry, bromatometry, dichrometry, and titration with potassium iodate. For each type of titration, the document describes the basic principles and provides some examples of applications. The document is presented by Miss Harshada R. Bafna and contains information on concepts, types, and specific techniques for various redox titration methods.
Learning objectives
Introduction
Types of solvents
Acidimetry in non aqueous medium
Alkalimetry in non aqueous medium
Estimation of Sodium benzoate and Ephedrine HCl
Applications of non aqueous titrations in pharmacy
Conclusion
Reference
Permanganate titration by krishna baokarkrishnabaokar
This document discusses potassium permanganate titration. It begins by outlining the key learning objectives, which include understanding why potassium permanganate is not used as a primary standard and how to prepare and standardize it. It then explains that permanganate behaves differently in acidic, neutral, and basic conditions when used as an oxidizing agent. The document also notes some disadvantages of using permanganate solutions and provides guidance on proper preparation, storage, and applications for titrating various analytes like ferrous ions, nitrites, and hydrogen peroxide.
This document describes how to determine the percentage of iron in a sample through a redox titration with potassium permanganate (KMnO4). It provides background on redox titrations and oxidation-reduction reactions. KMnO4 is first standardized against oxalic acid, since its concentration decreases over time. This allows the moles of KMnO4 used to be determined. The reaction of KMnO4 with Fe2+ is then used to find the moles of Fe2+ in the sample. From this, the mass and percentage of iron can be calculated.
Redox titrations involve the reaction of an oxidizing titrant with a reducing analyte. The document discusses the redox reaction of permanganate (KMnO4) with iron in an ore sample. It also provides the theory behind redox titrations, including Nernst equations that describe the cell potential before, at, and after the equivalence point of the titration reaction. The equivalence point potential can be calculated from the standard reduction potentials of the oxidized and reduced forms of the analyte and titrant.
Types of chemical reactions - Laboratory ActivityNarella Rebullar
These are synthesis, decomposition, combustion, single replacement and double replacement.
Laboratory Report.
University of Makati, Philippines.
III- BSE General Science
#Biochemistry #GeneralChemistry
Quantitative Determination of Total Hardness in Drinking Water by Complexomet...Nathan Nogales
This experiment aims to determine the total hardness of drinking water using a complexometric titration with EDTA. The standardization of EDTA is performed using a calcium carbonate standard. Reactions involving the calcium-EDTA and magnesium-EDTA complexes are discussed. The addition of magnesium chloride is meant to create a sharper titration endpoint but the amount added was insignificant compared to the EDTA. Analysis of a water sample from Viva found it to have a total hardness of 192.49 ppm CaCO3, which is 25.8% lower than the value claimed.
This document describes the precipitation method for determining the chloride ion concentration of a solution by titration with silver nitrate. Silver nitrate is added until all chloride ions are precipitated as silver chloride. Additional silver ions then react with potassium chromate indicator to form a red-brown silver chromate precipitate, signaling the endpoint. The method can be used to analyze water samples. It involves titrating aliquots of the sample with a standardized silver nitrate solution until concordant results are obtained.
Class-10-Chapter-01-Science-Chemistry-Chemical Reactions and Equations.pptxSoftcare Solution
Hello Friends,
Check out our new PowerPoint presentation on "Chemical Reactions and Equations" | Introduction to Chemical Reactions and Equations by softcare solution. We know these things in our daily life. Let’s them understand some concept about Chemical Reactions and Equations. At the end of this video, you will be able to understand the following points on Chemical Reactions and Equations: *******************************************************************
1. Chemical Reaction and Chemical Equation.
2. Types of Chemical Reaction.
3. Redox Reaction..
4. Corrosion and Rancidity.
*******************************************************************
NCERT solutions for Class 10th science.
****************************************************
We cover Complete Syllabus of All subjects
****************************************************
Our Study channel : For Business Enquiry - amitpandey.hrd@gmail.com
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Thank you for watching. If you liked the video, consider subscribing :)
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(Turn on your notification 🔔 to get all updates before anyone!!)
This document discusses aqueous solutions and their properties. It defines key terms including solute, solvent, solution, electrolyte, and nonelectrolyte. It explains that solutions can be solid, liquid, or gas and describes different types of aqueous solutions. Common examples like sea water, vinegar, and sugar water are provided. The document also discusses solubility, dissociation, hydration, and precipitation reactions.
This document contains a 50-question multiple choice test on chemistry concepts. The questions cover topics like chemical formulas, periodic trends, chemical bonding, stoichiometry, acid-base reactions, and organic chemistry. Each question is followed by 4 answer choices labelled A, B, C, or D.
Chemistry edexcel as unit 1 chapter 1 chemical quantities_v0.03Paul Hill
Here are the key steps and observations from the experiment:
- Weigh out 0.56g of iron powder, which is 0.01 moles
- Add to excess copper(II) sulfate solution
- A displacement reaction occurs, producing copper metal
- Filter, wash, dry the copper product
- Weigh the copper produced
- If equation 1 is correct, the mass of copper should be 0.63g (0.01 moles of Cu)
- However, the actual mass obtained is higher, indicating equation 2 is correct
- Equation 2 involves a change in oxidation state of iron from 0 to +3, a redox reaction
So in summary, the experiment shows the reaction involves a redo
1) A solution is a homogeneous mixture of two or more substances, where the solute is present in smaller amounts than the solvent.
2) An electrolyte is a substance that, when dissolved in water, allows the solution to conduct electricity through the formation of ions, while a nonelectrolyte does not form ions and the solution cannot conduct electricity.
3) Titrations involve slowly adding a solution of known concentration to another solution of unknown concentration until the chemical reaction between them is complete, as indicated by an indicator, and can be used to determine concentrations in acid-base and redox reactions.
This document provides information about salts in chemistry. It defines a salt as an ionic substance formed by the replacement of hydrogen ions in an acid by metal ions or ammonium ions. Salts consist of cation and anion parts from the base and acid respectively. The document also includes tables and diagrams showing solubility rules for common salts and their reactions with heat. It describes methods for preparing and purifying soluble and insoluble salts, as well as qualitative analysis of salts through observation of physical properties and chemical tests.
This document provides information on chemical equations and oxidation-reduction reactions. It defines key concepts like oxidation, reduction, oxidizing agents, reducing agents and oxidation numbers. Examples of different types of chemical reactions like combination, decomposition, displacement and combustion are outlined. Steps for writing and balancing chemical equations are described. Oxidation-reduction reactions are explained along with biological examples of electron transfer processes. Specific equations are given and identified as oxidation or reduction reactions.
This document discusses several chemical reactions and concepts:
1) It describes the dehydration of ethanol to produce ethene, and the test to identify ethene using bromine.
2) It discusses the oxidation of ethanol to produce ethanoic acid, including the chemical equation and properties of ethanoic acid.
3) It covers several homologous series including alkanes, alkenes, alcohols, carboxylic acids, and esters.
The document discusses several chemistry concepts and experiments including:
1) Testing for carbon dioxide by adding acid to carbonates which produces carbon dioxide gas.
2) Using flame tests to identify metal ions based on the color of flames they produce.
3) Metal ions forming precipitates when sodium hydroxide is added, such as calcium ions forming calcium hydroxide.
4) Experiments to test for chloride, sulfate, ammonium, nitrate, bromide and iodide ions using chemical reactions and indicators.
This document contains a SPM 2004 exam paper for Chemistry with 40 multiple choice questions testing various chemistry concepts. The questions cover topics such as states of matter, properties of substances like acids and bases, chemical equations and reactions including combustion, electrolysis, and displacement. Sub-atomic particles, relative atomic mass, and mole concept are also assessed. Diagrams of experimental set-ups and molecular structures are provided with some questions.
Revision on acid base and salt = with answersMRSMPC
This document provides information about chemistry revision on acids, bases and salts. It discusses soluble and insoluble salts such as chlorides, sulphates and nitrates. It also describes methods for preparing soluble and insoluble salts, including the titration and solid acid methods. The document further discusses the preparation of copper(II) sulphate through the reaction of copper(II) oxide with sulphuric acid, and provides chemical tests to identify the copper and sulphate ions.
Nitric acid and hydrochloric acid are strong acids that are highly soluble in water. Nitric acid is produced commercially via the Ostwald process, which involves catalytic oxidation of ammonia to produce nitric oxide, which is then oxidized to nitrogen dioxide and absorbed in water to form nitric acid. Hydrochloric acid is produced via electrolysis of sodium chloride to produce chlorine, which is then combined with hydrogen to form hydrochloric acid. Both acids are colorless liquids with pungent odors that are widely used in industry, such as in fertilizer production and cleaning applications. Proper storage of the acids requires acid resistant containers and secondary containment to mitigate hazards.
This document provides information on stoichiometry, which involves using mole ratios from balanced chemical equations to calculate mass relationships between substances in a chemical reaction. It outlines the steps to solve stoichiometry problems, which include writing a balanced equation, identifying known and unknown quantities, setting up mole ratio conversion factors between moles of reactants and products, and checking the answer. Key concepts discussed include the mole ratio from coefficients in a balanced equation, molar mass to convert between moles and grams, and the molar volume used to calculate liters of gas at standard temperature and pressure.
The document provides the marking scheme for an exam on acids, bases, and salts. It includes the questions asked, expected answers, and marks allocated for each part. The marking scheme covers topics like neutralization reactions, properties of acids and bases, concentration calculations using titration, identification of cations and anions in salts, and experiments related to acid-base and salt reactions. It aims to clearly outline the requirements to score full marks for the exam questions.
This document discusses precipitation reactions and provides information on:
- Types of precipitation reactions and how to determine if a product is soluble or insoluble using solubility rules.
- How to predict if a precipitation reaction will occur by assigning oxidation states, writing molecular, complete ionic, and net ionic equations.
- How to perform stoichiometric calculations involving precipitation reactions, including determining moles or mass of reactants and products.
- Key concepts related to solutions including molarity, using molarity in calculations, dilution, and limiting reagents.
This document provides information about acids and bases, including their properties and reactions. It defines acids as substances that produce hydrogen ions in aqueous solution, and bases as metal oxides or hydroxides. Strong acids are fully ionized in water, while weak acids are only partially ionized. The strength of an acid does not relate to its concentration. Common uses of acids include battery electrolytes, rust removal, and food preservation.
The document outlines methods for preparing specified salts through various chemical reactions. It discusses using precipitation reactions when salts are insoluble and acid-base reactions when salts contain sodium, ammonium, or potassium ions. The document provides examples of reacting acids with metal oxides, metals, and metal carbonates to produce salts. It also gives guidance on purification techniques like filtration, washing, drying, heating, cooling/crystallization after reactions. Finally, it includes 5 examples of stoichiometric calculations to determine moles, masses or volumes of reactants and products in salt forming reactions.
1. The document discusses several chemical processes and concepts including the Haber process, vanadium(V) oxide, ionic bonding, rates of reaction, electrolysis, and acid-base reactions.
2. It provides information on experimental procedures like determining the rate of a reaction between zinc and hydrochloric acid, and preparing zinc sulfate crystals from zinc carbonate and sulfuric acid.
3. Key concepts explained include the empirical and molecular formulas of an unknown compound determined through combustion analysis, the reactivity of potassium compared to sodium, and exothermic and endothermic reactions illustrated through temperature changes.
1. The document discusses redox (reduction-oxidation) reactions in terms of oxidation and reduction processes. It defines oxidation as a loss of electrons, hydrogen, or an increase in oxidation number, and reduction as a gain of electrons, hydrogen, or a decrease in oxidation number.
2. An example of an apple browning is provided, where the exposed iron in damaged apple cells reacts with oxygen and enzymes through oxidation. Tips are given to prevent browning, such as coating slices in acid.
3. Redox reactions are defined as those where oxidation and reduction occur simultaneously, often involving the transfer of electrons between reactants. Oxidizing agents undergo reduction while reducing agents undergo oxidation.
This document contains descriptions and diagrams of several chemical reactions and experiments:
1) A reaction between magnesium and copper chloride produces magnesium chloride and copper.
2) Precipitation of silver chloride is achieved through a reaction of silver nitrate and sodium chloride.
3) Copper(II) oxide reacts with sulfuric acid to produce copper(II) sulfate and water.
4) Heating zinc carbonate produces zinc oxide and carbon dioxide, and the gas changes limewater to chalky.
Revision on consumer, r te, thermo and carbon compoundMRSMPC
The document describes two experiments where zinc reacts with two different acids, labeled P and Q. In Experiment I, zinc reacts with Acid P, producing zinc chloride and hydrogen gas, while the temperature of the mixture increases. In Experiment II, zinc reacts with Acid Q, producing zinc sulfate and hydrogen gas, and again the temperature increases. The document provides data from Experiments I and II to study the rate of reaction between zinc and the two acids.
The document discusses different types of food additives and their functions, including:
- Colouring agents which restore colour to food
- Preservatives like benzoic acid and sodium nitrite which destroy microorganisms
- Antioxidants like ascorbic acid which prevent oxidation of food
- Flavouring agents like monosodium glutamate which give or enhance flavour
- Stabilisers and thickeners like pectin and gelatin which prevent separation and thicken foods
It also lists examples of specific additives that fall into each category.
The document discusses different types of food additives and their functions, including:
- Colouring agents which restore colour to food
- Preservatives like benzoic acid and sodium nitrite which destroy microorganisms
- Antioxidants like ascorbic acid which prevent oxidation of food
- Flavouring agents like monosodium glutamate which give or enhance flavour
- Stabilisers and thickeners like pectin and gelatin which prevent separation and thicken foods
It also lists examples of traditional medicines like ginger and garlic and their functions, as well as types and uses of modern medicines including analgesics, antibiotics, and psychotherapeutic drugs.
Revision on consumer, r te, thermo and carbon compoundMRSMPC
The document describes two experiments where zinc reacts with two different acids, labeled P and Q. In Experiment I, zinc reacts with Acid P, producing zinc chloride and hydrogen gas, while the temperature of the mixture increases. In Experiment II, zinc reacts with Acid Q, producing zinc sulfate and hydrogen gas, and again the temperature increases. The document provides data from Experiments I and II to study the rate of reaction between zinc and the two acids.
1) The document provides information about a chemistry pre-trial exam, including multiple choice questions about particles, physical properties, chemical reactions, and rates of reaction.
2) Section two involves questions about electrolysis of copper(II) sulfate solution and the products formed at the anodes and cathodes using different electrode materials.
3) Section three describes laboratory activities to prepare a salt through a reaction between zinc oxide and nitric acid, including excess reactants, products, and apparatus setup.
4) Section four involves questions about heat of neutralization reactions, including energy level diagrams and temperature change calculations.
5) Section five provides information about homologous series, including molecular formulas, boiling points, and
1. The document contains 20 multiple choice questions about chemistry concepts such as particles, states of matter, chemical reactions, rates of reaction, food additives, and acids and bases.
2. The questions cover topics like the types of particles that make up different substances, using carbon-14 to estimate the age of artifacts, interpreting temperature-time graphs, identifying reactants and products in chemical equations, factors that affect reaction rates, functions of food additives, and using bases to relieve acid indigestion.
3. Several questions also involve identifying the correct matches between concepts like transition metal catalysts and their industrial uses, common alloys and their main components, and calculating percentages of elements in compounds.
This document contains a chemistry test with three parts:
Part A contains 10 multiple choice questions about chemistry concepts like the periodic table, electron configuration, and chemical reactions.
Part B contains multi-part questions about specific elements and compounds. It asks students to identify elements on the periodic table, draw electron configurations, and describe chemical reactions and electrolysis.
Part C contains experimental questions about electrolysis using different apparatus set ups and solutions. It requires identifying electrodes and ions, writing chemical equations, and describing observations at the electrodes.
The test is designed to evaluate students' understanding of fundamental chemistry concepts and their ability to apply that knowledge to analyze experiments and unknowns. It provides context clues and diagrams to help students
Revision for salt, electrochemistry, carbon compounds , thermochemistryMRSMPC
The document discusses several chemical formulas, equations, and calculations including the heat of precipitation of barium sulfate from a mixture of potassium sulfate and barium chloride solutions. It also addresses the properties and production of natural rubber from latex and how treating rubber with sulfur through the process of vulcanization improves its properties for uses such as in tires and gloves.
Soap and detergent, medicine , food additives consumer 2011-edited-2MRSMPC
This document provides information about chemicals for consumers. It discusses soaps, detergents, and their properties. Soap is the salt formed from fatty acids and alkalis. Their general formula is RCOO-Na+. Detergents are salts formed from alkyl sulfates and alkalis. Soap and detergent both lower surface tension and emulsify oils to suspend dirt particles in water. Detergents are more effective than soap in hard water since they do not form insoluble precipitates. The document also discusses food additives and their functions like dyes, preservatives, flavorings, and stabilizers. Finally, it covers modern medicines like analgesics, antibiotics, and psychotherapeutic drugs along with their examples,
fats and natural rubber module 3 carbon compounds with answersMRSMPC
The document discusses key concepts related to fats and oils including:
1) Fats are solid at room temperature and found in animals, while oils are liquid at room temperature and found in plants.
2) Fat molecules contain saturated fatty acids that have no carbon-carbon double bonds, while unsaturated fatty acids contain at least one double bond.
3) Glycerol is an alcohol that reacts with fatty acids to form fat or oil molecules through esterification reactions.
1) The document provides formulas and examples of strong acids, weak acids, strong bases and weak bases.
2) It describes 4 chemical properties of acids: reaction with metals, oxides, alkalis and carbonates.
3) Beaker A shows acidic properties due to hydrogen chloride ionizing in water to form H+ ions, while Beaker B shows no change.
Discussion on rate of reaction =for quiz 1 and 2MRSMPC
The document discusses factors that affect the rate of chemical reactions including temperature, concentration, surface area, and the use of catalysts. It explains how increasing temperature, concentration, or surface area increases the frequency of particle collisions, leading to a faster reaction rate. Catalysts provide an alternative reaction pathway with lower activation energy, allowing more particles to have sufficient energy for reaction. Examples are provided of calculating reaction rates from graphs and sketching how rate curves would change with different conditions.
7. • Name the process represented by the
equation.
• saponification
• Why are the soap molecules not effective in
hard water?
• soap ion react with Ca2+
/ Mg2+
ion
• to produce an insoluble salt / solid / scum
9. • Which pair of atoms are isotopes?
• P and R
• Give the reason for your answer in (a)(i).
• Both atoms have same number of protons but
different number of neutrons // Both atoms
have same proton number but different
nucleon number
10. Draw the electron arrangement for atom Q.
When metals of Group 1 react with water, bubbles of colourless gas are evolved.
Diagram 2 shows the reaction of the first three alkali metals with water
in three different beakers labeled as W, X and Y.
X
W X
Y
In which beaker shows the reaction of
potassium with water?
11. • Based on Diagram 2, name the gas evolved when
metals of
• Group1 react with water.
• hydrogen gas
• State one observation when a few drops of
phenolphthalein indicator is added into the
solution formed in W, X and Y.
• Explain your answer.
• Colourless solution turns pink
• The reaction produces alkaline solution
• a: presence of OH-
12. • Complete the following chemical equation:
• Lengkapkan persamaan kimia berikut:
• …… Na + …… H2O → ………..… + …………..
• Based on Diagram 2, what can you infer about
the density of Group 1 metals compared to
water?
• density of Group 1 metals are lower than the
density of water // less dense than water
13. Molten lead(II) oxide
Carbon F
Heat
Panaskan
Carbon G
Carbon L
Silver nitrate solution
Larutan argentum nitrat
Carbon M
Diagram 3.1
Rajah 3.1
Diagram 3.2
Rajah 3.2
What is meant by electrolyte?
A compound/substance that can conduct electricity in molten state or aqueous solution and undergoes chemical changes
14. • Name the product formed at electrode G.
• lead
• Write the half equation for the reaction that
occurs at electrode F.
• 2 O2-
O2 + 4e
• State the ions present in silver nitrate solutio
Ag+
, H+
, NO3
-
, OH-
(a: name of ions)
• n.
15. • What would you observe at carbon electrode
M?
• grey solid/ deposit
• Explain your answer in (c)(ii).
• Silver is produced// Ag+
is discharged
• Because silver ion is lower than hydrogen
ion in the Electrochemical Series
16. • Describe how you can verify the product formed
at carbon electrode L.
• Insert a glowing wooden splinter into the test
tube
• Glowing splinter will rekindles / relights /
reignites
• State one application of electrolysis in industries.
• Extraction of reactive metal / electroplating /
purification of metal
17. Type of acid
Jenis asid
Example
Contoh
pH
Strong acid
Asid kuat
Hydrochloric acid
Asid hidroklorik
1.0
Weak acid
Asid lemah
Oxalic acid
Asid oksalik
3.0
What is meant by a weak acid?
Acid (substance) which ionises partially// has lower degree
of dissociation in water to produce low concentration of
H+
ion
18. • Why is the pH value of hydrochloric acid lower
than the pH value of oxalic acid?
• The concentration of hydrogen ions in
hydrochloric acid is higher
• The higher the concentration of hydrogen
ions, the lower the pH value
19. Hydrochloric acid
Asid hidroklorik
25 cm3
of 0.1 mol dm-3
sodium hydroxide
25 cm3
natrium hidroksida 0.1 mol dm-3
Write a chemical equation to represent the
reaction.
HCl + NaOH NaCl + H2
O
20. • 25 cm3
of 0.1 mol dm-3
sodium hydroxide solution is required to react
completely with 12.50 cm3
of dilute hydrochloric acid.
• Calculate the molarity of the dilute hydrochloric acid used.
• ) No of mole of NaOH = 0.1 (25)
• 1000
• = 0.0025 mol
•
• 1 mol of NaOH react completely with 1 mol of HCl
• 0.0025 mol of NaOH react completely with 0.0025 mol HCl
•
• Molarity of HCl = 0.0025 x 1000
• 12.5
• = 0.2 mol dm-3
25 cm3
of 0.1 mol dm-3
sodium hydroxide solution is required to react
completely with 12.50 cm3
of dilute hydrochloric acid.
Calculate the molarity of the dilute hydrochloric
acid used.
21. Zinc oxide
Zink oksida
+ HCl
Step 1
Langkah 1
Solution N
Larutan N
Zinc carbonate
Zink karbonat
Sodium chloride
Natrium klorida
+
Step 2
Langkah 2
+ S
Name the following solutions:
Namakan larutan- larutan berikut:
4(c)(i)
N: ……………………..………
S: ..
……………………………
N : Zinc chloride
S : Sodium carbonate
r: formula
22. • State the type of reaction in Step 2.
• double decomposition/ precipitation
23. Burning lithium
Litium yang terbakar
Chlorine gas
Gas klorin
Write a chemical equation for the reaction.
) 2Li + Cl2 2LiCl
State the changes in oxidation number for
chlorine
0 to -1
Explain why lithium acts as the reducing agent
in terms of electron transfer.
) lithium atom loses // donates electron // is
electron donor
24. Bromine water
Air bromin
Potassium iodide solution
Larutan kalium iodida
A small amount of 1,1,1-trichloroethane liquid
is added to the product in the test tube and
the mixture is shaken.
What is the colour of 1,1,1-trichloroethane
layer?
purple
Write the ionic equation for the reaction
between bromine and potassium iodide
solution. Br2
+ 2I-
2Br -
+ I2
25. • What is the role of bromine water in this
reaction?
• oxidizing agent
26. Dry hydrogen gas
Gas hidrogen kering
Heat
Panaskan
Metal oxide powder
Serbuk oksida logam
27. Experiment
Eksperimen
Result
Keputusan
Hydrogen + oxide of metal J
Hidrogen + oksida logam J
Metal oxide powder glows brightly.
Black powder turned brown.
Serbuk oksida logam berbara dengan terang.
Serbuk hitam menjadi perang.
Hydrogen + oxide of metal T
Hidrogen + oksida logam T
No reaction.
Powder turns yellow when hot and white
when cold.
Tiada tindak balas.
Serbuk bertukar kuning apabila panas dan
putih apabila sejuk.
Hydrogen + magnesium oxide
Hidrogen + magnesium oksida
No reaction.
White powder remained.
Tiada tindak balas.
Serbuk putih kekal.
Suggest a name for metal T. ) zinc
28. • Arrange the reactivity of J, T, Magnesium and
Hydrogen in ascending order.
• J, H , T(zinc), magnesium
• Based on the observations, explain how you obtain the
arrangement
• Reaction occur between H2 and oxide J, so, H is
• more reactive than J
• 2. No reaction occur between H2 and oxide T and
• between H-2 and magnesium oxide
• so, H2 is less reactive than Mg and T
• 3. Magnesium is more reactive than zinc
29. Compound K Compound L
Write the general formula for the homologous
series of compound K.
CnH2n+1COOH, n= 0,1,2, ….
30. • Name compound L.
• Methyl propanoate
• Compare two physical properties of
compounds K and L by completing the
following table:
Physical property
Sifat fizik
Compound K
Sebatian K
Compound L
Sebatian L
Odour
Bau
Solubility
Keterlarutan
31. Properties Compound K Compound L
Odour pungent smell sweet/fruity smell
Solubility soluble in water //
soluble in organic
solvent
not soluble in water //
soluble in organic
solvent
32. • Compound L can be produced from K in the laboratory.
• Sebatian L boleh dihasilkan dari K di dalam
makmal.
•
• (i) Describe briefly how this process can be carried
out.
• Add methanol to compound K (propanoic acid) in a
boiling tube
• Add a few drops of concentrated sulphuric acid
• Heat gently / warm the mixture
33. • Write the equation for the reaction
• C2H5COOH + CH3OH C2H5COOCH3 + H2O
• Compound K is produced from the oxidation
of propanol.
• Draw all possible isomers for propanol.
34. t1 t2 Time,s
Masa
Volu
me of
gas,
cm3
Isipad
u gas
Compare the rate of reaction at t1 and t2.
Based on the graph, explain your answer.
Rate of reaction at t1
is higher than t2
2. because gradient at t1
is greater than t2
3. The concentration of hydrochloric acid decreases with
time
35. 2HCl + CaCO3
CaCl2
+ CO2
+ H2
O
The following chemical equation shows the reaction between calcium carbonate and hydrochloric acid.
Persamaan kimia berikut menunjukkan tindak balas antara kalsium karbonat dengan asid hidroklorik.
Determine the mass of calcium carbonate needed in the reaction if 480 cm3
of gas is released at room
condition.
(The molar volume of gas at room condition: 24 dm3
mol-1
,
Relative atomic mass: C = 12 g, O= 16 g, Ca = 40 g)
No of mole of gas = 480 / 24000 = 0.02 mol
From equation,
1 mol of CO2
is produced from 1 mol of CaCO3
0.02 mol of CO2
is produced from 0.02 mol of CaCO3
Mass of CaCO3
= 0.02 [40 + 12 + (16)(3)] g mol-1
= 2.0 g
36. Two experiments are carried out to study the effect of the size of calcium carbonate on the rate of reaction.
Dua eksperimen dijalankan untuk mengkaji kesan saiz kalsium karbonat ke atas kadar tindak balas.
Experiment I : 1 g of calcium carbonate chips react with 20.0 cm3
of 0.2 mol dm-3
hydrochloric acid.
Eksperimen I : 1 g ketulan kalsium karbonat bertindak balas dengan 20.0 cm3
asid hidroklorik 0.2 mol dm-3
.
Experiment II : 1 g of calcium carbonate powder react with 20.0 cm3
of 0.2 mol dm-3
hydrochloric acid.
Time / s
Masa/ s 0 60 120 180 240 300 360
Volume
of gas / cm3
Isipadu
gas / cm3
Experiment
I 0.00
25.9
0
33.0
0
37.0
0
40.5
0
42.0
0
42.0
0
Experiment
II 0.00
28.0
0
36.5
0
41.0
0
42.0
0
42.0
0
42.0
0
The volume of gas released is recorded in
Table 7.1
Isipadu gas yang terhasil direkodkan dalam
Jadual 7.1
•Plot a graph of volume of gas against time for both experiments in the graph paper provided on page 28.
Axis label & unit
All points transferred correctly
Curve – smooth curve, correct shape
Consistent scale
Label curve for both experiment
37. • Based on the graph, determine the rate of
reaction at 90 sec for Experiment I.
• Correct gradient drawn at t=90s
• Calculation, answer and unit (0.11 ± 0.03)
cm3
s-1
38. • Another set of experiment was carried out to
study the effect of temperature on the rate of
reaction between sodium thiosulphate
solution and sulphuric acid as shown in Table
7.2
Experiment
Eksperimen
I II
Temperature of sodium
thiosulphate / o
C
Suhu natrium tiosulfat
40 50
Write the ionic equation for the reaction.
S2
O3
2-
+ 2H+
S + SO2
+ H2
O
Correct formulae
Balance
39. • Compare the rate of reaction between
Experiment I and II by using Collision Theory.
• The rate of reaction in Experiment II is higher
than Experiment I
• 2. Temperature of sodium thiosulphate
solution in Experiment II is higher
• 3. Kinetic energy of particles in Experiment II
is higher,
• 4. frequency of collision between
thiosulphate ions and hydrogen ions higher
in Experiment II,
• [a: ions if the name of the ions is given in
40. • Based on the statement, explain the meaning of
ecorrect elements [ie: carbon and hydrogen]
• 2. The simplest ratio of mole/atom of carbon to
hydrogen is 2:5
• 3. The molecular formula shows the actual
number of carbon and hydrogen atoms in a
molecule
• 4. 1 molecule of butane contains 4 carbon
atoms and 10 hydrogen atoms.
• mpirical formula and molecular formula
The molecular formula of butane is C4H10
and its empirical formula is C2H5.
Formula molekul bagi butana ialah C4H10
dan formula empiriknya ialah C2H5
41. The decomposition of copper(II) nitrate is
shown in the following equation:
2 Cu(NO3)2 2 CuO + 4 NO2 + O2
(Relative atomic mass: N=14, O=16,
Cu=64,
molar volume of gas at room condition; 24
dm3
mol-1
)
Determine the percentage composition by
mass of oxygen in copper(II) nitrate.
% of oxygen
= 6(16) X 100 = 51.06 %
64 + 14(2) + 16(6)
Correct RMM shown
Calculation
and answer
42. • If 3.2 g of copper(II) oxide is produced during
the heating process, calculate the volume of
oxygen gas evolved at room condition.
• Number of mole of CuO = 3.2 = 0.04
mol
• 64 + 16
• 2 mol of CuO is released with 1 mol of O2
• 0.04 mol of CuO is released with 0.02 mol of
O2
• Volume of O2evolved = 0.02 (24) dm3
mol-1
• = 0.48 dm3
43. • A student carried out two experiments to
determine the empirical formulae for
magnesium oxide and copper(II) oxide.
• Diagram 8 shows the apparatus set-up for
both experiments.
Experiment I
Eksperimen I
Heat
Panaskan
Magnesium coil
Pita magnesium
Experiment II
Eksperimen II
Copper(II) oxide
Kuprum(II) oksida
Heat
Panaskan
Dry hydrogen
Hidrogen kering
44. Explain the differences in the method used
for the determination of the empirical
formulae for both oxides.
• Magnesium is a reactive metal
• 2. Magnesium can combine / react [readily]
with oxygen to form magnesium oxide
• 3. Copper is less reactive than hydrogen //
copper situated lower than hydrogen in
Reactivity Series
• 4. Hydrogen can reduce copper(II) oxide to
copper.
45. • The following equations show two redox
reactions involving iron(II) ion, Fe2+
.
• I 2 Fe2+
+ Br2 → 2 Fe3+
+ 2 Br-
• II Fe2+
+ Zn → Fe + Zn2+
• Compare the role of Fe2+
ion in both reactions.
• Explain your answer.
Reaction I Reaction II
role Reducing agent1
Oxidizing agent1
The oxidation number
of iron increases from
+2 to +3// Fe2+
loss
electron to form Fe3+
1
oxidation number of
iron decreases from +2
to 0 // Fe2+
gain
electron to form Fe
atom1
Fe2+
undergoes
oxidation1
Fe2+
undergoes
reduction1
46. • The reaction between sodium and chlorine
forms a compound with a high melting point.
• Determine the mass of the compound formed
when 2.3 g sodium reacts with excess
chlorine.
• [Relative atomic mass Na= 23, Cl= 35.5]
• 2Na + Cl2 2NaCl
• Number of mole of Na = 2.3 = 0.1
mol 23
•
• 2 mol of Na produce 2 mol of NaCl
47. Reaction
Tindak balas
Reactants
Bahan Tindak balas
Observation
Pemerhatian
I
Iron + Chlorine gas
Ferum + Gas klorin
The hot iron wool ignites rapidly
with a bright flame.
A brown solid is formed.
Wul besi panas menyala dengan cepat
dan terang.
Pepejal perang terhasil.
II
Iron + Bromine gas
Ferum + Gas bromin
The hot iron wool glows moderately
bright and moderately fast.
A brown solid is formed.
Wul besi panas berbara sederhana
terang dan sederhana cepat.
Pepejal perang terhasil.
Write the chemical equation for either of
the reactions.
) 2 Fe + 3Cl2 2FeCl3 or 2 Fe +
3Br2 2FeBr3
48. • Compare the reactivity of both reactions.
• Explain your answer.
• The reactivity of reaction I is higher than
reaction II.
• 2. The atomic size of chlorine is smaller
than bromine
• 3. The forces of attraction of the nucleus
toward the
• electrons is stronger in chlorine atom
than in bromine atom
• 4. It is easier for chlorine atom to attract
electron
49. • Diagram 9 shows the standard representation
for the atoms of three elements; Li, C and Cl.
Using the given information, describe the
formation of two compounds with different
types of bonding.
50. • . Electron arrangement of atom Li: 2.1, Cl:
2.8.7, C: 2.4
• Formation of compound between Li and Cl
• 2. To achieve stable electron arrangement
• 3. Lithium atom need to lose / donate 1
valence electron to form lithium ion // Li
Li+
+ e while
• 4. Chlorine atom need to gain 1 electron to
form chloride ion // Cl2 + 2e 2Cl-
• 5. Li+
ion attracted to Cl-
ion by electrostatic
force to form ionic bond
51. • 6. Diagram - correct number of electrons
and shells - shows Li+
ion and Cl-
ion
• Formation of compound between C and Cl
• 7. Carbon atom share valence electron with
chlorine atom
• 8. Each C atom contributes 4 electrons and
each Cl atom contributes 1 electron // each
C atom share electron with 4 Cl atom
• 9. To form #
4 single#
covalent bond
• 10. diagram - correct number of
electrons and shells
• - shows sharing electron
52. Mg + 2 HCl
ΔH = -50.4 kJ mol -1
Mg Cl2 + H2
Determine the temperature change when
50 cm3
of 1.0 mol dm-3
of
hydrochloric acid reacts with excess
magnesium.
[Specific heat capacity of
solution: 4.2 J g-1 o
C-1
,
density of solution: 1 g cm-3
]
53. • Mol of hydrochloric acid = 1 x 50
• 1000
• = 0.05 mol
• 2 mol HCl react to produce 50.4 kJ
• 0. 05 mol of HCl react to produce = 0. 05 x
50.4
• 2 = 1.26 kJ
• θ = H
• mc
• = 1.26 x 1000
• (50)(4.2)
54. Alcohol
Alkohol
Molecular Formula
Formula molekul
Heat of combustion/ kJ mol-1
Haba pembakaran
Propanol C3H7OH -2100
Butanol C4H9OH -2877
•Write the equation for the complete combustion of either one of the alcohol.
C3
H7
OH + 9/2O2
3CO2
+ 4H2
O
or
C4
H9
OH + 6 O2
4CO2
+ 5H2
O
55. • Compare the heat of combustion between
propanol and butanol.
• Explain your answer.
• Heat of combustion of butanol is higher than
propanol.
• 2. The number of carbon atom per molecule
butanol is bigger than propanol
• 3. Butanol produce more carbon dioxide and
water molecules than propanol // more
bonds are formed // energy content is higher
in butanol.
• 4. Released more heat energy
56. • Describe a laboratory experiment to
determine the heat of combustion of a named
alcohol.
• Your answer should include:
• a labeled diagram
• procedure
57. • Diagram:
• Arrangement of apparatus is functional
• can with water, thermometer, spirit lamp with
alcohol
• no wire gauze, thermometer not touching
surface, flame touching can
• Labeled water, alcohol, [metal] can
•
58. • Procedure:
• 1. (100-250 cm3
) of water is measured and
poured into a copper can and the copper can is
placed on a tripod stand.
• 2. The initial temperature of the water is
measured and recorded.
• 3. A spirit lamp with ethanol is weighed and
its mass is recorded.
• 4. The lamp is then placed under the copper
can and the wick of the lamp is lighted up
immediately.
59. • 5. The water in the can is stirred continuously
until the temperature of the water
increases by about 20- 50 o
C.
• 6. The flame is put off and the highest
temperature reached by the water is
recorded.
• 7. The lamp and its content are weighed and
the mass is recorded.