Determine the strength in grams per litre of a given ag no3 solution being provided
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Mohr’s method is used to determine the chloride ion concentration by titrating with silver nitrate. Using pure sodium chloride the strength of silver ions can be also determined as the Ag(I) ions react with chloride ions, quantitatively, to form a precipitate of silver chloride.
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1) The document describes the Mohr's method for determining the concentration of silver nitrate (AgNO3) solution by titrating it against a standard sodium chloride (NaCl) solution.
2) In the titration, silver ions from AgNO3 react quantitatively with chloride ions from NaCl to form a precipitate of silver chloride. The endpoint is reached when excess Ag+ ions react with chromate ions from a potassium chromate indicator to form a red-brown precipitate of silver chromate.
3) The procedure involves titrating a known concentration of NaCl solution against the AgNO3 solution to determine its molarity, using potassium chromate as the indicator.
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Here are the steps to solve this problem:
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2) Given: Mass CuO = 5.6 g
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Moles CuO = Mass / Molar mass = 5.6 g / 80 g/mol = 0.07 mol
3) From the equation: 1 mol CuO requires 1 mol H2SO4
Moles H2SO4 needed = Moles CuO = 0.07 mol
4) Given: Concentration of H2SO4 = 1.25 mol/dm3
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Chapter 8 salt part 4
Here are the steps to solve this problem:
1) Write the balanced chemical equation:
CuO + H2SO4 → CuSO4 + H2O
2) Given: Mass CuO = 5.6 g
Molar mass CuO = 64 + 16 = 80 g/mol
Moles CuO = Mass / Molar mass = 5.6 g / 80 g/mol = 0.07 mol
3) From the equation: 1 mol CuO requires 1 mol H2SO4
Moles H2SO4 needed = Moles CuO = 0.07 mol
4) Given: Concentration of H2SO4 = 1.25 mol/dm3
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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.
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The document describes the continuous variation method used to construct ionic equations for insoluble salts. It involves carrying out experiments where the volume of one reactant is kept fixed while the volume of the other reactant is varied. The mole ratio of the reactants that results in all of the first reactant reacting indicates the ratio in the ionic equation. An example using lead (II) chromate (PbCrO4) precipitation is provided to illustrate the method.
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SI #7 Key
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3. It provides an example of the fermentation of glucose producing ethanol and carbon dioxide, and calculates related quantities.
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2. Calculating pH, concentrations of ions, and degree of dissociation for solutions of weak acids and bases.
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#19 key
1. 18.9 grams of K2Cr2O7 are present in 50.0 mL of 0.360 M K2Cr2O7 solution.
2. The molarity of the (NH4)2SO4 solution formed from dissolving 4.28 grams of (NH4)2SO4 in 300 mL of water is 0.108 M.
3. 58.7 mL of 0.240M CuSO4 solution contains 2.25 grams of CuSO4 solute.
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Precipitation Titrations
1. Precipitation titrations involve the titration of an analyte solution with a reagent that causes the formation of an insoluble precipitate.
2. The Mohr method is commonly used for chloride determination and involves titrating a chloride solution with silver nitrate using potassium chromate as an indicator.
3. At the endpoint, excess silver nitrate reacts with potassium chromate to form a reddish brown silver chromate precipitate, indicating that all the chloride ions have been precipitated out as silver chloride.
Mohr method
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.
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Prepared By GULAM MUHEYUDDEEN
ASSISTANT PROFESSOR
Department Of Pharmaceutical Chemistry
Jahangeerabad Institute Of Technology (Faculty Of Pharmacy) BARABANKI
Quantitative analysis and volumetric analysis
This document provides information on quantitative analysis and volumetric analysis techniques. It defines key terms like concentration, molarity, and standard solutions. It describes common volumetric apparatus and how to perform acid-base titrations using appropriate indicators. It also covers concepts like molar ratios, dilution calculations, and determining water of crystallization through titration reactions. The document provides examples of calculations for molarity, concentration, purity, and molar mass determinations.
Percentage of available chlorine in bleaching powder.
This document provides instructions for determining the percentage of available chlorine in bleaching powder using titration. Sodium thiosulfate is standardized against a dichromate solution and then used to titrate iodine liberated from the reaction of bleaching powder with potassium iodide in acidic medium. The amount of thiosulfate consumed corresponds to the available chlorine content of the bleaching powder. Questions are also provided about chlorine use in water supplies and the harms of chlorine versus chloride ions.
ebt method.docx
This document provides instructions for titrating HCl against a standard NaOH solution potentiometrically. A known volume of HCl is placed in a beaker and connected to a saturated calomel electrode and hydrogen electrode. Small additions of NaOH are made from a burette and the potential is measured after each addition. The potential readings are plotted against volume added to obtain the titration curve. The equivalence point is identified as the point of maximum slope on the curve or differential curve, indicating where the H+ concentration has changed the most with small volume additions of NaOH base. The experiment allows for the potentiometric titration of a strong acid against a strong base.
Precipitation titrations
This document discusses analytical chemistry techniques for precipitation titrations, specifically the determination of chloride ions. It describes two methods - Mohr's method and Volhard's method. Mohr's method titrates a chloride solution against silver nitrate using potassium chromate as an indicator. When all chloride ions are removed, the solution color changes from yellow to reddish brown. Volhard's method also uses silver nitrate but titrates any excess silver ions with ammonium thiocyanate, forming a reddish brown precipitate. The document provides step-by-step procedures for both methods to calculate the concentration of chloride ions in a water sample.
Volumetric analysis
This document provides information and examples on solutions and titrations in chemistry:
- It defines key terms like solute, solvent, concentration, molarity and explains how to calculate concentrations in g/dm3 and moldm-3.
- Examples are given for calculating the mass of a solute needed to make a solution of a given volume and molarity, and for calculating concentrations when solutions are diluted.
- A titration is described as a procedure using a burette to add one solution of known concentration to a flask of another until reaction is complete.
- Standard solutions that are suitable for titrations are outlined.
- Worked examples of titration calculations include determining
Report 1 prepare and standardize a 0.1 M NaOH solutions
This document describes an experiment to prepare and standardize a 0.1 M sodium hydroxide (NaOH) solution through titration. The student measured and diluted a 3 M NaOH solution to make an approximate 0.1 M NaOH solution. This solution was then standardized through titration against a 0.104 M sulfamic acid standard solution. The student determined the concentration of the NaOH solution to be 0.092 M on average, with a percent error of -9% due to imprecise measurement of the initial 3 M NaOH solution. The student concluded the procedure was successful in standardizing the NaOH solution and learning the titration technique.
Estimation of Copper contained in a supplied solution by iodometric method.pptx
This document summarizes a chemistry lab experiment on estimating the amount of copper in a solution using iodometric titration. The objectives are to determine the amount of copper in a copper salt solution and study oxidation-reduction titration. Standard sodium thiosulfate solution is used to titrate iodine liberated from the reaction of copper solution, potassium iodide, and acetic acid. Calculations are shown to find the molarity of copper in the original solution based on the titration results. The amount of copper determined in 1 liter of the supplied copper sulfate solution was 0.978 grams.
Negeri sembilan 2013
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.
Determination of acidity of water
This document describes an experiment to determine the acidity of a water sample. The experiment involves titrating the water sample with a standard sodium hydroxide (NaOH) solution using two different acid-base indicators - methyl orange and phenolphthalein. The titration with methyl orange determines the mineral acidity as mg/L of calcium carbonate (CaCO3), while titration with phenolphthalein determines the total acidity, including carbonic acid, as mg/L of CaCO3. The procedure, observations, and calculations for determining the mineral and total acidity are provided.
Precepitation titration mohrs method
This document discusses precipitation titrations, specifically Mohr's method for determining chloride concentration. Mohr's method involves titrating a chloride sample with silver nitrate solution until a red silver chromate precipitate forms, indicating the endpoint. The reaction between silver ions and chloride ions forms an insoluble silver chloride precipitate. Potassium chromate is used as the indicator which changes color upon reaction with excess silver ions after all chloride is precipitated. Mohr's method provides an accurate means of determining chloride concentration in neutral or unbuffered solutions like drinking water or saline solutions.
Sample paper 3 Class xi chem
This document contains a 30 question chemistry sample exam with multiple choice and long answer questions. It provides instructions for the exam, including question types and point values. The questions cover topics such as chemical formulas, hybrid orbitals, equilibrium reactions, acid-base chemistry, and organic chemistry reactions. Sample solutions are provided for some questions as examples. The exam is designed to test understanding of essential chemistry concepts and principles.
Exp 4
This document describes a procedure to determine the acidity of a water sample through titration with sodium hydroxide solution. The acidity is measured as both mineral acidity at pH 3.7 using methyl orange indicator and total acidity at pH 8.3 using phenolphthalein indicator. Dissolved carbon dioxide is usually the major contributor to acidity in surface waters. The titration results are used to calculate and report the acidity levels in the sample as mg/L of calcium carbonate equivalent. High acidity can interfere with water treatment and affect aquatic life.
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Percentage of available chlorine in bleaching powder.
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Given
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Model systems are smaller, simpler versions of complex biomolecules that can be used to study biological chemical processes. While not a perfect representation, model systems allow for controlled experiments that provide valuable information about real biological systems. Transition metal complexes with organic ligands are often used as model systems to mimic biological chemical reactions involving metal ions. Examples of model systems that have increased understanding of real systems include iron-porphyrin compounds for hemoglobin and copper complexes for copper-containing enzymes.
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The document provides guidelines for writing a third year project report. It discusses the different types of research projects including fundamental, descriptive, empirical, quantitative, applied, analytical and qualitative. It outlines the typical sections of a project report such as the title page, declaration, certificate, acknowledgment, index, abstract, introduction, experimental, results and discussion, conclusion and references. For each section, it provides details on the content and formatting. It emphasizes writing in a clear, concise and organized manner with proper citations and references. The document aims to help students structure their project reports and effectively communicate their research.
Chemical properties of Interhalogen compounds.pdf
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Determination of conductivity of soil sample.pdf
This document provides instructions for determining the conductivity of a soil sample. It explains that soil conductivity is a measure of its ability to carry an electrical current and can indicate nutrient levels and contamination. The procedure calibrates a conductivity cell using potassium chloride solutions, measures the conductance of distilled water, mixes a soil sample with water, filters it, and measures the conductance to determine the soil sample's conductivity.
Determination of Bulk density of soil sample..pdf
This document provides instructions for determining the bulk density of a soil sample using the cylinder method. It defines bulk density as the dry weight of soil divided by its volume, which includes both soil particles and pore space. The procedure involves heating a soil sample to remove moisture, placing it in a measuring cylinder, and recording the weight and occupied volume without compaction. Bulk density can be expressed in units of g/mL or g/cm3 and provides information about soil properties like porosity, root growth, and nutrient availability.
Determination of acidity of a water sample..pdf
The acidity of water is a measure of the quantitative capacity to react with a mineral base. The measured value usually varies with the pH indicator used in the experiment. The solution of phenolphthalein is colourless in acidic or mild basic medium (pH<8.0), while in basic medium (pH<9.6) solution is pink. The solution of methyl orange is generally red at pH lower than 3.1 and above pH 4.4 the solutions are yellow.
The dissolved strong mineral acids, weak organic acids, dissolved carbon dioxide and hydrolyzed mineral salts may contribute to the measured acidity of natural water. The acidity of water is a significant parameter of water as the presence of acids in natural water contributes to corrosiveness and influences chemical reaction rates. The biological processes are dependent on the acidity of water. The quantitative acidity measurement also reflects the quality of the source of water. The acidity of water is usually expressed in terms of CaCO3.
Techniques of soil sampling.pdf
Soil sampling is important to determine the quality and composition of soil. A representative soil sample should include incremental samples taken from the surface and at depths of 0.5 and 1.0 meters. Individual samples should be labeled and stored properly. As soil can appear homogeneous but actually vary in composition, careful sampling procedures are necessary to obtain samples truly representative of the soil being analyzed. Where soil is heterogeneous over a large area, sampling must be done with great care.
Inorganic Section solved FYBSC 2022.pdf
The document is an answer key for an inorganic chemistry and organic chemistry exam containing multiple choice and descriptive questions.
Some of the questions addressed in the summary include drawing orbital diagrams, electronic configurations of atoms, types of chemical bonds, and properties of ionic compounds.
The descriptive questions require explanations about anomalous electronic configurations, molecular geometry, decomposition of carbonates, quantum numbers, and dual nature of matter.
IDP MFDdraft.pptx
The document provides guidelines for developing an Institutional Development Plan (IDP). It outlines 7 key sections:
1) General instructions for developing the IDP including defining objectives, goals, and activity plans.
2) The IDP will be prepared for 5 years and include sustainability measures. It will be a living document that evolves over time.
3) Key steps in the IDP development process including stakeholder consultations and drafting/finalizing the plan.
4) IDP implementation grants will be awarded competitively and approved plans will be published online.
5) Institutions will report progress against targets to the Department of Higher Education periodically.
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Molecular orbital diagram of CO and NO
This document contains molecular orbital diagrams for carbon monoxide (CO) and nitric oxide (NO). The CO diagram shows the atomic orbitals of carbon and oxygen and the resulting molecular orbitals of 4σ, 2σ, 1σ, 3σ, and 2Π, 1Π. The NO diagram also shows the atomic orbitals of nitrogen and oxygen and their molecular orbitals of 2σ, 1σ, 3σ, 4σ, 2Π, and 1Π. Both diagrams provide the electron configurations of carbon, oxygen, nitrogen and illustrate the molecular orbital energy levels formed when they combine.
Polarisation and polarisability
Polarisation occurs when the electron cloud of an atom or ion is distorted by the influence of a nearby positive atomic nucleus or electric field. Polarisability is the ability of an atom or ion to become polarized. Polarization can range from a slight distortion to a sufficient distortion that forms a covalent bond between ions. According to Fajans' Rules, ions with higher charges and smaller sizes polarize anions more, while ions with higher charges and larger sizes polarize cations more. Ions with partially filled d orbitals also polarize more than ions with noble gas configurations.
Molecular orbitals diagrams of [Co(NH3)6]3+
The document presents an M.O. diagram for the [Co(NH3)6]3+ complex. It shows the metal (Co3+) orbitals interacting with the ligand (NH3) orbitals to form molecular orbitals. The Co3+ has a 3d6, 4s0 electronic configuration. The six ammonia ligands each contribute 2 sigma electrons, for a total of 12 ligand electrons. These interact with the metal orbitals to form the molecular orbital diagram shown, with no pi interactions included.
Evidences for covalent bonding in complexes
This document discusses evidence for covalent bonding in metal complexes from three perspectives:
1. The nephelauxetic effect shows that electron-electron repulsion is less in complexes than free metal ions due to delocalization of electrons over ligand orbitals.
2. Nephelauxetic parameters (β) quantify this effect, with softer ligands having smaller β values.
3. Electron paramagnetic resonance (EPR) spectroscopy reveals hyperfine splitting in complex spectra, showing interaction between ligand nuclear spins and metal electron spins, further indicating covalent bonding.
Molecular orbitals diagrams of [Ti(H2O)6]3+
The document presents an M.O. diagram for the [Ti(H2O)6]3+ complex. It shows the metal (Ti3+) orbitals and ligand (H2O) orbitals that form the molecular orbitals of the complex. The diagram displays the orbital interactions between the titanium 3d1, 4s0 orbitals and the 12 sigma electrons from the six water ligands to produce the molecular orbital configuration of the [Ti(H2O)6]3+ complex.
Molecular orbitals diagrams without pi interactions
This document presents a molecular orbital diagram for an ML6 complex, where M is a metal atom and L are six ligand atoms. The diagram shows the atomic orbitals of the metal interacting with the ligand orbitals to form molecular orbitals. The molecular orbitals are grouped as bonding, non-bonding, and antibonding. The diagram lacks π interactions between the ligands and metal and seeks to illustrate the interactions between just the s and p atomic orbitals.
Bohrn lande equation
The Born-Lande equation describes the lattice energy (U) of an ionic crystal as a function of the charges on the cation (Z+) and anion (Z-), the equilibrium interionic distance (r0), and other physical constants. It includes contributions from the Madelung constant, Coulomb interactions, and short-range repulsion. The document provides an example application of the Born-Lande equation to calculate the lattice energies of various ionic crystals such as LiF, CsI, and MgO.
Estimation of ca and mg in given water sample
This document describes an experiment to estimate calcium and magnesium ions using complexometric titration with EDTA. The procedure involves standardizing a solution of EDTA against zinc sulfate using Eriochrom Black T indicator. Then, a sample containing calcium or magnesium ions is titrated against the standardized EDTA solution. The end point is indicated by a color change of the indicator from red to blue. The amount of calcium carbonate in a given water sample can then be calculated from the titration results.
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Determine the strength in grams per litre of a given ag no3 solution being provided
- 1. SHREE MALLIKARJUN COLLEGE CLASS:SYBSC SAFETY: Refer to MSDS of sodium chloride, potassiumchromate and silver nitrate. -Dr. Mithil S. Fal Desai Aim: Determine the strength in grams per litre of a given AgNO3 solution being provided N/30 NaCl solution by Mohr’s method. Chemicals: Sodium chloride, potassium chromate and silver nitrate. Apparatus: Standard volumetric flask, pipette, burette, conical flask, beakers, funnel and glass rod. Theory: Mohr’s method is used to determine the chloride ion concentration by titrating with silver nitrate. Using pure sodium chloride the strength of silver ions can be also determined as the Ag(I) ions react with chloride ions, quantitatively, to form a precipitate of silver chloride. Ag+ (aq) + Cl- (aq) AgCl(s) At the endpoint, all the chloride ions are precipitated and excess Ag(I) ions react with the chromate ions, to form a red-brown precipitate of silver chromate. 2Ag+ (aq) + CrO4 2- (aq) → Ag2CrO4(s) The pH of the sample solutions should be 6-10. If the solutions are acidic, the gravimetric method or Volhard’s method is more suitable. Procedure: A) Preparation of 0.033 N (N/30) NaCl. calculate B) Preparation of indicator: dissolve 2 g of K2CrO4 in 40 mL of distilled water. C) Estimation of the strength of the given AgNO3 solution. Rinse and fill the burette with given AgNO3 solution. Pipette out N/30 mL of NaCl solution in a conical flask. Add 20 mL of distilled water and 1 mL potassium chromate indicator. Titrate the solution in the flask against 0.033N NaCl until the red-brown colour of silver chromate is observed. Repeat the titration to get constant readings. Results: i) Strength of AgNO3 solution is =____N =____gL-1 Further reading (available in the library) 2) Vogel’s textbook of quantitative chemical analysis, J. Mendham, R. C. Denney, J. D. Barns, M. Thomas, B. Sivasankar, Pearson India Education, 6th Edition. Question 1) What is Volhard’s method? 2) Can we use KMnO4 as an indicator in this titration? 3) What is the advantage of Volhard’s method over Mohr’s method?