To estimate the concentration of KMnO4 and CuSO4 solutions, colorimetrically
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This document outlines a procedure to estimate the concentration of potassium permanganate (KMnO4) and copper sulfate (CuSO4) solutions using a colorimeter. Standard solutions of varying concentrations of each compound are prepared. The absorbance of each standard solution is measured using different colorimeter filters to select the filter with the highest absorbance. A calibration curve of absorbance versus concentration is plotted for each compound. The absorbance of unknown solutions is then measured and the concentrations are determined using the calibration curves. The procedure aims to estimate the unknown concentrations of KMnO4 and CuSO4 colorimetrically based on the Beer-Lambert law relationship between absorbance and concentration.
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How long could one survive in a perfectly airtight room?
Given
Inhaled air contains 21% oxygen while exhaled breath contains approximately 16% oxygen and 5% carbon dioxide
The minimum oxygen level required for survival is 19 %.
Dimensions of room in meters: 5 X 5 X 3
The role of Model systems.pdf
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.
Writing Third Year Project Report: Some Handy Guidelines
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Chemical properties of Interhalogen compounds.pdf
Interhalogen compounds exhibit various chemical properties and reactivities. AX-type interhalogens like ICl hydrolyze to form hydrogen halides and hypohalous acids. ClF3 and BrF3 can fluorinate metal oxides to form metal fluorides and oxygen. Higher interhalogens like ClF5 and IF7 can ionize to form polyatomic ions. IF7 reacts with water to form IOF5 and HF, and with silicon dioxide to form IOF5 and silicon tetrafluoride.
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.
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Determine the strength in grams per litre of a given AgNO3 solution being pro...
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.
अडण्णे शिगमो लोकसाहित्य
This is a small attempt to preserve heritage and folk culture of Goan village Adnem
Credits to Ghanashyam K. Devidas, Lakshimikant Bhavu, Vithobha Bhavu
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.
Estimation of water of crystallization in mohr’s salt by titrating with stand...
The document describes an experiment to determine the water of crystallization in Mohr's salt, (NH4)2Fe(SO4)2.XH2O, by titrating a solution of the salt with standardized potassium manganate(VII). The experiment involves standardizing the KMnO4 solution using sodium oxalate, then titrating samples of Mohr's salt solution and calculating the iron content. Based on comparing the experimental iron percentage to theoretical percentages for different values of X, the water of crystallization is determined to be 6 moles, giving the formula (NH4)2Fe(SO4)2.6H2O.
Estimation of oxalic acid experimental data
The document describes the titration of oxalic acid with potassium permanganate. It provides the theory of the redox reaction, where manganese is reduced and carbon is oxidized. It then gives the experimental procedure for standardizing the KMnO4 solution using sodium oxalate and then using the standardized solution to determine the concentration of an unknown sample of oxalic acid. The calculations section shows how to determine the equivalent weight of oxalic acid and use the titration data to find the exact normality of KMnO4 and the normality and mass of oxalic acid in the unknown sample.
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.
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To estimate the concentration of KMnO4 and CuSO4 solutions, colorimetrically
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