The document analyzes the water quality of Mankato State University's tap water by measuring alkalinity, acidity, and hardness. Experiments found the water had high alkalinity (29.33 ppm of CaCO3), lower acidity (8 ppm of CaCO3), and was classified as hard (210 ppm of CaCO3). This indicates the water is well-buffered against acidification and has higher dissolved metal content. In conclusion, measuring these factors provides insight into the water's chemical properties and quality.
This document provides instructions for determining the alkalinity of a water sample using a double-endpoint titration. Alkalinity is caused by carbonate, bicarbonate, and hydroxide ions and refers to a water sample's ability to neutralize acids. A titration with sulfuric acid is conducted, with two endpoints detected using different pH indicators. The volumes of acid needed at each endpoint can identify which ions are present and be used to calculate the sample's total, phenolphthalein, carbonate, bicarbonate, and hydroxide alkalinities in mg/L CaCO3. Tables are provided to match titration results to ion combinations and determine which acid volumes to use
Lab 4 alkalinity –acidity and determination of alkalinity in waterAnas Maghayreh
Environmental lab
Lab 4 alkalinity –acidity and determination of alkalinity in water
experiment at JORDAN UNIVERSITY OF SCIENCE AND TECHNOLOGY
by: ANAS MAGHAYREH
Determination of hardness and alkalinity of waste waterAakash Deep
This power point presentation illustrates the principles and methods of estimation of hardness and alkalinity of waste water.
I have included the principle, titration method, formulas and some sample problems based on them.
The document describes a jar test experiment to determine the optimal coagulant dosage for treating turbid water. Jar tests simulate the coagulation/flocculation process in water treatment plants. In this experiment, different dosages of aluminum sulfate were added to water samples, which were then rapidly and slowly mixed to form and combine floc. Turbidity measurements after settling showed an optimal dosage between 6-8 ml of aluminum sulfate coagulant reduced turbidity the most. The jar test process and results help operators adjust treatment chemicals to changing source water quality.
This experiment determined various solids concentrations in water samples to assess water quality. Three water samples - tap water, surface water, and mixed water - were tested. Parameters like total solids (TS), total volatile solids (TVS), total fixed solids (TFS), total suspended solids (TSS), fixed suspended solids (FSS), total dissolved solids (TDS), and total volatile dissolved solids (TVDS) were measured using techniques like weighing, filtration, evaporation at 105°C, and combustion at 550°C. The results showed that surface water had the highest solids concentrations, while tap water had the lowest as it was
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.
This document describes an experiment to determine the alkalinity of a water sample through titration with sulfuric acid. Alkalinity is measured by titrating a water sample with acid until the pH reaches 4.5, neutralizing hydroxyl, carbonate, and bicarbonate ions. The titration is performed twice - first with phenolphthalein to measure phenolphthalein alkalinity from hydroxyl ions, then with a mixed indicator to measure total alkalinity from additional carbonate and bicarbonate ions. The alkalinity of the tested sample was found to be 83 mg/L, within acceptable limits for drinking water.
1. The document describes an experiment to determine the hardness of water samples through titration with EDTA using indicators. Total hardness, calcium hardness, and magnesium hardness were calculated based on the titration volumes.
2. Hardness is caused by calcium and magnesium ions in water and is a measure of its ability to form precipitates with soap. It can be temporary, from bicarbonates, or permanent, from chlorides and sulfates.
3. The results found a total hardness of 400 mg/L as CaCO3, calcium hardness of 140 mg/L as CaCO3, and magnesium hardness of 260 mg/L as CaCO3 for the water sample tested.
This document provides instructions for determining the alkalinity of a water sample using a double-endpoint titration. Alkalinity is caused by carbonate, bicarbonate, and hydroxide ions and refers to a water sample's ability to neutralize acids. A titration with sulfuric acid is conducted, with two endpoints detected using different pH indicators. The volumes of acid needed at each endpoint can identify which ions are present and be used to calculate the sample's total, phenolphthalein, carbonate, bicarbonate, and hydroxide alkalinities in mg/L CaCO3. Tables are provided to match titration results to ion combinations and determine which acid volumes to use
Lab 4 alkalinity –acidity and determination of alkalinity in waterAnas Maghayreh
Environmental lab
Lab 4 alkalinity –acidity and determination of alkalinity in water
experiment at JORDAN UNIVERSITY OF SCIENCE AND TECHNOLOGY
by: ANAS MAGHAYREH
Determination of hardness and alkalinity of waste waterAakash Deep
This power point presentation illustrates the principles and methods of estimation of hardness and alkalinity of waste water.
I have included the principle, titration method, formulas and some sample problems based on them.
The document describes a jar test experiment to determine the optimal coagulant dosage for treating turbid water. Jar tests simulate the coagulation/flocculation process in water treatment plants. In this experiment, different dosages of aluminum sulfate were added to water samples, which were then rapidly and slowly mixed to form and combine floc. Turbidity measurements after settling showed an optimal dosage between 6-8 ml of aluminum sulfate coagulant reduced turbidity the most. The jar test process and results help operators adjust treatment chemicals to changing source water quality.
This experiment determined various solids concentrations in water samples to assess water quality. Three water samples - tap water, surface water, and mixed water - were tested. Parameters like total solids (TS), total volatile solids (TVS), total fixed solids (TFS), total suspended solids (TSS), fixed suspended solids (FSS), total dissolved solids (TDS), and total volatile dissolved solids (TVDS) were measured using techniques like weighing, filtration, evaporation at 105°C, and combustion at 550°C. The results showed that surface water had the highest solids concentrations, while tap water had the lowest as it was
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.
This document describes an experiment to determine the alkalinity of a water sample through titration with sulfuric acid. Alkalinity is measured by titrating a water sample with acid until the pH reaches 4.5, neutralizing hydroxyl, carbonate, and bicarbonate ions. The titration is performed twice - first with phenolphthalein to measure phenolphthalein alkalinity from hydroxyl ions, then with a mixed indicator to measure total alkalinity from additional carbonate and bicarbonate ions. The alkalinity of the tested sample was found to be 83 mg/L, within acceptable limits for drinking water.
1. The document describes an experiment to determine the hardness of water samples through titration with EDTA using indicators. Total hardness, calcium hardness, and magnesium hardness were calculated based on the titration volumes.
2. Hardness is caused by calcium and magnesium ions in water and is a measure of its ability to form precipitates with soap. It can be temporary, from bicarbonates, or permanent, from chlorides and sulfates.
3. The results found a total hardness of 400 mg/L as CaCO3, calcium hardness of 140 mg/L as CaCO3, and magnesium hardness of 260 mg/L as CaCO3 for the water sample tested.
Alkalinity in water is measured by titrating a water sample with sulfuric acid and monitoring the pH. Alkalinity is caused by hydroxides, carbonates, and bicarbonates and is expressed in units of mg/L of calcium carbonate. The amount of acid needed to reduce the pH to 8.3 measures phenolphthalein alkalinity, while the amount to reduce to 4.5 measures total alkalinity. Different combinations of hydroxides, carbonates, and bicarbonates can be present depending on the initial pH. Alkalinity data provides information useful for water treatment processes like coagulation, softening, and corrosion control.
This document summarizes a student's lab experiment measuring turbidity in water samples. Turbidity is an indicator of water quality, measuring the cloudiness caused by suspended particles. The student tested tap water and bottled water from a lava company, finding turbidity levels of 2.4 NTU and 0.11 NTU respectively. Both results are within World Health Organization and EPA drinking water guidelines. Potential sources of error in turbidity measurement are discussed. The conclusion is that the water samples are suitable for drinking based on their turbidity levels.
This document describes procedures for determining biochemical oxygen demand (BOD) in a water sample. It defines BOD as a measure of the amount of oxygen used by aerobic bacteria to break down organic matter in water. The document outlines the objective, introduces BOD and the 5-day BOD test, discusses total and carbonaceous BOD, and lists safety procedures for handling wastewater samples.
This document provides information about determining the total hardness of a water sample using EDTA titration. It defines hardness as the concentration of calcium and magnesium ions in water. The document outlines the theory behind using EDTA to chelate calcium and magnesium ions, describes the chemicals and apparatus needed, and provides step-by-step instructions for performing an EDTA titration to quantify total water hardness.
Analysis BOD is an important parameter in identifying the extend of pollution in a water body. This presentation explains the various methods of BOD analysis as per the APHA manual
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.
This document describes an experiment to determine total dissolved and suspended solids in a water sample. The procedure involves filtering a water sample and evaporating the filtrate to determine total dissolved solids based on residue weight. Total suspended solids are determined by filtering a sample through a weighed filter and calculating residue weight. The results are used to classify water quality and evaluate treatment effectiveness.
Total soluble solids and Total suspended solidsAnuj Jha
This document defines total soluble solids and total suspended solids and discusses their significance. Total soluble solids refers to materials that are completely dissolved in water and filterable, as well as the residue left after evaporating a filtered sample. They are useful for determining water quality for drinking, agriculture, and industry. High soluble solid levels can negatively impact taste, odor, dissolved oxygen levels, and corrosion. Total suspended solids refers to materials that are not dissolved in water and non-filterable, as well as the residue of a non-filtered evaporated sample. Suspended solids are aesthetically displeasing and can harbor chemical and biological agents while depleting dissolved oxygen levels.
The document discusses iron and manganese in drinking water. It states that iron and manganese occur naturally in groundwater and can cause aesthetic issues like staining but do not pose health risks at typical concentrations. It discusses common treatment methods for iron and manganese like oxidation and filtration. Testing is needed to determine appropriate treatment methods based on the concentrations and forms of iron and manganese present.
This document provides a procedure for determining the alkalinity of water samples. Alkalinity is measured through acid-base titration and is important as it indicates a water sample's ability to resist changes in pH. The procedure involves titrating the sample with sulfuric acid using phenolphthalein and methyl orange indicators. The titrations are used to determine the phenolphthalein alkalinity and total alkalinity in mg/L of calcium carbonate. For the given water sample, the phenolphthalein alkalinity was found to be 0 while the total alkalinity was determined to be 65 mg/L, within the recommended limit of less than 200 mg/L.
Biological Oxygen Demand Lab Analysis and BackgroundJonathan Damora
The purpose of this experiment is to perform a Biochemical Oxygen Demand test on primary clarifier effluent from a wastewater treatment plant to determine a BOD versus time curve. This curve can then be used to determine the Ultimate BOD of the wastewater sample and the rate constant for its decay.
Total solids in water include total suspended solids, total dissolved solids, and volatile suspended solids. Dissolved solids consist of particles like calcium and chloride that pass through a small pore filter, while suspended solids include particles like silt, clay, and organic debris. Sources of solids in water include sewage, industrial discharge, road runoff, and soil erosion. Measuring total solids is important for controlling wastewater treatment and assessing regulatory compliance. The concentration of total solids is calculated by weighing solids in a water sample before and after drying.
This document describes a test to determine the total dissolved solids (TDS) in a water sample. The student measured an electrical conductivity of 440 μS/cm and calculated a TDS level of 264 mg/L. This result is within the WHO excellent range of less than 300 mg/L for drinking water. High TDS can cause water to taste bitter or salty and can harm aquatic animals. Reverse osmosis can be used to remove dissolved solids from water with elevated TDS levels.
This document provides information about the chemical oxygen demand (COD) test for measuring organic matter in wastewater. It discusses that COD measures the oxygen required to chemically oxidize organic material using potassium dichromate and sulfuric acid. COD and BOD both measure how much oxygen water will consume, but COD can oxidize more material so values are higher than BOD. The document outlines the COD test procedure and calculations for determining COD levels in wastewater samples. It also discusses standards, sources of BOD and COD, and limitations of the COD test.
This document discusses coagulation, which is the process of using chemical agents to remove suspended solids from water. It classifies coagulants as primary coagulants or coagulant aids. Primary coagulants neutralize particle charges to cause clumping, while coagulant aids add density and toughness to flocs. Common primary coagulants include alum, ferrous sulfate, and ferric sulfate. Coagulant aids improve coagulation by producing denser, faster-settling flocs. The document then provides details on alum and ferrous sulfate as primary coagulants, lists common coagulant aids, and reviews the coagulation/flocculation process.
Laboratory manual of water supply and sewerage engineeringTaufique Hasan
This document provides the procedure for determining the total alkalinity of water through titration. It defines alkalinity as the capacity of water to neutralize acids and discusses the significance of alkalinity measurements in water and wastewater treatment. The procedure involves titrating a water sample with sulfuric acid to two end points using phenolphthalein and methyl orange indicators. The ml of acid used is then used to calculate the total, hydroxide, carbonate, and bicarbonate alkalinity concentrations in the sample.
Coagulation and flocculation are important water treatment processes used to remove small particles from water. Coagulation involves adding chemicals like aluminum sulfate or ferric chloride to destabilize colloidal particles and reduce charges. This allows particles to agglomerate into larger flocs during flocculation. Jar tests are used to determine the optimum pH and coagulant dose. Mechanical and hydraulic flocculators are then used to slowly mix water and form flocs, which are removed by sedimentation. Proper design of coagulant chambers, flocculators, and clarifiers is needed for effective treatment.
Environmental Engineering Practical Series - Alkalinity Test of WaterSuyash Awasthi
Alkalinity of water is essential parameter to be found before its consumption. Following is a self explanatory presentation of why it is important and how to find the same in any sample of water.
WATER ANALYSIS /Water quality testing p.k.kPUSHPA KHOLA
This document discusses water quality testing parameters and methods. It notes that water contains contaminants and periodic testing is needed to ensure safety. Key physical, chemical, and biological characteristics are examined, including odor, temperature, pH, total solids, dissolved solids, suspended solids, alkalinity, hardness, calcium, chloride, fluoride, phosphate, sulfate, nitrate, oil and grease, and dissolved oxygen. Methods like titration, spectrophotometry, and incubation are described. Indian drinking water standards provide guidelines for parameters like TDS, pH, and hardness. Equipment used in analysis includes spectrophotometers, pH/TDS meters, COD digesters, and TSS filter assemblies. Regular water testing
The document provides instructions for performing several water quality tests to determine various characteristics including total solids, turbidity, coagulant dosage, pH, alkalinity, hardness, chlorides, sulfates, iron, manganese, biochemical oxygen demand, and coliforms. The jar test procedure is described to determine the optimal coagulant dose (alum) for clarifying a water sample by measuring turbidity at different coagulant dosages and identifying the lowest turbidity dose.
Marking scheme-chemistry-perfect-score-module-form-4-set-4Mudzaffar Shah
The document provides a marking scheme for an exam on acids, bases, and salts. It includes:
1) 11 multiple choice questions on acid-base concepts like neutralization reactions, ions present, calculating molarity, and distinguishing between strong/weak acids.
2) 9 more multiple choice questions testing identification of solutions, gas tests, and acid/base properties.
3) 10 essay questions requiring explanations of acid/base definitions, calculations of standard solutions, titration procedures, comparisons of acid types, and writing hypotheses and procedures for experiments.
4) Rubrics for grading lab reports with criteria like correctly recording burette readings, setting up tables, stating observations/inferences, and comparing
Alkalinity in water is measured by titrating a water sample with sulfuric acid and monitoring the pH. Alkalinity is caused by hydroxides, carbonates, and bicarbonates and is expressed in units of mg/L of calcium carbonate. The amount of acid needed to reduce the pH to 8.3 measures phenolphthalein alkalinity, while the amount to reduce to 4.5 measures total alkalinity. Different combinations of hydroxides, carbonates, and bicarbonates can be present depending on the initial pH. Alkalinity data provides information useful for water treatment processes like coagulation, softening, and corrosion control.
This document summarizes a student's lab experiment measuring turbidity in water samples. Turbidity is an indicator of water quality, measuring the cloudiness caused by suspended particles. The student tested tap water and bottled water from a lava company, finding turbidity levels of 2.4 NTU and 0.11 NTU respectively. Both results are within World Health Organization and EPA drinking water guidelines. Potential sources of error in turbidity measurement are discussed. The conclusion is that the water samples are suitable for drinking based on their turbidity levels.
This document describes procedures for determining biochemical oxygen demand (BOD) in a water sample. It defines BOD as a measure of the amount of oxygen used by aerobic bacteria to break down organic matter in water. The document outlines the objective, introduces BOD and the 5-day BOD test, discusses total and carbonaceous BOD, and lists safety procedures for handling wastewater samples.
This document provides information about determining the total hardness of a water sample using EDTA titration. It defines hardness as the concentration of calcium and magnesium ions in water. The document outlines the theory behind using EDTA to chelate calcium and magnesium ions, describes the chemicals and apparatus needed, and provides step-by-step instructions for performing an EDTA titration to quantify total water hardness.
Analysis BOD is an important parameter in identifying the extend of pollution in a water body. This presentation explains the various methods of BOD analysis as per the APHA manual
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.
This document describes an experiment to determine total dissolved and suspended solids in a water sample. The procedure involves filtering a water sample and evaporating the filtrate to determine total dissolved solids based on residue weight. Total suspended solids are determined by filtering a sample through a weighed filter and calculating residue weight. The results are used to classify water quality and evaluate treatment effectiveness.
Total soluble solids and Total suspended solidsAnuj Jha
This document defines total soluble solids and total suspended solids and discusses their significance. Total soluble solids refers to materials that are completely dissolved in water and filterable, as well as the residue left after evaporating a filtered sample. They are useful for determining water quality for drinking, agriculture, and industry. High soluble solid levels can negatively impact taste, odor, dissolved oxygen levels, and corrosion. Total suspended solids refers to materials that are not dissolved in water and non-filterable, as well as the residue of a non-filtered evaporated sample. Suspended solids are aesthetically displeasing and can harbor chemical and biological agents while depleting dissolved oxygen levels.
The document discusses iron and manganese in drinking water. It states that iron and manganese occur naturally in groundwater and can cause aesthetic issues like staining but do not pose health risks at typical concentrations. It discusses common treatment methods for iron and manganese like oxidation and filtration. Testing is needed to determine appropriate treatment methods based on the concentrations and forms of iron and manganese present.
This document provides a procedure for determining the alkalinity of water samples. Alkalinity is measured through acid-base titration and is important as it indicates a water sample's ability to resist changes in pH. The procedure involves titrating the sample with sulfuric acid using phenolphthalein and methyl orange indicators. The titrations are used to determine the phenolphthalein alkalinity and total alkalinity in mg/L of calcium carbonate. For the given water sample, the phenolphthalein alkalinity was found to be 0 while the total alkalinity was determined to be 65 mg/L, within the recommended limit of less than 200 mg/L.
Biological Oxygen Demand Lab Analysis and BackgroundJonathan Damora
The purpose of this experiment is to perform a Biochemical Oxygen Demand test on primary clarifier effluent from a wastewater treatment plant to determine a BOD versus time curve. This curve can then be used to determine the Ultimate BOD of the wastewater sample and the rate constant for its decay.
Total solids in water include total suspended solids, total dissolved solids, and volatile suspended solids. Dissolved solids consist of particles like calcium and chloride that pass through a small pore filter, while suspended solids include particles like silt, clay, and organic debris. Sources of solids in water include sewage, industrial discharge, road runoff, and soil erosion. Measuring total solids is important for controlling wastewater treatment and assessing regulatory compliance. The concentration of total solids is calculated by weighing solids in a water sample before and after drying.
This document describes a test to determine the total dissolved solids (TDS) in a water sample. The student measured an electrical conductivity of 440 μS/cm and calculated a TDS level of 264 mg/L. This result is within the WHO excellent range of less than 300 mg/L for drinking water. High TDS can cause water to taste bitter or salty and can harm aquatic animals. Reverse osmosis can be used to remove dissolved solids from water with elevated TDS levels.
This document provides information about the chemical oxygen demand (COD) test for measuring organic matter in wastewater. It discusses that COD measures the oxygen required to chemically oxidize organic material using potassium dichromate and sulfuric acid. COD and BOD both measure how much oxygen water will consume, but COD can oxidize more material so values are higher than BOD. The document outlines the COD test procedure and calculations for determining COD levels in wastewater samples. It also discusses standards, sources of BOD and COD, and limitations of the COD test.
This document discusses coagulation, which is the process of using chemical agents to remove suspended solids from water. It classifies coagulants as primary coagulants or coagulant aids. Primary coagulants neutralize particle charges to cause clumping, while coagulant aids add density and toughness to flocs. Common primary coagulants include alum, ferrous sulfate, and ferric sulfate. Coagulant aids improve coagulation by producing denser, faster-settling flocs. The document then provides details on alum and ferrous sulfate as primary coagulants, lists common coagulant aids, and reviews the coagulation/flocculation process.
Laboratory manual of water supply and sewerage engineeringTaufique Hasan
This document provides the procedure for determining the total alkalinity of water through titration. It defines alkalinity as the capacity of water to neutralize acids and discusses the significance of alkalinity measurements in water and wastewater treatment. The procedure involves titrating a water sample with sulfuric acid to two end points using phenolphthalein and methyl orange indicators. The ml of acid used is then used to calculate the total, hydroxide, carbonate, and bicarbonate alkalinity concentrations in the sample.
Coagulation and flocculation are important water treatment processes used to remove small particles from water. Coagulation involves adding chemicals like aluminum sulfate or ferric chloride to destabilize colloidal particles and reduce charges. This allows particles to agglomerate into larger flocs during flocculation. Jar tests are used to determine the optimum pH and coagulant dose. Mechanical and hydraulic flocculators are then used to slowly mix water and form flocs, which are removed by sedimentation. Proper design of coagulant chambers, flocculators, and clarifiers is needed for effective treatment.
Environmental Engineering Practical Series - Alkalinity Test of WaterSuyash Awasthi
Alkalinity of water is essential parameter to be found before its consumption. Following is a self explanatory presentation of why it is important and how to find the same in any sample of water.
WATER ANALYSIS /Water quality testing p.k.kPUSHPA KHOLA
This document discusses water quality testing parameters and methods. It notes that water contains contaminants and periodic testing is needed to ensure safety. Key physical, chemical, and biological characteristics are examined, including odor, temperature, pH, total solids, dissolved solids, suspended solids, alkalinity, hardness, calcium, chloride, fluoride, phosphate, sulfate, nitrate, oil and grease, and dissolved oxygen. Methods like titration, spectrophotometry, and incubation are described. Indian drinking water standards provide guidelines for parameters like TDS, pH, and hardness. Equipment used in analysis includes spectrophotometers, pH/TDS meters, COD digesters, and TSS filter assemblies. Regular water testing
The document provides instructions for performing several water quality tests to determine various characteristics including total solids, turbidity, coagulant dosage, pH, alkalinity, hardness, chlorides, sulfates, iron, manganese, biochemical oxygen demand, and coliforms. The jar test procedure is described to determine the optimal coagulant dose (alum) for clarifying a water sample by measuring turbidity at different coagulant dosages and identifying the lowest turbidity dose.
Marking scheme-chemistry-perfect-score-module-form-4-set-4Mudzaffar Shah
The document provides a marking scheme for an exam on acids, bases, and salts. It includes:
1) 11 multiple choice questions on acid-base concepts like neutralization reactions, ions present, calculating molarity, and distinguishing between strong/weak acids.
2) 9 more multiple choice questions testing identification of solutions, gas tests, and acid/base properties.
3) 10 essay questions requiring explanations of acid/base definitions, calculations of standard solutions, titration procedures, comparisons of acid types, and writing hypotheses and procedures for experiments.
4) Rubrics for grading lab reports with criteria like correctly recording burette readings, setting up tables, stating observations/inferences, and comparing
This document summarizes information about Indira Gandhi International Airport in New Delhi. It provides details about the airport's construction, facilities, suppliers, socio-economic issues, and CSR initiatives. Key points include that the airport was built at a cost of INR128.5 billion and opened in 2010 with a capacity of 34 million passengers. A public-private consortium led by GMR Group now manages the airport.
Diploma_I_Applied science(chemistry)_U-II(A) Preparation of solution Rai University
This document provides definitions and concepts related to solutions and concentration units. It defines key terms like solute, solvent, saturated and unsaturated solutions. It also explains concepts like mole, molecular weight, equivalent weight and how to calculate them. Finally, it discusses different units of concentration including normality, molarity, molality, percentage, parts per million (ppm) and how to interconvert between them through examples.
Laboratory solution preparation by Farhang HamidFarhang Hamid
Preparation of 0.1 M Na2CO3 solution in 250 ml D.W
part per million (PPm )
Buffer solution
Preparation of 1% w/v Na2CO3 solution
Concentration units
g(sample)=M.wt(sample)*Molarity*Volume
M1×V1=M2×V2
mass percent solution=(gram(solute))/(100 grams(soluion))%
D=mass/volume≫≫mass=Denstiy ×Volume
The document outlines procedures for determining various types of solids in water samples, including total solids, fixed solids, volatile solids, total dissolved solids, suspended solids, and settleable solids. Total solids include all materials retained after evaporation and drying of a sample. Fixed solids are the residues remaining after ignition, while volatile solids are lost during ignition. The procedures involve filtering samples, evaporating filtrates to determine dissolved fractions, and weighing residues to calculate concentrations.
1) Water treatment involves ensuring a safe and clean drinking water supply. It requires identifying a water source and protecting it from contamination through appropriate treatment and distribution.
2) Conventional drinking water treatment typically includes aeration, coagulation/flocculation, sedimentation, filtration and disinfection. It aims to remove microbes, particles, dissolved solids and other pollutants.
3) The key processes involve adding coagulants to neutralize particle charges, forming flocs for removal via sedimentation and filtration. Chlorine is commonly used for disinfection but produces disinfection byproducts, so alternatives like chloramines and ozone are also used.
1. The document discusses acids and bases, including their definitions and properties.
2. An acid is defined as a proton donor, donating hydrogen ions (H+) in water. A base is a proton acceptor, accepting hydrogen ions.
3. Common strong acids include hydrochloric acid (HCl), nitric acid (HNO3), and sulfuric acid (H2SO4) which fully ionize in water.
This document discusses acids and bases, including their properties and how to test for them. It provides information on:
- The pH scale ranges from 0-14, with acids having lower values and bases having higher values. A pH of 7 is neutral.
- Acids donate H+ ions in solution and have a pH below 7. Bases donate OH- ions and have a pH above 7.
- Indicators like litmus paper and cabbage juice can be used to test if a substance is acidic or basic - acids turn indicators one color while bases turn them another.
- Common household substances like lemon juice, vinegar, baking soda and bleach are identified along the pH scale.
- A
The document provides an overview of titration including terminology, basic concepts, and types of titrations. It defines titration as a quantitative analytical method to determine an analyte by reacting it with a titrant of known concentration. The key aspects covered are:
- Titration relies on a chemical reaction between the analyte and titrant, with the equivalence point determined.
- Common titration types include direct titration to determine the analyte directly, titer determination to find the accurate titrant concentration, and back titration where the analyte reacts indirectly.
- Calculations use the titrant volume, concentration, and titer along with constants to find the analyte amount or concentration in a sample
This document outlines a water quality field study to compare and contrast freshwater systems using various probes and tests. Students will measure temperature, conductivity, pH, and dissolved oxygen at multiple sites to analyze water health. They will also make visual observations and sample macroinvertebrates. The objectives are to understand factors affecting each measurement and how they indicate water quality. A hypothesis about site comparisons will be stated before collecting and analyzing data.
This document discusses various physicochemical parameters that are used to test water quality, including temperature, pH, electrical conductivity, carbon dioxide, alkalinity, bicarbonate, biochemical oxygen demand (BOD), and chemical oxygen demand (COD). It explains that water quality must be regularly monitored and tested against these parameters to ensure it is safe for drinking, domestic, agricultural, and industrial uses. Each parameter is important to measure as it provides insight into the water ecosystem and potential contamination issues.
This document provides instructions for using a compact laboratory kit to test water quality parameters.
The kit allows users to test for ammonium, carbonate hardness, total hardness, nitrate, nitrite, pH, phosphate, oxygen, and oxygen consumption. It includes reagents, test vessels, color comparison cards, and auxiliary tables to help interpret results.
Tests are based on colorimetric and titrimetric methods. The document provides definitions of key terms, testing principles and ranges, sampling guidance, and step-by-step instructions for each parameter. It also addresses potential influences on tests and how to perform method controls.
This document discusses the effect of electrolytes on the phase separation of aqueous-organic systems. Specifically, it examines how adding salts like sodium carbonate and sodium thiosulfate affects the cloud point temperature of a 2-propanol and water solution. The main findings are:
1) The cloud point temperature decreases as the concentration of added salt increases, indicating that salts enhance the "salting out" effect and promote phase separation at lower temperatures.
2) Sodium thiosulfate has a stronger salting out effect than sodium carbonate at the same concentration due to its higher solubility in water.
3) As the concentration of 2-propanol increases, the cloud point temperature also increases,
- pH is a measure of how acidic or basic a solution is, with values from 0 to 14. Solutions with a pH less than 7 are acidic and greater than 7 are basic.
- The pH scale is determined by international agreement and is based on standard buffer solutions. pH can be measured using a glass electrode and meter or indicators.
- pH is important in many applications including biology, medicine, agriculture and more. It is calculated as the negative logarithm of the hydronium ion concentration.
- For strong acids and bases, pH can be calculated directly from concentration but weak acids and bases require more complex calculations using acid dissociation constants and mass balances.
The document discusses various parameters for measuring water quality, including color, pH, turbidity, alkalinity, and hardness. It provides details on each parameter, including what they measure, typical units, and limits according to regulations. Color is measured in platinum-cobalt units and can be caused by dissolved impurities. pH indicates acidity and should be between 6.5-8.5. Turbidity refers to water clarity and is measured in Nephelometric Turbidity Units. Alkalinity and hardness measure a water sample's ability to neutralize acids and form precipitates with soap, respectively.
Study of abiotic factors across the brahmaputra belt in relation to its suita...eSAT Journals
Abstract
A healthy ecosystem is a result of balanced interaction between biotic and abiotic factors. Water temperature, pH, DO, FCO2, TA, TH etc are the most important abiotic factors influencing the physico-chemical and biological events of water body (Rahman et al., 2008). All species have their own optimal range for these abiotic parameters. In relation to aquatic life, there maturation time is also dependent on these parameters. These factors have great influence on aquatic life (DuttaMunshi and DuttaMunshi, 1995). This paper deals with the observation of fluctuation of these abiotic factors across the Brahmaputra Belt and its relation with aquatic life, mostly fishes.
Keywords: Water temperature, pH, DO, FCO2, TA, TH etc…
The document discusses various physical, chemical, and biological properties that are monitored in water resources, including:
1. Acidity, alkalinity, conductivity, color, phosphorus, nitrogen, and total solids. It describes methods for measuring these parameters and their environmental significance.
2. Hardness is discussed in detail, including what causes hard water, its effects on soap and limescale formation, and methods for softening hard water using heating or sodium carbonate.
3. Sources of parameters like phosphorus, nitrogen, and dissolved solids that can impact water quality are outlined. Maintaining appropriate levels of these is important for balancing aquatic life and human use of water resources.
Dissolved Oxygen Measurement Techniques and Aplications for the Water Quality...Valentina Giraldo
The document discusses various techniques for measuring dissolved oxygen levels in water samples, including electrochemical probes, titrimetric tests, and colorimetric tests. Clark electrochemical probes were found to be the most accurate and easiest to use. Field tests of five sites on the Passaic River found the highest dissolved oxygen levels at the upstream sites and lowest at a site downstream of road runoff. Issues with the biochemical oxygen demand tests highlighted the need for proper technique when using testing kits.
This document discusses determining the alkalinity of a water sample through titration with dilute sulfuric acid using phenolphthalein and methyl orange indicators. Alkalinity is a measure of a water's capacity to neutralize acids and is primarily due to carbonate, bicarbonate, and hydroxide ions. The procedure involves adding sodium carbonate and an indicator to a water sample, then titrating with acid and recording the endpoint color changes to calculate alkalinity concentration.
A STUDY ON OCEAN ACIDIFICATION DUE TO CARBON DIOXIDE ALONG THE COAST OF VISAK...Soma Sekhar Sriadibhatla
Extensive Data Analytics on samples to understand Ocean Acidification process, a serious damage to ecosystem, increase in production of Carbon dioxide.
This document discusses water technology and the analysis of water hardness. It outlines various sources of water including rainwater, surface water, groundwater, and seawater. Water can become impure through dissolving gases, minerals, and organic matter. Hardness in water is caused by calcium, magnesium, and other ions and prevents soap from lathering. Hardness can be temporary (removed by boiling) or permanent. The document describes methods for measuring hardness using EDTA titration and calculating hardness levels in terms of calcium carbonate equivalents and other units.
This document describes a procedure for determining water hardness through titration with EDTA. Water hardness is defined as the calcium and magnesium ion content and is reported in parts per million (ppm) of calcium carbonate. The titration uses EDTA to chelate calcium and magnesium ions until the indicator Eriochrome Black T changes color, signaling the endpoint. Standard solutions of calcium carbonate and EDTA are prepared and used to determine the concentration of EDTA and calculate water hardness based on the volume of EDTA needed to reach the endpoint in a sample.
The document summarizes an experiment that measured the hardness of various water samples through atomic absorption spectrophotometry (AA) and EDTA titration. AA found decreasing hardness in the order of two tap water samples, Fiji bottled water, and Aquafina bottled water. However, EDTA titration found decreasing hardness in the order of a tap water sample, Fiji water, another tap water, and Aquafina. Fiji water was found to have the highest magnesium concentration, likely due to geological differences between Fiji and the US. Aquafina's extensive filtration process resulted in immeasurably low hardness. Hardness varied between the two tap water samples possibly due to their source aquifers.
The document describes the Kjeldahl method for determining total nitrogen in a sample. It involves three main steps: digestion, distillation, and titration. In digestion, the sample is broken down in sulfuric acid to convert nitrogen into ammonium ions. Distillation transforms ammonium ions into ammonia gas, which is captured in an absorbing solution. Finally, titration uses sulfuric acid to determine the amount of ammonia in the solution, allowing calculation of the nitrogen content in the original sample. The Kjeldahl method is commonly used to indirectly estimate protein content through nitrogen levels and provides important information about water quality and soil fertility.
The document discusses the challenges of accurately measuring pH in deionized water due to its low ionic strength and buffering capacity. It explains that resistivity can be used instead to infer pH, as deionized water with 18.2 MΩ resistivity will have a neutral pH of 7. The types of ions present from dissolved salts affect pH, depending on if they come from strong acids/bases or weak acids/bases. Different deionization system configurations like SAC-WBA or SAC-SBA will produce characteristically lower or higher pH ranges due to the ions they remove or don't remove.
The document summarizes an experiment to measure the alkalinity of various water samples. Four samples were tested - tap water, bottled water, and two unknown solutions. Titration was performed using phenolphthalein and bromocresol green indicators to determine the phenolphthalein alkalinity and total alkalinity. The unknown samples had higher alkalinity levels than the tap and bottled water. Alkalinity is important to understand the buffering capacity of water and its ability to neutralize acids. The titration process and indicators help identify the presence of carbonate, bicarbonate, and hydroxide ions and determine the sample's alkalinity in mg/L CaCO3 units
1. Minnesota State University
Measuring Alkalinity, Acidity, and
Hardness to determine Water Quality
Fall
13
Written by: Raquel Collison
ABSTRACT – Alkalinity, acidity, and hardness have been classified as three important factors affecting
Minnesota State University’s tap water quality. The various experiments conducted to test the stated factors were
performed using a burette and cold tap water and three trials were noted to represent each qualification standard.
The results revealed that the water properties (in respective order) stated that the water had a high alkalinity
(29.33 ppm of CaCO3), lower acidity (8 ppm of CaCO3), and was classified to have a hardness value of 210
(ppm of CaCO3). From this information conclusions were made regarding the low sensitivity of the sample
water supply towards additional acid (such as polluted rain), representing its fertility in a natural system, as well
as be classified with a hardness rating of “hard,” which signifies a greater dissolved metal content than other
chemically treated waters. This information then can be better understood as means of classification of
Mankato’s water supply and as a basis for any treatment options that may be required.
2. Water quality control measures have been taken across the United States for
concerns relative to both the natural environment and human use. These concerns
are almost always symbiotic, representative of the need for consistent monitoring of
the three largest factors that contribute to water quality: alkalinity, acidity, and
hardness. In this experiment, we will investigate the three factors and determine an
average for each, so that we can better understand the makeup and chemical
balance of Mankato State University’s tap water system in order to make valid
conclusions relative to quality as dictated by the various ranking systems proposed.
The classification guidelines are defined as follows:
Alkalinity represents the ability of water molecules to accept H+ protons. In
short, it signifies the capacity of water to neutralize acids that may stem from acid
rain, for example. A high alkalinity means that a lake is fertile and buffered, in other
words, its pH does change enough to affect the aquatic animals, and so life thrives in
such a water body with a high alkalinity.
Acidity represents the ability of water molecules to neutralize OH- molecules,
the exact opposite of alkalinity. Acidic water typically has a high CO2 concentration,
which in usually high levels can lead to eutrophication of a water body.
Eutrophication is the resulting death of a lake caused by the oxygen – depleting
process of dead algae breakdown by microbes (“The Carbon Dioxide Greenhouse
Effect,” 2013).
Water hardness is computed by analyzing the concentration of dissolved
metals found in a water body – specifically calcium and magnesium – which can
Introduction
3. affect the efficiency of societal processes. For example, heavy metal machinery that
work with vast amounts of water perform more economically when the water is soft
(containing very little dissolved metal compounds) because there is less corrosion
and thus, less money is spent in costly maintenance (“Water Hardness and
Alkalinity,” n.d.).
In this report, we will be analyzing three separate experiments in order to
determine the general water quality of Mankato’s tap water system. The results will
allow us to make valid conclusions based upon the chemical makeup of the water,
which will furthermore allow us to better understand the effects that alkalinity,
acidity, and hardness have on our changing world.
4. Alkalinity. Observations relative to the amount of sulfuric acid needed to put cold
tap water at a pH of 4.5 appeared consistent within our group’s data. After the addition of
the acid to each 25 mL water sample, we noted the amount lost from the burette in order
to calculate the volume required to change the water with the added buffer (bromocresol
green – methyl indicator) into a yellow hue. Our findings can be expressed in Table 1.
Titration trial run 1 2 3
Volume of water
sample (mL)
25 25 25
Initial burette
reading of acidic
solution (mL)
5.0 3.5 4.3
Final burette reading
of EDTA solution
(mL)
5.7 4.3 5.0
Amount of acid
added to water (mL)
0.7 0.8 0.7
Ppm of CaCO3 28 32 28
Methods
Results
Table 1. Calculations relative to finding alkalinity of tap water through the
addition of an acid.
Average alkalinity = 29.33
Standard Deviation = 2.31
Please refer to the three attached handouts in regards to the materials and methods used in in the
alkalinity, acidity, and hardness labs respectively
5. According to the results, the average amount of sulfuric acid required to bring the
solution to a yellow hue (which represents the pH change of the water to 4.5) is around
0.7 mL. The alkalinity was calculated as follows:
CaCO3 = [(0.02)(mL of acid)(50,000)] / 25
Where: CaCO3 represents alkalinity in mg/L
0.02 represents the normality of the acid
25 represents the water sample volume in mL
Table 2 refers to relative alkaline levels in mg/L and their effect on a water body.
According to the results from the experiment, our resulting average alkalinity
level fell into the “not sensitive” level, which will be mentioned to a greater extent in the
Discussion.
United States EPA Category Concentration of CaCO3 (in mg/L)
Acidified < 1
Critical < 2
Endangered 2 - 5
Highly Sensitive 5 - 10
Sensitive 10 - 20
Not Sensitive > 20
Table 2. Distribution of the concentration of CaCO3 as dictated by the EPA1.
6. Acidity. Observations relative to the amount of base required to bring the cold tap
water solution to a pH of 8.3 were as follows in Table 3.
According to the results, the average amount of basic solution needed to put the
water at a pH of 8.3, was 0.2 mL (which turned the solution [with the added
phenothaliene indicator] pink). The acidity was calculated as follows:
CaCO3 = [(0.02)(mL of base)(50,000)] / 25
Where: CaCO3 represents the acidity of the solution in mg/L
0.02 represents the normality of the base
25 represents the water sample volume in mL
Titration trial run 1 2 3
Volume of water
sample (mL)
25 25 25
Initial burette
reading of basic
solution (mL)
11.4 11.6 11.7
Final burette
reading of basic
solution (mL)
11.6 11.7 12
Amount of basic
solution added (mL)
0.2 0.1 0.3
Ppm of CaCO3
8 4 12
Table 3. Calculations relative to finding acidity of tap water through the addition of a
base.
Average Acidity = 8
Standard Deviation = 4
7. Due to the waters calculated higher number (8), we can now determine that that
the solution is more likely to neutralize H+ protons (alkaline), then to neutralize OH- ions
(acid).
Hardness. Observations relative to the amount of ethylenediaminetetraacetate
(EDTA) required to determine the hardness of the water is listed in Table 4.
According to the results, the average amount of EDTA solution needed to
determine water hardness (which turned the solution blue) was 10.5 mL. It was calculated
as follows:
Titration trial run 1 2 3
Volume of water
sample (mL)
50 50 50
Initial burette
reading of EDTA
solution (mL)
0 10.3 20.6
Final burette
reading of EDTA
solution (mL)
10.3 20.6 31.5
Amount of EDTA
solution added (mL)
10.3 10.3 10.9
Ppm of CaCO3
206 206 218
Table 4. Calculations relative to finding the hardness of tap water through the addition
of an EDTA solution
Average ppm of CaCO3 = 210
Standard Deviation = 6.93
8. CaCO3 = [(0.02)(mL of EDTA)(50,000)] / 50
Where: CaCO3 represents water hardness
0.02 represents the normality of the EDTA solution
50 represents the water sample volume in mL
From the equation and additional statistics from the experiment (Table 4), we
have determined the average hardness level to equal 210. Utilizing Table 5, we can define
the metal content as follows:
According to the chart, our average number of 210 falls into the “Hard” water
quality guideline, where there is a greater amount of dissolved ions, such as Na+, K+,
Ca2+, Mg2+, Cl-, and HCO3-, among others, in our tap water supply.
Hardness Level Water Class
0 - 75 Soft
75 - 150 Moderately Hard
150 - 300 Hard
Over 300 Very Hard
Table 5. Distribution of the amount of dissolved ions in water and their relative
hardness concentration classifications
9. The results we received from the alkalinity, acidity, and hardness labs
respectively play an important role in the understanding of the chemical properties of our
local water supply.
To begin, alkalinity represents the capacity of a water body to neutralize H+
protons; in other words, it is a buffer that prevents a lake or stream from becoming too
acidic for life to flourish. From the results of our alkalinity experiment, we have
determined the average water alkalinity level at 29.33 for Mankato’s tap water system.
According to Table 2 from the Results, our local water supply is not sensitive to possible
additions of acid, as alkalinity acts as a buffer.
In a natural environment, alkalinity plays a role in the fertility of a specific water
supply. In aquatic settings, a high alkalinity represents the water’s ability to neutralize
acid rain (additional H+ protons), for example, and maintain the pH of the system at a
relatively neutral 7 – 8 range. In these regards, animal life is able to flourish in an
environment that maintains a relatively constant pH. If a body of water has a low
alkalinity, the pH drops below seven and becomes acidic because there is little to no
buffer to neutralize the acid rain and so life becomes sparse or perishes. In general,
alkalinity represents the capacity of the water to accept H+ protons, while pH represents
the intensity relative to the quantity of H+ suspended in the water body. Most alkalinity
that is found naturally in water bodies comes from calcium carbonate (CaCO3).
Alkalinity is also important in agriculture – for the levels of both the soil and added water
must remain relatively equal.
Discussion
10. Acidity is the ability of water to neutralize OH- ions. In our lab experiment, we
concluded that the average acidity of the water tested was 8 mg/L. Because of eight’s
location on the pH scale (as shown in Figure 1), we can determine, and furthermore
support from the alkalinity test, that the water is more alkaline than acidic.
This means that our example water supply has a greater ability to neutralize H+ p
We calculated water hardness through finding the average amount of calcium
carbonate (CaCO3) in the sample, which resulted in 210 parts per million (ppm).
According to Table 5 from the Results section, our water sample had received a water
hardness classification of “hard” which represents that a greater amount of dissolved ions
were contained within the examples we used for each trial. In a human society, a water
body which is classified as “soft” has many important benefits. For example, household
detergents are more efficient when utilized with soft water, and factories that operate with
heavy machinery prefer soft water so that their machines run more efficiently and with
less corrosion over their lifetime. Relative to drinking water however, hard water can
actually be beneficial, for it contains many of the minerals we need that are not consumed
from our solid food diets.
Figure 1.
Retrieved from: http://www.abundanthealthcenter.com/blog/the-acid-alkaline-ph-scale
11. In conclusion, water quality is determined by symbiotic factors that can be
classified in order to make appropriate chemical treatment decisions that will better our
water supply for both human and animal abundance. Water is a very important resource,
and so it is with great importance that it is cared for and utilized in the most efficient way
possible.
12. 1Godfrey, P.J., Mattson M.D. , Walk, M.F. , Kerr P.A. , Zajicek, O.T., and Ruby, A.
(1996). “The Massachusetts Acid Rain Monitoring Project: Ten Years of
Monitoring Massachusetts Lakes and Streams with Volunteers.” University of
Massachusetts Water Resources Research Center. Received from
http://www.uri.edu/ce/wq/ww/Publications/pH&alkalinity.pdf.
2013, February). “The Carbon Dioxide Greenhouse Effect.” The Discovery of Global
Warming. Retrieved from http://www.aip.org/history/climate/co2.htm.
(n.d.). “Water Hardness and Alkalinity.” USGS – Water Quality Information.
Retrieved from http://water.usgs.gov/owq/hardness-alkalinity.html.
Please refer to the attached packets for more information.
References
Appendix