ph Alkalinity of Water
|
|
- Asher Norman
- 7 years ago
- Views:
Transcription
1 ph Alkalinity of Water DOC Based on ISO standard :1994 ph-metric Titration 0.4 to 20 mmol/l of Total Alkalinity 1. Introduction Alkalinity of water is its acid-neutralizing capacity. It is the sum of all the titratable bases. For many surface waters, alkalinity values are primarily a function of carbonate, bicarbonate, and hydroxide content. The measured values also may include contributions from borates, phosphates, silicates or other bases if these are present. Alkalinity is determined by end point titration with a strong acid solution. Phenolphthalein alkalinity abbreviated by p is also known as composite alkalinity which corresponds to titratable alkalinity at ph 8.3. Total alkalinity is also known as methyl red (methyl orange) endpoint alkalinity which corresponds to titratable alkalinity at ph 4.5. This application note is based on ISO standard :1994 (Water quality Determination of alkalinity Part 1: Determination of total and composite alkalinity). 2. Principle The phenolphthalein end point alkalinity or composite alkalinity abbreviated by p is the measurement by titration to the phenolphthalein end point (ph 8.3) of that portion of alkalinity arbitrarily attributed to all the hydroxyl c(oh - ) and half the carbonate (CaCO 3 ) content of water. P c(co 3 2- ) c(co 2aq ) + c(oh - ) c(h + ) +c(*) The methyl red (methyl orange) end point alkalinity is an arbitrary measurement of the total alkalinity of water, abbreviated TA, and is obtained by titration to the methyl red (methyl orange) indicator endpoint (ph 4.5) to assess the equivalent hydrogen carbonate (HCO 3 - ), carbonate (CaCO 3 ) and hydroxide (OH - ) concentration of water. TA 2 c(co 3 2- ) + c(hco 3 - ) + c(oh - ) c(h + ) +c(*) Note: In both cases, other buffering substances (*) such as ammonia, borate, phosphate silicate and organic anions may be included in the determination. The number of detected equivalent point depends on the initial ph of the solution. By definition, p is zero for water which has a ph value of 8.3 or less. The current standard uses HCl 0.1 eq/l as a titrant, but another strong acid such as H 2 SO eq/l can also be used. Results are normally expressed as mmol/l (or meq/l) of alkalinity but other units can be used (see Results section). Using an appropriate combined ph electrode with temperature, the alkalinity determination can be linked with a ph and temperature measurement of the sample. 3. Electrode and reagents Combined ph Electrode with Temperature sensor: Intellical PHC805 Titrant: HCl or H 2 SO eq/l solution in deionized water Deionized water 4. Ranges and settings 4.1. Default parameters The sample size and titrant concentration depend on the quality of the water. Using the application note settings described below with the following parameters: V sample = 100 ml Burette volume = 10 ml Titrant concentration = 0.1 eq/l (corresponding to a 0.1 mol/l HCl solution) Page 1 of 10
2 4.2. Working ranges In accordance with the norm ISO , the previous configuration with 0.1 eq/l of titrant HCl or H 2 SO 4, 10 ml-burette is done for a Total Alkalinity between 0.4 mmol/l (20 mg/l CaCO 3 ) corresponding to 0.4 ml of titrant 0.1 eq/l and 20 mmol/l (1000 mg/l CaCO 3 ) corresponding to 20 ml of titrant 0.1 eq/l. For the best accuracy and reproducibility, the result range is between 3.5 meq/l or 175 mg/l CaCO 3 for 35% of the cylinder 10 ml-burette capacity and 10 meq/l or 500 mg/l CaCO 3 for the cylinder 10 ml-burette capacity. With the same conditions, the "experimental" limit corresponding to a titrant volume of 0.5 ml is 0.5 meq/l or 25 mg/l CaCO 3. For low alkalinity, below 0.5 mmol/l or 25 mg/l CaCO 3 (corresponding to 0.5 ml of titrant 0.1 eq/l), it is recommended to use a low alkalinity method with 0.02 eq/l titrant and 200 ml for sample volume, using the calculation above. For high alkalinity, between 10 mmol/l (500 mg/l CaCO 3 ) and 20 mmol/l (1000 mg/l CaCO 3 ) it is recommended to use smaller sample volumes (less than 50 ml) with the same titrant 0.1 eq/l Settings Note: In the following tables, an x in the or column indicates that the parameter can be edited in that respective. Refer also to the User Manual Sample Default parameters: Setting Name x x Water s Amount x x 100 [ml] Settings for leveling (Method: leveling) If the option of an external pump is present on the device, the leveling method allows for the leveling of the sample at the beginning of the titration. Default parameters: Setting Active x x No s Time x x 30 [s] The time of the leveling has to be adapted depending on the amount of sample and the leveling tube Settings for ph measurement (Method: phi) By default the initial measurement of ph is done with the parameters described below: Setting Active x x Yes Max. stability time x 120 [s] Stability criterion x [ph/min] Stirring speed x x 25 [%] Settings for alkalinity measurement The alkalinities are measured using a 10-mL burette, an incremental addition and an End Point detection method with the parameters described below: Titrant settings used for the calculation: Setting Name x x HCl Titer x x 0.1 [eq/l] Page 2 of 10
3 Note: The Real concentration value is updated after each automatic or manual calibration of titrant. Detection settings: Results settings: R x Setting Active x x Yes Stirring speed x x 25 [%] Measured parameter Predose x x 0 [ml] Max. vol. stop point x 20 [ml] Ordinate stop point x 3.4 [ph] Stop on last EQP x Yes Delay x x 0 [s] Stability criterion x [mph/min] Min. increment size x 0.1 [ml] Max. increment size x 1.0 [ml] Equivalence point #1 x 8.3 [ph] Equivalence point #2 x 4.5 [ph] Result x name x x p ph R1 R2 R3 R4 Total Alkalinity p (1) Total Alkalinity (2) R x max. resolution x 3 decimals 3 decimals 1 decimal 1 decimal R x hide x x Yes Yes No No R x limit check x x Yes Yes Yes Yes R x min x x 0 mmol/l 0.4 mmol/l 0 mg/l as 20 mg/l as CaCO 3 CaCO 3 R x max x x 10 mmol/l 20 mmol/l 500 mg/l as 1000 mg/l as CaCO 3 CaCO 3 R x unit x mmol/l mmol/l mg/l as (1) CaCO 3 (2) mg/l as CaCO 3 R x EQP index x 1 2 N/A N/A R x equation x N/A N/A R3 = R2*FX (1) R3 = R2*FX (2) R x user value x x N/A N/A 50 (1) 50 (2) R x sample x 1 equivalent R x titrant 1 if HCl is used x equivalent 2 if H 2 SO 4 is used (1) (2) R3 (Phenolphthalein alkalinity): in the default settings, p is expressed in mg/l as CaCO 3 with the User Value set at 50. R4 (Total alkalinity): in the default settings, Total Alkalinity is expressed in mg/l as CaCO 3 with the User Value set at 50. For results R1 and R2, only the Name and the Rx max. resolution can be modified. R1 and R2 have to be expressed in mmol/l in order to have correct results for R3 and R4 as results of the equation. For results R3 and R4, R x max. resolution, R x min, R x max, R x unit and R x user value can be modified to express the results in alternative units using the R x user value from mmol/l (see Alternative units on page 5). Note: When the titrant is H 2 SO 4 some coefficients must be adjusted: Set the Name of the titrant and the Titrant equivalents value to 2 (refer to Mode in the User Manual). Page 3 of 10
4 4.4. Recommendations for modifications of settings Values of End points The values p ph 8.3 and TA ph 4.5 can be modified in the titration program depending on the sample: End point ph Test condition Phenolphthalein Total Alkalinity Alkalinity Alkalinity, 30 mg CaCO 3 /L Alkalinity, 150 mg CaCO 3 /L Alkalinity, 500 mg CaCO 3 /L Silicates, phosphates known or suspected Routine or automated analyses Industrial waste or complex system Modification of parameters To reduce the time of titration, a predose in volume (by default volume at 0 ml) prior to starting the titration followed by a delay of at least 5 seconds can be set. Ensure that the predose does not overshoot the end point by completely titrating the sample. 5. Procedure 5.1. Sample analysis Sampling This standard can be used with natural, drinking and wastewaters with TA between 0.4 and 20 mmol/l. The sample must not be filtered, diluted, concentrated or altered in any way. Avoid excessive agitation and prolonged exposure to air. Samples should be analyzed as soon as possible after collection but can be stored at least 24 hours by cooling to 4 C or below. Warm the sample to room temperature before analyzing Sample preparation Pipette 100 ml of water into the 150 ml-plastic beaker Analysis step Dip the electrode and delivery tip in the sample. Press Start. 6. Results 6.1. Displayed Results At the end of the titration the following results are available: 1. Value of phi 2. Value of p in mg/l as CaCO 3 (volume of titrant in ml to reach defined ph, 8.3 ph by default) 3. Value of Total Alkalinity in mg/l as CaCO 3 (volume in ml to reach defined ph, 4.5 ph by default) Note: Results in mmol/l are calculated but, by default, are hidden in the result screen. However, they are available in the Data Log (refer to the User Manual for additional information) Results calculation of Alkalinity in meq/l The results are normally expressed in mmoles/l (or meq/l) of alkalinity as described by the following relation: V(titr) C(titr) 1000 R = V(smp) V(titr) = Total volume of titrant in ml, delivered to reach the end point (e.g. ph 4.5) C(titr) = Titrant concentration in eq/l (currently 0.1 eq/l) V(smp) = Volume of the sample (currently 100 ml) With these parameters, 1 ml of 0.1 eq/l of strong acid represents 0.1 meq or mmol of alkalinity. Page 4 of 10
5 Alternative units Depending on the country, many other units can be used for the results. Factors for the conversion from millimoles per liter are given in the table below (column R x user value): R x user value Comments mmol/l CaCO CO 2-3 has 2 alkalinity functions per molecule mg/l CaCO 3 50 MW of CaCO 3 is g/mol with 2alkaline functions per molecule mg/l HCO 3 61 MW of HCO - 3 is 61 g/mol with 1 alkaline function per molecule Clark degree 3.50 German degree 2.80 French degree 5.0 U.S. degree Examples of ph-alkalinity determination The results described below are indicative and obtained for a given water type in optimized conditions respecting Good Laboratory Practices. These indicative values are sample-dependent, electrode-dependent and operating cell dependent ph Alkalinity determination of mineral water (phi < 8.3) Results for 5 determinations in milliequivalents/l: Sample: 100 ml of mineral water. Nominal concentration: 296 mg/l as CaCO 3 Settings: see values by default Number of determinations: 10 Temperature of analysis: room temperature Mean value of Total Alkalinity: mmol/l Standard deviation: mmol/l Relative standard deviation: 0.02% Curve ph versus volume of titrant: 7.2. ph Alkalinity determination of water with phi > 8.3 and high alkalinity Results for 10 determinations in milliequivalents/l: Sample: 100 ml of Na 2 CO 3 solution Nominal concentration: 250 mg/l as CaCO 3 Settings: see values by default Number of determinations: 10 Temperature of analysis: room temperature Mean value of Total Alkalinity: mmol/l Standard deviation: mmol/l Relative standard deviation: 0.26% Curve ph versus volume of titrant: 8. Bibliography Water quality - Determination of total and composite alkalinity, International standard ISO (1994) EPA method number Standard Methods For the Examination of Water and Wastewater, 22nd edition, 2012, 2-34 part 2320 Page 5 of 10
6 9. Appendices: Electrode and Titrant calibrations To increase accuracy of the measurement of ph-alkalinity of the sample, it is recommended to perform a calibration of the electrode and titrant every 7 days. Always perform a calibration for a new electrode and/or titrant Calibration of the electrode Note: In the following tables, an x in the or column indicates that the parameter can be edited in that respective. Refer also to the User Manual Electrode and reagents Combined ph Electrode with Temperature sensor: Intellical PHC805 Titrant: HCl or H 2 SO eq/l solution in deionized water IUPAC Series ph standards (500 ml): ph 4.005, ph and ph Electrode calibration Calibrate the electrode with ph 4.005, and ph IUPAC Series ph standards Electrode calibration settings By default the calibration of the electrode is done with the parameters described below: Setting Calibration frequency x x 7 [Day(s)] Stability criterion x [ph/min] Max. stability time x 300 [s] Stirring speed x x 25 [%] Buffer set x x IUPAC 1.68, 4.01, 7.00, 10.01, Results of electrode calibration At the end of the series of buffers, the results are displayed. The values given below are indicative results, obtained in optimized conditions respecting Good Laboratory Practices. These indicative values are sampledependent, electrode-dependent and operating cell dependent. Electrode PHC805 Slope at 25 C 99.2% Slope mv/ph Offset 10.5 mv 9.2. Calibration of the titrant by a primary standard: Borax Note: In the following tables, an x in the or column indicates that the parameter can be edited in that respective. Refer also to the User Manual Principle The strong acid (HCl or H 2 SO 4 ) used as titrant has to be calibrated with Borax which reacts with H + ions according to: B 4 O H + + H 2 O -> 4HBO Electrode and reagents Combined ph Electrode with Temperature sensor: Intellical PHC805 Titrant: HCl or H 2 SO eq/l solution in deionized water Standard solution: 95 mg of Borax (Na 2 B 4 O 7.10H 2 O) Deionized water Page 6 of 10
7 Default parameters The sample size and titrant concentration depend on the quality of the water. Use the application note settings described below with the following parameters: V sample = 100 ml Burette volume = 10 ml Titrant concentration = 0.1 eq/l (corresponding to a 0.1 mol/l HCl solution) Titrant calibration settings The sample size of the standard solution is set at 95 mg, completed to 100 ml with deionized water. The calibration is done using a 10-mL burette, a dynamic incremental addition and an Inflexion Point as the detection method with the parameters described below: Detection settings: Standard: Setting Stirring speed x x 25 [%] Predose x x 2 [ml] Max. vol. stop point x 8 [ml] Ordinate stop point x 2 [ph] Stop on last EQP x Yes Delay x x 5 [s] Stability criterion x [mph/min] Min. increment size x 0.02 [ml] Max. increment size x 0.8 [ml] EQP 1 min ordinate x 4.5 [ph] EQP 1 max ordinate x 6.5 [ph] Max. resolution x 4 decimals R1 limit check x Yes Min. titer x [eq/l] Max. titer x [eq/l] Setting Standard name x Borax Standard amount x 95 [mg] Min. amount x 90 [mg] Max. amount x 100 [mg] Concentration x x 99.5 [%] x [mg] Resolution x 1 decimal Standard equivalents x 2 x 1 if HCl is used Titrant equivalents 2 if H 2 SO 4 is used Molar weight x Note: When the titrant is H 2 SO 4 some coefficients must be adjusted: Set the Name of the titrant and the Titrant equivalents value to 2 (refer to Mode in the User Manual). Page 7 of 10
8 Results: At the end of the titrant calibration the titer is calculated and expressed in eq/l. The saved value will be used for the following Alkalinity titrations Procedure Setting Titer 0.1 [eq/l] A 0.1 eq/l Borax solution contains 0.05 mol/l (or 1/20 mol/l) of Borax. To calibrate the acidic titrant with the 10 ml-burette: 1. Prepare a 100-mL sample of 0.1 eq/l Borax solution by accurately weighing about 95 mg of Borax. 2. Complete to 100 ml with deionized water. 3. Dip the electrode and delivery tip in the solution. 4. Press Start Results of the titrant calibration The result is expressed as eq/l concentration of the titrant and based on the following formula: Where: [2 x m(sdt)x P% ] C(titr) = [M(sdt)x V(titr)] m(sdt) = Weighed mass of Borax in mg, about 95 mg weighed accurately M(sdt) = Molar weight of Borax, g/mol P % = Purity of the weighted powder, 99.5 % V(titr) = Total volume of titrant delivered to reach the equivalent point, in ml The calibration result can be accepted if 5 determinations give a result with a relative standard deviation of less than 0.5% Examples of titrant calibration Results for 10 determinations in milliequivalents/l The results described below are indicative and obtained for a given water type in optimized conditions respecting Good Laboratory Practices. These indicatives values are sample-dependent, electrode-dependent and operating cell dependent. Sample: 95 mg of Borax with purity 99.5% completed to 100 ml of distilled water Settings: see values by default Number of determinations: 5 Temperature of analysis: room temperature Titer of titrant: eq/l SD: eq/l RSD: 0.09 % Curve ph versus volume of titrant: Page 8 of 10
9 9.3. Calibration of the titrant by a secondary standard: NaOH Note: In the following tables, an x in the or column indicates that the parameter can be edited in that respective. Refer also to the User Manual Principle In some cases sodium hydroxide (NaOH) is used to calibrate HCl or H 2 SO 4 titrant despite the fact that NaOH is not suitable as a primary standard because it readily absorbs moisture (H 2 O) and carbon dioxide (CO 2 ) from the atmosphere. This classical reaction takes place: NaOH + H + --> H 2 O + Na Settings Detection settings: The limits of the inflexion points have to be adapted to the reaction. Standard settings for NaOH: Mode Mode Setting EQP 1 min ordinate x 6.5 [ph] EQP 1 max ordinate x 10.5 [ph] Mode Mode Setting Standard name x NaOH Standard amount x 100 [ml] Min. amount x 95 [ml] Max. amount x 105 [ml] Concentration x [%] x ml Resolution x 4 decimals Standard equivalents x 1 x 1 if HCl is used Titrant equivalents 2 if H 2 SO 4 is used Molar weight x [g/mol] Procedure To calibrate the acidic titrant with the 10 ml-burette: 1. Accurately prepare a 100 ml sample of eq/l NaOH freshly prepared solution. 2. Dip the electrode and delivery tip in the solution. 3. Press Start Results of the titrant calibration The result is expressed as eq/l concentration of the titrant and based on the following formula: Where: [ V(sdt) x C(sdt) ] C(titr) = V(titr) V(sdt) = Volume of NaOH solution in ml, ml C(sdt) = Concentration of NaOH solution in ml, eq/l V(titr) = Total volume of titrant delivered to reach the equivalent point, in ml The calibration result can be accepted if 5 determinations give a result with a relative standard deviation of less than 0.5%. Page 9 of 10
10 Examples of titrant calibration Results for 5 determinations in milliequivalents/l The results described below are indicative and obtained for a given water type in optimized conditions respecting Good Laboratory Practices. These indicatives values are sample-dependent, electrode-dependent and operating cell dependent. Titrant: H 2 SO 4 Sample: 100 ml of NaOH eq/l Settings: see values by default Number of determinations: 5 Temperature of analysis: room temperature Titer of titrant (Average): eq/l SD: eq/l RSD: % Curve ph versus volume of titrant: Note: For this curve, the calibration is stopped after a delivery of 8 ml of titrant and not after the last equivalent point is found Quality of the NaOH solution Over time, a slow degradation of the sodium hydroxide solution occurs which leads to a bad titrant calibration. As the solution absorbs carbon dioxide from the atmosphere, carbonate species appear and a second inflexion appears into the curve at low ph (between 5 and 4 ph). When such a profile is observed, the sodium solution should not be used for titrant calibration. Page 10 of 10
ph and Acidity in Tomato Sauce
ph and Acidity in Tomato Sauce DOC316.52.93100 Endpoint potentiometric titration Scope and application: Tomato sauce 1. Introduction This working procedure refers to the determination of titratable acidity
More informationph and Acidity in Wine and Fruit Juice
ph and Acidity in Wine and Fruit Juice DOC316.52.93089 Endpoint potentiometric titration Scope and application: Wine and fruit juice 1. Introduction This working procedure refers to the titration of total
More informationStandard Methods for the Examination of Water and Wastewater
2320 ALKALINITY*#(1) 2320 A. Introduction 1. Discussion Alkalinity of a water is its acid-neutralizing capacity. It is the sum of all the titratable bases. The measured value may vary significantly with
More informationChemistry 119: Experiment 7. Potentiometric Titration of Ascorbic Acid in Vitamin C Tablets
Chemistry 119: Experiment 7 Potentiometric Titration of Ascorbic Acid in Vitamin C Tablets Vitamin C is another name for ascorbic acid (C 6 H 8 O 6, see below ), a weak acid that can be determined by titration
More informationph: Measurement and Uses
ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic
More informationTo determine the equivalence points of two titrations from plots of ph versus ml of titrant added.
Titration Curves PURPOSE To determine the equivalence points of two titrations from plots of ph versus ml of titrant added. GOALS 1 To gain experience performing acid-base titrations with a ph meter. 2
More informationDetermination of calcium by Standardized EDTA Solution
Determination of calcium by Standardized EDTA Solution Introduction The classic method of determining calcium and other suitable cations is titration with a standardized solution of ethylenediaminetetraacetic
More informationph units constitute a scale which allows scientists to determine the acid or base content of a substance or solution. The ph 0
ACID-BASE TITRATION LAB PH 2.PALM INTRODUCTION Acids and bases represent a major class of chemical substances. We encounter them every day as we eat, clean our homes and ourselves, and perform many other
More informationPreparation of frequently used solutions
Preparation of frequently used solutions Content 1. Diluting Concentrated Acids (Last Login: 08/08/2009) 2. Indicators (Last Login: 27/07/2009) 3. Standard Buffer Solutions (Last Login: 27/07/2009) 4.
More informationPotentiometric determination. Application Bulletin 125/3 e. Branch General analytical laboratories; water analysis; beverages
Simultaneous determination of calcium, magnesium, and photometric indication in water and beverage samples Branch General analytical laboratories; water analysis; beverages Keywords Titration; potentiometric
More informationVolumetric Analysis. Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115
Volumetric Analysis Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115 Experimental Aims To prepare and standardize (determine concentration) a NaOH solution Using your standardized NaOH calculate
More informationI. ACID-BASE NEUTRALIZATION, TITRATION
LABORATORY 3 I. ACID-BASE NEUTRALIZATION, TITRATION Acid-base neutralization is a process in which acid reacts with base to produce water and salt. The driving force of this reaction is formation of a
More informationDETERMINATION OF PHOSPHORIC ACID CONTENT IN SOFT DRINKS
DETERMINATION OF PHOSPHORIC ACID CONTENT IN SOFT DRINKS LAB PH 8 From Chemistry with Calculators, Vernier Software & Technology, 2000 INTRODUCTION Phosphoric acid is one of several weak acids that present
More informationEvaluation copy. Titration of a Diprotic Acid: Identifying an Unknown. Computer
Titration of a Diprotic Acid: Identifying an Unknown Computer 25 A diprotic acid is an acid that yields two H + ions per acid molecule. Examples of diprotic acids are sulfuric acid, H 2 SO 4, and carbonic
More informationProperties of Acids and Bases
Lab 22 Properties of Acids and Bases TN Standard 4.2: The student will investigate the characteristics of acids and bases. Have you ever brushed your teeth and then drank a glass of orange juice? What
More informationD. LAB 4. ACID-BASE TITRATIONS, ALKALINITY, AND BUFFER CAPACITY
D. LAB 4. ACID-BASE TITRATIONS, ALKALINITY, AND BUFFER CAPACITY Introduction In this lab, you will titrate several solutions of known composition as well as the samples collected in the first weeks of
More informationACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND
#3. Acid - Base Titrations 27 EXPERIMENT 3. ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this experiment a solution of hydrochloric
More informationAcid Base Titrations
Acid Base Titrations Introduction A common question chemists have to answer is how much of something is present in a sample or a product. If the product contains an acid or base, this question is usually
More informationDetermination of the amount of sodium carbonate and sodium hydroxide in a mixture by titration.
Module 9 : Experiments in Chemistry Lecture 38 : Titrations : Acid-Base, Redox and Complexometric Objectives In this lecture you will learn the techniques to do following Determination of the amount of
More information15. Acid-Base Titration. Discover the concentration of an unknown acid solution using acid-base titration.
S HIFT INTO NEUTRAL 15. Acid-Base Titration Shift into Neutral Student Instruction Sheet Challenge Discover the concentration of an unknown acid solution using acid-base titration. Equipment and Materials
More informationDetermination of the Amount of Acid Neutralized by an Antacid Tablet Using Back Titration
Determination of the Amount of Acid Neutralized by an Antacid Tablet Using Back Titration GOAL AND OVERVIEW Antacids are bases that react stoichiometrically with acid. The number of moles of acid that
More informationAcid-Base Titrations Using ph Measurements
Acid-Base Titrations Using ph Measurements Introduction According to the Brønsted Lowry definition, an acid is a substance that donates a hydrogen ion and a base is a substance which will accept a hydrogen
More informationChemical equilibria Buffer solutions
Chemical equilibria Buffer solutions Definition The buffer solutions have the ability to resist changes in ph when smaller amounts of acid or base is added. Importance They are applied in the chemical
More informationTITRATION CURVES, INDICATORS, AND ACID DISSOCIATION CONSTANTS
TITRATION CURVES, INDICATORS, AND ACID DISSOCIATION CONSTANTS Adapted from "Chemistry with Computers" Vernier Software, Portland OR, 1997 INTRODUCTION Titration is the volumetric measurement of a solution
More informationCustomer application report
16 Cape Town drinking water monitoring solution from Metrohm On 28 July 2010, the General Assembly of the United Nations declared clean water and sanitation as a fundamental human right! This underlines
More informationWater Softening for Hardness Removal. Hardness in Water. Methods of Removing Hardness 5/1/15. WTRG18 Water Softening and Hardness
Water Softening for Removal 1 in Water High concentration of calcium (Ca2+) and magnesium (Mg2+) ions in water cause hardness Generally, water containing more than 100 mg/l of hardness expressed as calcium
More information5.0 EXPERIMENT ON DETERMINATION OF TOTAL HARDNESS
5.0 EXPERIMENT ON DETERMINATION OF TOTAL HARDNESS Sl. No. Contents Preamble 5.1 Aim 5.2 Introduction 5.2.1 Environmental Significance 5.3 Principle 5.4 Materials Required 5.4.1 Apparatus Required 5.4.2
More informationExperiment 6 Titration II Acid Dissociation Constant
6-1 Experiment 6 Titration II Acid Dissociation Constant Introduction: An acid/base titration can be monitored with an indicator or with a ph meter. In either case, the goal is to determine the equivalence
More informationTopic 18 Acids and Bases. 18.1 Exercises
Topic 18 Acids and Bases 18.1 Exercises 1. Define: (a) ph The negative log of the hydrogen ion concentration in a solution. i.e. ph = log[h 3 O + ] (b) poh The negative log of hydroxide ion concentration
More informationCHM1 Review for Exam 12
Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and
More informationEXPERIMENT 20: Determination of ph of Common Substances
Materials: ph paper and color chart (ph range 3 to 12) or ph meter distilled water white vinegar household ammonia (or baking soda) spot plate test or 3 small test tubes stirring rod solutions / fruits
More informationDirect ISE Method Method 8359 10 to 1000 mg/l Na + Sodium ISE
Sodium DOC316.53.01240 Direct ISE Method Method 8359 10 to 1000 mg/l Na + Sodium ISE Scope and application: For drinking water and process water. Test preparation Instrument-specific information This procedure
More informationTotal Water Hardness
Test 14 INTRODUCTION When water passes through or over deposits such as limestone, the levels of Ca 2+, Mg 2+, and HCO Ð 3 ions present in the water can greatly increase and Hard-Water Cations cause the
More informationAcid Base Titrations in Aqueous Solvents
Acid Base Titrations in Aqueous Solvents Introduction: All kind of titrations in various samples are performed today in process analysers and laboratories, by far the most of them are acid base titrations.
More informationContinuous process of sodium bicarbonate production by Solvay method
Continuous process of sodium bicarbonate production by Solvay method Manual to experiment nr 10 Instructor: Dr Tomasz S. Pawłowski 1 Goal of the experiment The goal of the experiment is introduction of
More informationAdditional Lecture: TITRATION BASICS
Additional Lecture: TITRATION BASICS 1 Definition and Applications Titration is the incremental addition of a reagent solution (called titrant) to the analyte until the reaction is complete Common applications:
More informationPhenolphthalein-NaOH Kinetics
Phenolphthalein-NaOH Kinetics Phenolphthalein is one of the most common acid-base indicators used to determine the end point in acid-base titrations. It is also the active ingredient in some laxatives.
More informationTo see how this data can be used, follow the titration of hydrofluoric acid against sodium hydroxide below. HF (aq) + NaOH (aq) H2O (l) + NaF (aq)
Weak Acid Titration v120413 You are encouraged to carefully read the following sections in Tro (2 nd ed.) to prepare for this experiment: Sec 4.8, pp 158-159 (Acid/Base Titrations), Sec 16.4, pp 729-43
More informationFormulas, Equations and Moles
Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule
More informationChem 1B Saddleback College Dr. White 1. Experiment 8 Titration Curve for a Monoprotic Acid
Chem 1B Saddleback College Dr. White 1 Experiment 8 Titration Curve for a Monoprotic Acid Objectives To learn the difference between titration curves involving a strong acid with a strong base and a weak
More informationQUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN -
QUESTION (2012:3) (i) Complete the table below showing the conjugate acids and bases. Conjugate acid Conjugate base - HCO 3 2 CO 3 H 2 O OH HCN CN - (ii) HPO 4 2 (aq) Write equations for the reactions
More informationTitrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration
Acid-Base Indicators and Titration Curves Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical
More informationEstimation of Hardness of Water by EDTA Method
Estimation of Hardness of Water by EDTA Method 1 EXPERIMENT 1 Estimation of Hardness of Water by EDTA Method INTRODUCTION Water hardness is the traditional measure of the capacity of water to precipitate
More informationExperiment 4 (Future - Lab needs an unknown)
Experiment 4 (Future - Lab needs an unknown) USING A ph TITRATION TO DETERMINE THE ACID CONTENT OF SOFT DRINKS 2 lab periods Reading: Chapter 9, 185-197; Chapter 10, pg 212-218; Chapter 14 pg 317-323,
More informationChem101: General Chemistry Lecture 9 Acids and Bases
: General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water
More informationENE 806, Project Report 3 CHEMICAL PRECIPITATION: WATER SOFTENING. Grégoire Seyrig Wenqian Shan
ENE 806, Project Report 3 CHEMICAL PRECIPITATION: WATER SOFTENING Grégoire Seyrig Wenqian Shan College of Engineering, Michigan State University Spring 2007 ABSTRACT The groundwater with high level initial
More informationAcid-Base Titrations. Setup for a Typical Titration. Titration 1
Titration 1 Acid-Base Titrations Molarities of acidic and basic solutions can be used to convert back and forth between moles of solutes and volumes of their solutions, but how are the molarities of these
More informationWe remember that molarity (M) times volume (V) is equal to moles so this relationship is the definition of the equivalence point.
Titrations Titration - a titration is defined as the determination of the amount of an unknown reagent (analyte) through the use of a known amount of another reagent (titrant) in an essentially irreversible
More informationAcid Dissociation Constants and the Titration of a Weak Acid
Acid Dissociation Constants and the Titration of a Weak Acid One of the most important applications of equilibria is the chemistry of acids and bases. The Brønsted-Lowry acid-base theory defines an acid
More informationElectrical Conductivity of Aqueous Solutions
Electrical Conductivity of Aqueous Solutions PRE-LAB ASSIGNMENT: Reading: Chapter 4.-4.3 in Brown, LeMay, Bursten & Murphy.. Using Table in this handout, determine which solution has a higher conductivity,.
More informationQ.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base A4 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA 1. LEWIS acid electron pair acceptor H, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N BF 3 see
More informationLESSON ASSIGNMENT. After completing this lesson, you should be able to: 7-1. Solve basic titration problems.
LESSON ASSIGNMENT LESSON 7 Titration. TEXT ASSIGNMENT Paragraphs 7-1 through 7-5. LESSON OBJECTIVES After completing this lesson, you should be able to: 7-1. Solve basic titration problems. 7-2. Convert
More informationCHEMICAL PRECIPITATION: WATER SOFTENING
CHEMICAL PRECIPITATION: WATER SOFTENING Submitted to: Dr. Hashsham Research Complex Engineering Department of Civil and Environmental Engineering Michigan State University East Lansing, MI 4884 Authors
More informationComplexometric Titration Analysis of Ca 2+ and Mg 2+ in seawater
Complexometric Titration Analysis of Ca 2+ and Mg 2+ in seawater Introduction As the mountains on the continents are draped with snow, the mountains on the ocean floor are draped with sediment rich in
More informationTitration curves. Strong Acid-Strong Base Titrations
Titration curves A titration is a procedure for carrying out a chemical reaction between two solutions by the controlled addition from a buret of one solution (the titrant) to the other, allowing measurements
More informationEXPERIMENT 2 THE HYDROLYSIS OF t-butyl CHLORIDE. PURPOSE: To verify a proposed mechanism for the hydrolysis of t-butyl Chloride.
PURPOSE: To verify a proposed mechanism for the hydrolysis of t-butyl Chloride. PRINCIPLES: Once the Rate Law for a reaction has been experimentally established the next step is its explanation in terms
More informationThe Determination of Acid Content in Vinegar
The Determination of Acid Content in Vinegar Reading assignment: Chang, Chemistry 10 th edition, pages 153-156. Goals We will use a titration to determine the concentration of acetic acid in a sample of
More informationComplexometric Titrations
Complexometric Titrations Complexometric titrations are based on the formation of a soluble complex upon the reaction of the species titrated with the titrant. M + L ML In the module Chemistry 2 you were
More informationNitrogen, Ammonia. Known Addition ISE Method 1 Method 10002 Minimum of 0.8 mg/l NH 3 N. Ammonia ISE. Test preparation. Instrument-specific table
Nitrogen, Ammonia DOC316.53.01234 Known Addition ISE Method 1 Method 10002 Minimum of 0.8 mg/l NH 3 N Scope and application: For wastewater 2. Ammonia ISE 1 Adapted from the Standard Methods for the Examination
More informationCalculation of Molar Masses. Molar Mass. Solutions. Solutions
Molar Mass Molar mass = Mass in grams of one mole of any element, numerically equal to its atomic weight Molar mass of molecules can be determined from the chemical formula and molar masses of elements
More informationTITRATION OF VITAMIN C
TITRATION OF VITAMIN C Introduction: In this lab, we will be performing two different types of titrations on ascorbic acid, more commonly known as Vitamin C. The first will be an acid-base titration in
More informationEquilibrium Constants The following equilibrium constants will be useful for some of the problems.
1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO
More informationGA/7 Potentiometric Titration
Rev. 7/99 7-1 INTRODUCTION GA/7 Potentiometric Titration The potentiometric titration is a useful means of characterizing an acid. The ph of a solution is measured as a function of the amount of titrant
More informationQ.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base 2816 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA LEWIS acid electron pair acceptor H +, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N + BF
More informationHot water extractable acidity or alkalinity of paper (Reaffirmation of T 428 om-08) (No changes from Draft 1)
NOTICE: This is a DRAFT of a TAPPI Standard in ballot. Although available for public viewing, it is still under TAPPI s copyright and may not be reproduced or distributed without permission of TAPPI. This
More informationPractical Lesson No 4 TITRATIONS
Practical Lesson No 4 TITRATIONS Reagents: 1. NaOH standard solution 0.1 mol/l 2. H 2 SO 4 solution of unknown concentration 3. Phenolphthalein 4. Na 2 S 2 O 3 standard solution 0.1 mol/l 5. Starch solution
More information9. Analysis of an Acid-Base Titration Curve: The Gran Plot
9. Analysis of an Acid-Base Titration Curve: The Gran Plot In this experiment, you will titrate a sample of pure potassium hydrogen phthalate (Table 10-4) with standard NaOH. A Gran plot will be used to
More informationThe Relationship between ph and Deionized Water
The Relationship between ph and Deionized Water The basics of ph The topic of ph and water has been well documented over the years; however, there is still much confusion about its significance in high
More informationFactors Affecting Precipitation of Calcium Carbonate
Factors Affecting Precipitation of Calcium Carbonate John A. Wojtowicz Chemcon Laboratory tests with clear solutions showed that precipitation of calcium carbonate does not occur in the ph range 7.5 to
More informationNeutralizing an Acid and a Base
Balancing Act Teacher Information Objectives In this activity, students neutralize a base with an acid. Students determine the point of neutralization of an acid mixed with a base while they: Recognize
More informationExperiment 7: Titration of an Antacid
1 Experiment 7: Titration of an Antacid Objective: In this experiment, you will standardize a solution of base using the analytical technique known as titration. Using this standardized solution, you will
More informationF321 MOLES. Example If 1 atom has a mass of 1.241 x 10-23 g 1 mole of atoms will have a mass of 1.241 x 10-23 g x 6.02 x 10 23 = 7.
Moles 1 MOLES The mole the standard unit of amount of a substance (mol) the number of particles in a mole is known as Avogadro s constant (N A ) Avogadro s constant has a value of 6.02 x 10 23 mol -1.
More information4.1 Stoichiometry. 3 Basic Steps. 4. Stoichiometry. Stoichiometry. Butane Lighter 2C 4 H 10 + 13O 2 10H 2 O + 8CO 2
4. Stoichiometry 1. Stoichiometric Equations 2. Limiting Reagent Problems 3. Percent Yield 4. Limiting Reagent Problems 5. Concentrations of Solutes 6. Solution Stoichiometry 7. ph and Acid Base Titrations
More informationChemistry 201. Practical aspects of buffers. NC State University. Lecture 15
Chemistry 201 Lecture 15 Practical aspects of buffers NC State University The everyday ph scale To review what ph means in practice, we consider the ph of everyday substances that we know from experience.
More informationAcetic Acid Content of Vinegar: An Acid-Base Titration E10-1
Experiment 10 Acetic Acid Content of Vinegar: An Acid-Base Titration E10-1 E10-2 The task The goal of this experiment is to determine accurately the concentration of acetic acid in vinegar via volumetric
More informationph Measurement and Control
ph Measurement and Control Tech Tip #14 1997 I. The Need for ph II. ph System Requirements III. ph Electrode Conditioning Procedures IV. How the electrode works V. Identifying the Electrode Components
More information4.0 EXPERIMENT ON DETERMINATION OF CHLORIDES
4.0 EXPERIMENT ON DETERMINATION OF CHLORIDES Sl. No. Contents Preamble 4.1 Aim 4.2 Introduction 4.2.1 Environmental Significance 4.3 Principle 4.4 Materials Required 4.4.1 Apparatus Required 4.4.2 Chemicals
More informationExperiment 17: Potentiometric Titration
1 Experiment 17: Potentiometric Titration Objective: In this experiment, you will use a ph meter to follow the course of acid-base titrations. From the resulting titration curves, you will determine the
More informationph Measurements of Common Substances
Chem 100 Section Experiment 10 Name Partner s Name Introduction ph Measurements of Common Substances The concentration of an acid or base is frequently expressed as ph. Historically, ph stands for the
More informationSyllabus OC18 Use litmus or a universal indicator to test a variety of solutions, and classify these as acidic, basic or neutral
Chemistry: 9. Acids and Bases Please remember to photocopy 4 pages onto one sheet by going A3 A4 and using back to back on the photocopier Syllabus OC18 Use litmus or a universal indicator to test a variety
More informationUnderstanding hydrogen ion concentration (ph)
World Bank & Government of The Netherlands funded Training module # WQ - 06 Understanding hydrogen ion concentration (ph) New Delhi, May 1999 CSMRS Building, 4th Floor, Olof Palme Marg, Hauz Khas, New
More information1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11
SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436
More informationLab #10 How much Acetic Acid (%) is in Vinegar?
Lab #10 How much Acetic Acid (%) is in Vinegar? SAMPLE CALCULATIONS NEED TO BE DONE BEFORE LAB MEETS!!!! Purpose: You will determine the amount of acetic acid in white vinegar (sold in grocery stores)
More informationA Beer s Law Experiment
A Beer s Law Experiment Introduction There are many ways to determine concentrations of a substance in solution. So far, the only experiences you may have are acid-base titrations or possibly determining
More informationExperiment 16-Acids, Bases and ph
Definitions acid-an ionic compound that releases or reacts with water to form hydrogen ion (H + ) in aqueous solution. They taste sour and turn litmus red. Acids react with certain metals such as zinc,
More informationProtocol: HPLC (amino acids)
Page 1 of 6 1. Chemicals Composition M MW gram volume (ml) product code 0-pthaldialdehyde C 8H 6O 2 134.13 Sigma P0657 Perchloric acid HClO 4 3.5 100.46 Dilute 70% stock solution 1:1 with demi to obtain
More informationDetermination of the total acid number in petroleum products
Branch General analytical chemistry; petrochemistry Keywords Titration; nonaqueous titration; potentiometric titration; Solvotrode easyclean, Optrode; Thermoprobe; photometric titration; thermometric titration;
More informationEXPERIMENT 7. Identifying a Substance by Acid-Base Titration
EXPERIMENT 7 Identifying a Substance by Acid-Base Titration SAFETY WARNING In this experiment you will be working with NaOH pellets and using 0.25 M NaOH as a titrant. Sodium hydroxide is extremely basic,
More informationAcid Base Titration: ph Titration Curve
Acid Base Titration: ph Titration Curve OVERVIEW In this experiment, you will perform a ph-monitored titration of acetic acid and of an unknown acid. From the ph titration of the acetic acid, you will
More informationWrite the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present.
Chapter 16 Acids and Bases Concept Check 16.1 Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO 2. They called
More informationColor, True and Apparent
Color, True and Apparent DOC316.53.01037 Platinum-Cobalt Standard Method 1, 2, 3 Method 8025 15 to 500 color units Scope and application: For water, wastewater and seawater; equivalent to NCASI method
More information18 Conductometric Titration
Lab Activity 18 CONDUCTOMETRIC TITRATION LAB ACTIVITY 18 Conductometric Titration Background Titration is the a method of determining the concentration of an unknown solution (the analyte) by reacting
More informationChem 321 Lecture 13 - Acid-Base Titrations 10/10/13
Student Learning Objectives Chem 321 Lecture 13 - Acid-Base Titrations 10/10/13 Indicators A common end point for acid-base titrations is the color change associated with an acid-base indicator. An acid-base
More informationLab 25. Acid-Base Titration and Neutralization Reactions: What Is the Concentration of Acetic Acid in Each Sample of Vinegar?
Lab 25. Acid-Base Titration and Neutralization Reactions: What Is the Concentration of Acetic Acid in Each Sample of Vinegar? Introduction Vinegar is basically a solution of acetic acid (CH3COOH). It is
More informationDissolving of sodium hydroxide generates heat. Take care in handling the dilution container.
TITRATION: STANDARDIZATION OF A BASE AND ANALYSIS OF STOMACH ANTACID TABLETS 2009, 1996, 1973 by David A. Katz. All rights reserved. Reproduction permitted for education use provided original copyright
More informationColor, True and Apparent
Color, True and Apparent DOC316.53.01037 Platinum-Cobalt Standard Method 1, 2, 3 Method 8025 15 to 500 color units 5 to 500 color units (low range technique) Scope and application: For water, wastewater
More informationEXPERIMENT 12 A SOLUBILITY PRODUCT CONSTANT
PURPOSE: 1. To determine experimentally the molar solubility of potassium acid tartrate in water and in a solution of potassium nitrate. 2. To examine the effect of a common ion on the solubility of slightly
More informationUSEPA Electrode Method Method 8156
ph DOC316.53.01245 USEPA Electrode Method Method 8156 Scope and application: For drinking water 1, wastewater 2 and process water. 1 Based on Standard Method 4500-H+B, ASTM Method D1293-95 and USEPA Method
More informationDetermining the Identity of an Unknown Weak Acid
Purpose The purpose of this experiment is to observe and measure a weak acid neutralization and determine the identity of an unknown acid by titration. Introduction The purpose of this exercise is to identify
More informationOXIDATION-REDUCTION TITRATIONS-Permanganometry
Experiment No. Date OXIDATION-REDUCTION TITRATIONS-Permanganometry INTRODUCTION Potassium permanganate, KMnO 4, is probably the most widely used of all volumetric oxidizing agents. It is a powerful oxidant
More information