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titration experiment of hcl and naoh

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3 Determination of the Concentration of a Solution of Sodium Hydroxide

To determine the concentration of an unknown hydrochloric acid solution using acid-base titration methods.

Expected Learning Outcomes

  • Describe and perform an acid-base titration experiment using indicators to find the end point.

Solve stoichiometry problems in the solution phase.

Textbook Reference

Tro,  Chemistry: Structures and Properties , 2nd Ed, Ch. 8.7.

Introduction

Acid-base chemistry, definitions.

There are a number of different definitions of acids and bases present. However, for most purposes, the Brønsted-Lowry definition of acids and bases are the most useful:

  • An acid is a proton (H + ) donor. Common examples include hydrochloric (muriatic) acid, citric acid, and ascorbic acid (Vitamin C).
  • A base is a proton acceptor. Among the best known of these substances are hydroxides, such as sodium hydroxide; however, other bases exist. Examples of these include sodium bicarbonate (baking soda) and sodium hypochlorite (bleach).

\textrm{CH}_3\textrm{COOH}

Acid-Base Neutralization Reactions

One of the most commonly observed and studied types of acid-base reaction is the  acid-base neutralization reaction , where an acid is reacted with a base:

\begin{equation*} \textrm{acid}+\textrm{base} \to \textrm{water} + \textrm{salt} \end{equation*}

where the identity of the salt can be determined by taking the cation from the base and taking the anion from the acid.

If I react sodium hydroxide with hydrochloric acid, the cation is Na + from the sodium hydroxide and the anion is Cl – from the hydrochloric acid:

\begin{equation*} \ce{HCl}(aq) + \ce{NaOH} (aq) \to \ce{H2O}(l) + \ce{NaCl}(aq) \end{equation*}

The Titration Setup

A titration experiment is one where one attempts to determine the concentration of a sample solution by reacting two samples in such a way that the exact volume of the two reactants are known. If the concentration of one of the two reactant solutions is known exactly, then one can determine the concentration of the second solution accurately.

A buret (a long tube with a tap at the bottom) with an Erlenmeyer flask underneath.

A typical titration setup is illustrated in the figure below. A measured volume of the analyte – typically the acid – is placed in the Erlenmeyer flask at the bottom along with an indicator.  The indicator is a compound that will change color when the reaction has completed to the end point. A volumetric pipet is typically used to measure out the exact amount of analyte needed.

A buret is used to deliver the titrant (typically the base in acid-base titrations). The titrant is added in dropwise such that the volume of titrant required to change the color of the indicator can be recorded to the nearest 0.01 mL. Therefore, we can determine the exact (or as close to exact as we can) volume of titrant required to react with the analyte.

\textrm{HC}_8\textrm{H}_4\textrm{KO}_4

From the information obtained the concentration of the provided sodium hydroxide solution can be determined. Sodium hydroxide cannot be used as a primary standard readily, as it tends to be extremely hydroscopic and therefore the mass of sodium hydroxide used is not an accurate starting point for determining the concentration of base used. For this reason, we use KHP as a primary standard, with which the concentration of the sodium hydroxide solution can be determined accurately (and therefore act as a secondary standard).

The end-point – which is when the analyte is completely reacted with the titrant – is determined using phenolphthalein as an indicator. When the end-point of the titration is reached, the color of the solution changes from colorless to pink.

You will use the Determine the concentration of an unknown HCl solution and Standardization of NaOH experiment (OLI Unit 3 – Module 11)

  • You must prepare your notebook just like a regular face-to-face experiment and record all your data there in handwriting .  At the end of the experiment, you are required to scan and submit your lab notebook entries.
  • While there are directions on the OLI webpage, we have written new ones that are designed to allow you to repeat the experiment.
  • Volumes from volumetric flasks and pipettes should have four significant figures .
  • For each titration, you may want to try a rough titration first where you go through it quickly so you have a maximum volume it might be at, and then try it more carefully by starting off with adding NaOH to within a few mL before doing the titration in full.  The rough attempt should be recorded in the notebook but can be ignored for the data analysis.

Preparation of a Solution of Potassium Hydrogen Phthalate

  • Remove the KHP, a 250 mL beaker, and scale from the stockroom.
  • Place a weigh boat on the scale and tare the balance. Be sure to record the entire reading on the scale.
  • Transfer 7-9 g of KHP to the weigh boat. Note that the transfer mode is “Realistic”. Clicking once, quickly on the “Hold to Pour” button will transfer this amount. Record the mass of the KHP.  Afterwards, transfer all of this into a 250 mL volumetric flask.  (Note: the volume of a volumetric flask has four significant figures).
  • Make up the solution to 250 mL in the volumetric flask with distilled water from the stockroom.

Standardization of the Sodium Hydroxide Solution

In this part, you will determine the exact concentration of the ~0.1 M sodium hydroxide solution using the potassium hydrogen phthalate solution you prepared earlier as a standard.

  • Fill the buret approximately to the 5.00 mL mark with the NaOH solution.
  • Using a volumetric pipet, measure out 25.00 mL of the potassium hydrogen phthlate solution and put this in a 250 mL Erlenmeyer flask.
  • Put a few drops of phenolphthalein from the stockroom into the Erlenmeyer flask.
  • Overlap the buret on top of the Erlenmeyer flask so it is placed directly above the Erlenmeyer flask and is poised to deliver the solution.
  • Add portions of the sodium hydroxide from the buret into the Erlenmeyer flask.  As you near the desired concentration, be sure to add in the sodium hydroxide dropwise until the phenolphthalein indicator turns pink.
  • Record the final volume in the buret.
  • Empty the contents of the Erlenmeyer flask.

Repeat this part at least two more times.  Do a fourth trial if the volume delivered from the first three trials are more than 0.2 mL apart.

Determination of the Concentration of the Unknown Hydrochloric Acid Solution

Repeat how you did the titration of KHP against sodium hydroxide, except using 25 mL of the unknown hydrochloric acid solution instead of 25 mL of the KHP solution.

Data Analysis

This laboratory experiment is rather complex to calculate and takes some time to do. Be sure to complete all calculations carefully. If you do not understand how to do these calculations, please be sure to consult your instructor or a mentor in the Math/Science Resource Center.

Determining the Concentration of Potassium Hydrogen Phthalate (KHP) Solution

Potassium hydrogen phthalate has a molar mass of 204.2 g/mol. Given the mass of the potassium hydrogen phthalate present and the volume of the volumetric flask (which you will need to convert into liters), you should be able to determine the molarity of the solution using the definition

\begin{equation*} \textrm{molarity (M)} = \frac{\textrm{moles of solute}}{\textrm{liters of solution}} \end{equation*}

If we dissolve 3.224 g potassium hydrogen phthalate (KHP) to form a solution of 100.0 mL, the molarity of KHP in this solution is

\begin{align*} ? \mbox{ mol KHP} &= 3.224\mbox{ g KHP} \times \frac{\mbox{mol KHP}}{204.2\mbox{ g KHP}} \\ &= 0.01579\mbox{ mol} \\ ?\mbox{ L soln} &= 100.0 \textrm{ mL} \times \frac{\mbox{L}}{1000 \textrm{ mL}} \\ &= 0.1000\textrm{ L} \\ ?\frac{\mbox{mol}}{\mbox{L}} &= \frac{0.01579\textrm{ mol}}{0.1000\textrm{ L}} \\ &= 0.1579\textrm{ M} \end{align*}

Determining the concentration of the 0.1 M sodium hydroxide solution

This can be solved as a solution stoichiometry problem. To do this, the first step is to determine the number of moles of sodium hydroxide present, and then divide by the volume of NaOH used.

10.00 mL of a 0.1523 M KHP solution requires 14.22 mL of sodium hydroxide to neutralize.  Determine the concentration of the NaOH solution.

\begin{align*} ?\mbox{mol NaOH} &= 10.00 \mbox{ mL KHP} \times \frac{\mbox{L KHP}}{1000\mbox{ mL KHP}} \times \frac{0.1523 \mbox{ mol KHP}}{\mbox{L KHP}} \times \frac{1\mbox{ mol NaOH}}{1\mbox{mol KHP}} \\ &= 0.001523 \mbox{ mol NaOH} \\ ?\mbox{ L NaOH} &= 14.22\mbox{ mL} \times \frac{\mbox{L}}{1000\textrm{ mL}} \\ &=0.01422\textrm{ L}\\ \unit[?]{M} &= \frac{0.001523\textrm{ mol}}{0.01422\textrm{ L}} \\ &= 0.1071\textrm{ M} \end{align*}

Similar approaches can then be used to find the concentration of hydrochloric acid.

Determination of the Concentration of a Solution of Sodium Hydroxide Copyright © by Yu Kay Law is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License , except where otherwise noted.

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Shop Experiment Acid-Base Titration Experiments​

Acid-base titration.

Experiment #24 from Chemistry with Vernier

titration experiment of hcl and naoh

Introduction

A titration is a process used to determine the volume of a solution needed to react with a given amount of another substance. In this experiment, you will titrate hydrochloric acid solution, HCl, with a basic sodium hydroxide solution, NaOH. The concentration of the NaOH solution is given and you will determine the unknown concentration of the HCl. Hydrogen ions from the HCl react with hydroxide ions from the NaOH in a one-to-one ratio to produce water in the overall reaction:

{{\text{H}}^{\text{ + }}}{\text{(aq) + C}}{{\text{l}}^{\text{ - }}}{\text{(aq) + N}}{{\text{a}}^{\text{ + }}}{\text{(aq) + O}}{{\text{H}}^{\text{ - }}}{\text{(aq)}} \to {{\text{H}}_{\text{2}}}{\text{O(1) + N}}{{\text{a}}^{\text{ + }}}{\text{(aq) + C}}{{\text{l}}^{\text{ - }}}{\text{(aq)}}

When an HCl solution is titrated with an NaOH solution, the pH of the acidic solution is initially low. As base is added, the change in pH is quite gradual until close to the equivalence point, when equimolar amounts of acid and base have been mixed. Near the equivalence point, the pH increases very rapidly. The change in pH then becomes more gradual again, before leveling off with the addition of excess base.

In this experiment, you will use a computer to monitor pH as you titrate. The region of most rapid pH change will then be used to determine the equivalence point. The volume of NaOH titrant used at the equivalence point will be used to determine the molarity of the HCl.

In this experiment, you will

  • Use a pH Sensor to monitor changes in pH as sodium hydroxide solution is added to a hydrochloric acid solution.
  • Plot a graph of pH vs . volume of sodium hydroxide solution added.
  • Use the graph to determine the equivalence point of the titration.
  • Use the results to calculate the concentration of the hydrochloric acid solution.

Sensors and Equipment

This experiment features the following sensors and equipment. Additional equipment may be required.

titration experiment of hcl and naoh

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This experiment is #24 of Chemistry with Vernier . The experiment in the book includes student instructions as well as instructor information for set up, helpful hints, and sample graphs and data.

titration experiment of hcl and naoh

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A thermometric titration

In association with Nuffield Foundation

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Use this class practical to practise locating the end-point of a titration by measuring the temperature change

In this experiment, students titrate sodium hydroxide solution with hydrochloric acid. By measuring the temperature change each time a portion of acid is added, students can determine the end-point of the titration, indicated by the highest temperature. They then use this information to calculate the concentration of the hydrochloric acid.

The practical takes about one hour, and is best carried out individually or in pairs.

  • Eye protection (goggles)
  • Thermometer, 0–100 °C (see note 5 below)
  • Two insulated (polystyrene) cups
  • Beaker, 250 cm 3
  • Burette, 50 cm 3
  • Burette stand
  • Clamp and stand (optional)
  • Cork, one-holed, to fit thermometer (optional)
  • Pipette, 20 cm 3 or 25 cm 3
  • Pipette safety filler
  • Hydrochloric acid, 2.00 M (IRRITANT), about 75 cm 3
  • Sodium hydroxide solution, 1.50 M (CORROSIVE), about 30 cm 3

Health, safety and technical notes

  • Read our standard health and safety guidance.
  • Wear eye protection throughout.
  • Hydrochloric acid, HCl(aq), (IRRITANT at concentration used) – see CLEAPSS Hazcard  HC047a  and CLEAPSS Recipe Book RB043. This concentration is necessary to achieve a reasonable change in temperature. The concentration of the hydrochloric acid should not be indicated on bottle available to the students.
  • Sodium hydroxide solution, NaOH(aq), (CORROSIVE at concentration used) – see CLEAPSS Hazcard  HC091a  and CLEAPSS Recipe Book RB085. This concentration is necessary to achieve a reasonable change in temperature. The concentration of the sodium hydroxide should be indicated on bottle available to the students.
  • Instead of using the thermometer to stir the titration mixture, it could be clamped in position in a cork, as shown in the diagram, and the mixture swirled after each addition of acid. Alternatively, a temperature sensor attached to a computer can be used in place of a thermometer. Data logging software could then be used to provide a detailed plot of the readings.
  • Stand an insulated cup in a beaker for support.

A diagram showing the equipment required for a thermometric titration using hydrochloric acid

Source: Royal Society of Chemistry

In this thermometric titration, students can determine the end-point of the titration using the highest temperature recorded during the experiment

  • Using a pipette and safety filler, transfer 20 cm 3 (or 25 cm 3 ) of the sodium hydroxide solution into the cup, and measure the steady temperature.
  • Using the burette, add a small portion (3–5 cm 3 ) of dilute hydrochloric acid to the solution in the cup, noting down the actual volume reading. Stir by swirling the cup and measure the highest temperature reached.
  • Immediately add a second small portion of the dilute hydrochloric acid, stir, and again measure the highest temperature and note down the volume reading.
  • Continue in this way until there are enough readings to decide the maximum temperature reached during this experiment. You will need to add at least 30 cm 3 of the acid.
  • Plot a graph of temperature against the volume of acid added, and use extrapolation of the two sections of the graph to deduce the maximum temperature reached without heat loss.
  • Use your results to calculate the concentration of the hydrochloric acid.

Teaching notes

The main concern in this experiment is the heat loss. If possible, a lid should be used. More reliable results can be achieved using two polystyrene cups (one inside the other).

With abler or older students, it is possible to discuss the extrapolation of the cooling curve to estimate the maximum temperature reached without heat loss. Creative Chemistry provide a resource on thermometric titration which includes an example of a typical plot of temperature vs volume of acid for this experiment, as well as the use of extrapolation to determine the maximum temperature change.

To reinforce the theory involved here, an indicator could also be used to show that the end-point really did occur at the highest temperature.

Additional information

This is a resource from the  Practical Chemistry project , developed by the Nuffield Foundation and the Royal Society of Chemistry. This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. Practical Chemistry activities accompany  Practical Physics  and  Practical Biology .

The experiment is also part of the Royal Society of Chemistry’s Continuing Professional Development course:  Chemistry for non-specialists .

© Nuffield Foundation and the Royal Society of Chemistry

  • 14-16 years
  • 16-18 years
  • Practical experiments
  • Acids and bases
  • Quantitative chemistry and stoichiometry
  • Reactions and synthesis

Specification

  • (e) simple procedures to determine enthalpy changes
  • determine the enthalpy changes for combustion and neutralisation using simple apparatus; and
  • 2.8.6 recall experimental methods to determine enthalpy changes;
  • 1.8.11 investigate the temperature change during neutralisation and demonstrate understanding that neutralisation reactions are exothermic (heat is given out);
  • 1.8.10 investigate the temperature change during neutralisation and demonstrate understanding that neutralisation reactions are exothermic (heat is given out);

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  • w ogóle na komórkach przy wąskim wyświetlaczu to z reklamami kiepsko wygląda
  • Basic terms
  • Titration end point
  • End point indicators
  • End point detection
  • Equivalence point calculation
  • Titration curve calculation
  • Titration calculation
  • Back titration
  • Sample & titrant volume
  • Volumetric glassware
  • Volumetric glass cleaning
  • Glassware calibration
  • Standard substances
  • Sources of errors
  • End point (pH) indicators
  • Indicators preparation
  • Polyprotics and mixtures
  • Solutions used
  • Solutions standardization
  • HCl determination
  • H 2 SO 4 determination
  • Acetic acid in vinegar
  • H 3 PO 4 determination
  • NaOH determination
  • NaOH & Na 2 CO 3 assay
  • Potentiometric titrations
  • Permanganate titration
  • Precipitation
  • Argentometry
  • Solution standardization
  • Chlorides - Mohr method
  • Chlorides - Volhard method
  • Complexometric
  • EDTA titration overview
  • EDTA standardization
  • magnesium titration
  • calcium titration
  • zinc titration
  • nickel titration
  • aluminum titration
  • total water hardness
  • Further reading
  • » Acid-base titration
  • » Sodium hydroxide titration

Titration of sodium hydroxide with hydrochloric acid

General remarks.

Determination of sodium hydroxide concentration is about as often discussed as hydrochloric acid titration - both acid and base are strong, so calculation of titration curve and equivalence point are pretty straightforward. However, titration itself is not as easy. Sodium hydroxide easily adsorbs carbon dioxide from the atmosphere, and presence of carbonic acid interferes with the end point detection. Titration - as described - allows determination of initial amount of sodium hydroxide, that is ignore carbon dioxide presence.

This is a simple neutralization reaction:

HCl + NaOH → NaCl + H 2 O

H + + OH - → H 2 O

See hydrochloric acid determination for more details.

sample size

Depending on the titrant concentration (0.2 M or 0.1 M), and assuming 50 mL burette, aliquot taken for titration should contain about 0.28-0.36 g (0.14-0.18 g) of sodium hydroxide (7-9 or 3.5-4.5 millimoles).

end point detection

Equivalence point of strong acid titration is usually listed as exactly 7.00. That's not necesarilly the case, as it depends on the solution temperature and ionic strength of the solution, besides, slight hydrolysis of NaOH shifts pH down by about 0.02 unit. Not that it changes much - we are still very close to 7. However, as we have discussed on the acid-base titration end point detection page, unless we are dealing with a diluted solution (in the range of 0.001 M) we can use almost any indicator that gives observable color change in the pH 4-10 range. Lab practice shows that the most suitable and easy to use indicator in this case is methyl orange .

If sodium hydroxide is contaminated with sodium carbonate - which is not rare - added titrant reacts first with hydroxide and later protonates weaker bases - carbonate:

CO 3 2- + H + -> HCO 3 -

and then hydrogen carbonate:

HCO 3 - + H + -> H 2 CO 3

Presence of carbonic acid shifts pH of the solution down, which may effect in premature end point detection. To avoid this problem, we should titrate the solution to the end point (first sign of red tint), then heat the solution to boil to remove CO 2 . If at this stage color of the solution changes back to yellow, we should cool it and titrate again. Depending on the amount of carbonates present we may have to repeat the procedure more than once.

solutions used

To perform titration we will need titrant - 0.2 M or 0.1 M hydrochloric acid solution , indicator - methyl orange and some amount of distilled water to dilute sodium hydroxide sample.

  • Pipette aliquot of sodium hydroxide solution into 250mL Erlenmeyer flask.
  • Add about 70 mL of distilled water.
  • Add 1-2 drops of methyl orange solution.
  • Titrate with hydrochloric acid solution till the first color change.
  • Heat the solution to boil to remove dissolved carbon dioxide. Solution may change color back to yellow.
  • Titrate with HCl solution till the first color change. Repeat titration and boiling till yellow color doesn't return after cooling the solution.

result calculation

According to the reaction equation

Hydrochloric acid reacts with sodium hydroxide on the 1:1 basis. That makes calculation especially easy - when we calculate number of moles of HCl used it will be already number of moles of NaOH titrated.

To calculate sodium hydroxide solution concentration use EBAS - stoichiometry calculator . Download determination of sodium hydroxide concentration reaction file, open it with the free trial version of the stoichiometry calculator .

Click n=CV button above HCl in the input frame, enter volume and concentration of the titrant used. Click Use button. Read number of moles and mass of sodium hydroxide in the titrated sample in the output frame. Click n=CV button in the output frame below sodium hydroxide, enter volume of the pipetted sample, read sodium hydroxide concentration.

Note that presence of carbonates - while interferes with the end point detection - doesn't interfere with the determination of initial amount of sodium hydroxide. However, if we want to determine amount of sodium hydroxide that was not yet neutralized by carbon dioxide, we should titrate the solution against two indicators, this is so called Warder's method which we will discuss separately.

sources of errors

Carbon dioxide interferes with the determination (end point detection) as described above. During heating, if the solution is allowed to boil too vigorously, it may splash and some sodium hydroxide can be lost. Titration - as described - doesn't allow to determine amount of sodium hydroxide that was not yet reacted with carbon dixode. Otherwise - just the general sources of titration errors

Need more info?

Principles of Analytical Chemistry: A Textbook

by Miguel Valcarcel

(commissions earned)

Complete list of suggested books

last modified on October 27 2022, 21:28:27.

Dean's Analytical Chemistry Handbook - tam sa fajne (chyba) listy co czym oznaczac, warto obejrzec

Technical info: $section - alkalimetry, $subsection - , $page - NaOH, $url_call - acid-base-titration-sodium-hydroxide

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titration experiment of hcl and naoh

The technique known as titration is an analytical method commonly used in chemistry laboratories for determining the quantity or concentration of a substance in a solution. In a titration, an analyte -- the substance whose quantity or concentration is to be determined -- is reacted with a carefully controlled volume of solution of accurately-known concentration called a standard solution . The standard solution (also known as the titrant ) is usually added to the solution containing the analyte by means of a buret , a piece of volumetric glassware capable of accurately measuring solution volumes.

There are many types of titrations in common use in the analytical chemistry laboratory. Each type uses a different kind of chemical reaction. Examples of titration types include

  • acid-base titration ,
  • reduction-oxidation titrations,
  • precipitation titrations, and
  • complexometric titrations.

The most commonly studied type is the acid-base titration. For this project we focus our attention exclusively on this type, and we develop a mathematical model that describes the relationship between the volume of added titrant (a base) and changes in concentration of the analyte (an acid). The model presented would need only slight modifications to be applicable to other titration types listed above.

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IMAGES

  1. Titration Of Hcl With Naoh

    titration experiment of hcl and naoh

  2. Acids and Bases I

    titration experiment of hcl and naoh

  3. Titration of HCl with NaOH

    titration experiment of hcl and naoh

  4. Chemical Science: Classic Chemistry Experiments : Titration of sodium

    titration experiment of hcl and naoh

  5. Titration Of Hcl With Naoh

    titration experiment of hcl and naoh

  6. Titration of NaOH and HCl

    titration experiment of hcl and naoh

COMMENTS

  1. Titrating sodium hydroxide with hydrochloric acid

    Stage 1. Using a small funnel, pour a few cubic centimetres of 0.4 M hydrochloric acid into the burette, with the tap open and a beaker under the open tap. Once the tip of the burette is full of solution, close the tap and add more solution up to the zero mark. (Do not reuse the acid in the beaker - this should be rinsed down the sink.)

  2. Titration of hydrochloric acid with sodium hydroxide

    Titrate with NaOH solution till the first color change. result calculation. According to the reaction equation. HCl + NaOH → NaCl + H 2 O. Hydrochloric acid reacts with sodium hydroxide on the 1:1 basis. That makes calculation especially easy - when we calculate number of moles of NaOH used it will be already number of moles of HCl titrated.

  3. PDF Chemistry 120: Experiment 1 Preparation of a Standard Sodium Hydroxide

    Add about 6 mL (use a 10-mL graduated cylinder) of the 50% sodium hydroxide solution to a 1-liter bottle. Fill the bottle to its shoulder with the distilled water. Place the stopper or the lid on the bottle, and thoroughly mix the solution by shaking the bottle. Warning: Concentrated NaOH is very corrosive!

  4. Titration of HCl with NaOH

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  5. PDF Acid/Base Chemistry: Titration Lab

    A titration is an analytical procedure used to determine the accurate concentration of a sample by reacting it with a standard solution. One type of titration uses a neutralization reaction, in which an acid and a base react to produce a salt and water: In equation 1, the acid is HCl (hydrochloric acid) and the base is NaOH (sodium hydroxide).

  6. Determination of the Concentration of a Solution of Sodium Hydroxide

    When the end-point of the titration is reached, the color of the solution changes from colorless to pink. Procedures. You will use the Determine the concentration of an unknown HCl solution and Standardization of NaOH experiment (OLI Unit 3 - Module 11)

  7. Titration: Practical and Calculation (NaOH and HCl)

    Must see: My new website at http://ww.acechemistry.co.uk. This video, with the help of flash animations, shows and explains how you can determine the concent...

  8. Acid-Base Titration > Experiment 24 from Chemistry with Vernier

    A titration is a process used to determine the volume of a solution needed to react with a given amount of another substance. In this experiment, you will titrate hydrochloric acid solution, HCl, with a basic sodium hydroxide solution, NaOH. The concentration of the NaOH solution is given and you will determine the unknown concentration of the HCl. Hydrogen ions from the HCl react with ...

  9. A thermometric titration

    In this thermometric titration, students can determine the end-point of the titration using the highest temperature recorded during the experiment. Using a pipette and safety filler, transfer 20 cm 3 (or 25 cm 3) of the sodium hydroxide solution into the cup, and measure the steady temperature. Using the burette, add a small portion (3-5 cm 3 ...

  10. PDF Chemistry 130 Experiment 6: Titration and Analysis

    Experiment 6: Titration and Analysis Introduction ... The most common type of neut ralization occurs between a strong acid [like HCl] and a strong base [like NaOH] to yield a "salt" and water. HCl(aq) + NaOH(aq)-----> NaCl(aq) + H2O(l) The total acid (or base) concentration of a solution can be obtained by carrying out a procedure called ...

  11. PDF Experiment 6 Titration II

    Figure 1 is a titration curve for the titration of HCl by NaOH, a strong acid and strong base, where 25.0 mL of 0.1 M HCl is titrated with 0.1 M NaOH. NaOH titration of HCl 0 2 4 6 8 10 12 14 0 102030 mL NaOH added p H 40 Phenolphthalein Equivalence Point Methyl Red Figure 1. Titration of 25.0 mL of 0.1M HCl by 0.1 M NaOH. Blocked areas on the ...

  12. NaOH vs HCl Titration using Phenolphthalein

    In this video, I have demonstrated the whole experiment related to NaOH vs HCl titration. Also included precautions, practical copy record and important poin...

  13. Titration of sodium hydroxide with hydrochloric acid

    Sodium hydroxide easily adsorbs carbon dioxide from the atmosphere, and presence of carbonic acid interferes with the end point detection. Titration - as described - allows determination of initial amount of sodium hydroxide, that is ignore carbon dioxide presence. reaction. This is a simple neutralization reaction: HCl + NaOH → NaCl + H 2 O. or

  14. PDF Lab Report #4 Titration of Hydrochloric acid with Sodium Hydroxide

    Lab Report #4. um HydroxideSCH3U. 02Thursday, December 19, 2013Introd. tion The following lab was an acid-base neutralizing titration. A titration is a technique, in which a reagent, called a titrant, of known concentration is use. to determine the concentration of an analyte or unknown solution. Using a.

  15. Performing Titrations

    HCl + NaOH NaCl + H 2 O During the course of the titration, the titrant (NaOH) is added slowly to the unknown solution. As it is added, the HCl is slowly reacted away. The point at which exactly enough titrant (NaOH) has been added to react with all of the analyte (HCl) is called the equivalence point.

  16. Titration Lab Report

    About the lab tiration titration lab report aim to find the concentration of sodium hydroxide titrating hydrochloric acid with sodium hydroxide. introduction. ... HCl+NaOH → H2O+NaCl. Predictions. When this experiment is carried out the base in the conical flask should turn colorless after adding acid to the solution. The base solution should ...

  17. PDF Submit to Lab Report Titration of Hydrochloric Acid with Sodium

    hydrochloric acid (HCl) with sodium hydroxide (NaOH). The purposes of the experiment are to find the amount of NaOH that will affect the color of the solution once it reaches the end point, to find the unknown concentration of HCl solution, and also to apply knowledge of using glassware especially the buret and pipette. Before doing this ...

  18. Titration Project, Part 1

    The chemical equation allows us to calculate the concentration of a solution of HCl by titration with the base NaOH (where the concentration of NaOH is accurately known). Let's suppose that our solution is 0.02500 L of an unknown concentration of the acid, HCl. We wish to find its concentration by titration with 0.1000 M NaOH.

  19. Determining solute concentration by acid-base titration (worked example

    First, calculate the number of moles of strong base required to reach the equivalence point of the titration. Then, using the mole ratio from the balanced neutralization equation, convert from moles of strong base to moles of acid. Finally, divide the number of moles of acid by the given volume of the acid solution to find the concentration.

  20. Understanding Acid-Base Titration: pH, pKa, and Titrant

    If a strong acid such as HCl was titrated with NaOH, the solution would be neutral at the equivalence point as the product, NaCl, ... which you will have in your experiment: 1) the Figure 1. Titration curve of an aqueous acetic acid solution with 0.1 M NaOH. volume of the acid solution and 2) the concentration in g acid/L solution. ...

  21. Titration NaOH vs HCl

    Titration involving Sodium Hydroxide and Hydrochloric Acid

  22. Solved Question 34 (3 points) During a classroom titration

    During a classroom titration experiment, Amina tries to verify the concentration of sulfuric acid (H 2 SO 4). In each trial, she titrates 2 5 ml of the sulfuric acid with 0. 0 5 0 0 mol / L sodium hydroxide (NaOH). For the volume of NaOH, the data from three trials are 3 1. 4 mL, 3 1 mL, 3 1. 2 mL, respectively. Find the ...