Aim: The aim of this experiment is to monitor the pH change using a pH meter and data logger as HCl is titrated with NaOH and to then determine the molarity of the HCl solution.
Introduction
A titration is an analytical method in which the unknown concentration of a solution, analyte, is calculated by determining the volume of a solution with known concentration needed, titrant, to completely react with the analyte. In this case the hydrochloric acid solution (HCl) is the analyte since its concentration is unknown and it is titrated with sodium hydroxide (NaOH) which serves as a titrant since its concentration is known. This is as an acid-base titration and in it the hydrogen ions from the HCl react with hydroxide ions from the NaOH to produce
…show more content…
As the base, NaOH, is added drop by drop the pH gradually increases until the equivalence point. This is when the amount of hydroxide ions (from base) added equals to the amount of hydrogen ions (from acid) present in the solution. At this point the pH increases very rapidly until it reaches a more gradual rate of increase.
The pH change can be followed using a pH meter and measuring the pH after each drop of base added. Then, plotting a pH versus volume of base graph the volume at equivalence point can be determined. The curve of a strong acid-base titration is shown in Figure 1.0.
Figure 1.0 – The titration curve obtained when plotting the pH versus volume of base added during a strong acid-base titration. Objectives: Use a pH Sensor to monitor changes in pH during a titration of HCl with
…show more content…
The burette is attached to a laboratory stand with 2 clamps. The burette is first rinsed with 0.1M NaOH and then it is filled with it a bit above the 0.00 mL mark. NaOH is drained from the burette so that there are not bubbles in the tip and so that the NaOH reaches exactly the 0.00 mL level. Dispose of the waste NaOH solution that was drained. 50 mL of distilled water is added to the 250 mL beaker and 10 mL of HCl is pipetted into the beaker. The beaker is placed on the magnetic stirrer and a stirring bar is placed inside the solution. The beaker and the magnetic stirrer are placed under the burette. The support ring is attached to the laboratory stand and a pH Sensor is positioned on it so that it is immersed in the HCl solution. Make sure the stirrer will not hit the pH probe. Turn on the magnetic stirrer and adjust it to medium stirring (no splashing). Connect the pH Sensor to the Vernier computer
A hot plate was placed under the ring stand. 50 mL of 3.0 M NaOH in a 250 mL beaker and a stir bar was placed in the beaker. The beaker with NaOH was placed on the hot plate and 3.75 grams of NaAlO2*5H2O was placed in the beaker. The temperature probe was placed in the beaker with the solution, not touching the bottom of the beaker. The solution was heated and stirred till the solution dissolved.
Marwah Alabbad Post lab 10/21/15 Question 1: 1. Experiment 1: Number of trails NaOH concentration (M) Volume of HCl solution (mL) Initial volume of NaOH(mL) final volume of NaOH(mL) The volume of NaOH to titrate HCl (mL) Concentration of HCl (M) 1st 0.1023 25.0 10.05 36.12 26.07 0.085 2nd 0.1023 25.0 5.74 31.40 25.66 0.105 3rd 0.1023 25.0 9.84 35.52 25.68 0.105 First trail calculation: 0.02607L× (0.1023mole NaOH/1L)×(1 mol of HCL/1 mol of NaOH)×(1/0.025)= 0.085M of HCl
8. Place a clean funnel into the mouth of a 250ml volumetric flask. 9. Carefully pour the oxalic acid crystals into the funnel. 10.
= 10^-3 M = 1,000 mL Here C1,C2; are the first and second concentrations of solution V1 and V2 ; are the required and current volumes. The impeller turned on and DDA, and tap water left to be mixed properly with water for 2 minutes. Approximately 150 grams of quartz added into the solution.
3. Upon adding 20 drops of NaOH, a white precipitate was formed signifying acidic impurity. In the second NaOH mixture, about 20 drops were administered and no precipitate formed indicating that the ample is more pure than before. Data: Weight of flask = 75.10 grams Weight of the flask with solids =
Standard Sodium hydroxide solution is the alkaline solution that will be used to titrate with soda water as it is a common solution that can be easily found in an ordinary school laboratory. It is a strong base. Carbonic acid is a weak acid which will react with a strong base to form a basic (pH > 7) solution. When Phenolphthalein is added to Soda water, the resultant solution is colourless. After titration with a strong base (sodium hydroxide), the solution will turn to pink as the solution becomes
Titration is the basis of the Titration Lab because the goal of the lab was to titrate. Titration is determining the concentration of a solution by neutralizing it with another known concentration. We titrated the NaOH in the HCl. The titration caused a
The equation of the reaction between sodium hydroxide and ethanoic acid is as follows: CH3COOH + NaOH → CH3COONa + H2O We can measure the end point of titration process and we can also measure the amount of reactants. The concentration of ethanoic acid in the vinegar can be determined through stoichiometric calculations, Using the values obtained from the titration, and also the chemical equation as a reference. Phenolphthalein indicator is used in this acid-base titration Equipment and materials:
Its pH is greater than 7 and turns red litmus paper into blue. Acid- base neutralization is done by adding an acid to a base or a base to an acid until the substance has equal hydrogen and hydroxide ions. This is used to determine unknown concentration of a
Practical I: Acid-base equilibrium & pH of solutions Aims/Objectives: 1. To determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3.
Introduction Buffer is a solution that resists a change in pH when bases or acid are added. Solutions that are acidic contain high concentrations of hydrogen ions (H+) and have pH values less than seven. Buffer usually consist of a weak acid, and its conjugate base or a weak base and its conjugate acid. The function of buffer is to resist the changes in hydrogen ion concentration as a result of internal and environmental factor. This buffer experiment is important so that we relies the important of buffer in our life.
Buffer solutions of pH 4 and 7 6. Graduated cylinder - 100 mL 7. Volumetric flask with stopper - 250 mL 8. Two 100-mL beakers 9. Two 50-mL Burettes 10.
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.
That caused a new initial reading of NaOH on the burette (see Table1 & 2). The drops were caused because the burette was not tightened enough at the bottom to avoid it from being hard to release the basic solution for titrating the acid. The volume of the acid used for each titration was 25ml. The volume of the solution was then calculated by subtracting the initial volume from the final volume. We then calculated the average volume at each temperature.
Abstract — This experiment was conducted to familiarize the students with the procedures regarding distillation—to be more precise, the separation of ethanol from an alcoholic beverage—using a distillation set-up consisting of boiling chips, a Bunsen burner, a condenser, a thermometer and several other materials. In the end, it was discovered that one may actually separate a homogeneous mixture, given that the components of said mixture differ in volatility and that they utilize a complete distillation set-up and follow laboratory safety rules and regulations. Keywords — Matter, homogeneous and hetereogeneous mixtures, distillation, volatility, boiling point I. INTRODUCTION There are typically two categories of matter, these are pure substances