To perform this experiment, we will utilize emission spectra, titrations, and thermal gravimetric analysis, using knowledge from Experiments 10, 4, Titrations of Na2CO3 and NAHCO3 by HCl (hydrochloric acid) will be performed to determine the concentration of HCl, as well as the number of moles of HCl present within the sample of baking soda. As a result, we will be able to determine the molar concentration of HCl by determining its equivalence point (the point on the graph where the exact amount of rectant needed to perform a reaction has been added) from graphical analysis. Na2CO3(aq.) + HCl(aq.) ==> NaHCO3(aq.)
Calculate the concentration of grams of sodium stearate per milliliter of diluted solution. To do this, multiply the concentration of sodium stearate in the dishwashing liquid by the dilution of the solution (1.50 mL dishwashing liquid per 100 mL solution). Answer = 1.5 *10^-4 g/mL 4. Calculate the number of moles of sodium stearate in a single layer. To do this, first take the number of drops used to achieve the monolayer (1 drop) and convert it to mL using the calibrated number of drops per mL.
Repeat the titration until there are two titres within 0.1cm3 of each other. Record results in a suitable table. Results: Rough Titre: 7.653 First Run: 6.553 Second Run: 6.453 Third Run: 6.553 Calculations: During the titration, iron(II) ions are oxidised to iron(III) ions and manganate(VII) ions are reduced to manganese(II) ions. The equation is as follows: 5Fe2+(aq) + MnO4-(aq) + 8H+(aq) ? 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) The above equation shows that one mole of manganate(VII) ions reacts with 5 moles of iron(II) ions in acid solution.
Materials: • 2 Graduated Cylinders • Distilled Water • Stirring Rod • Balance • One 250ml Beaker • One Erlenmeyer Flask • Filter Paper • Copper (II) Sulphate Pentahydrate • Strontium Chloride Hexahydrate Procedure 1. Two graduated cylinders are used and 75ml of distilled water are added to both 2. The two reactants are made into a solution by
Calculate the exact normality of Na2S2O3 knowing that in this chemical reaction 1 gram-equivalent of K2Cr2O7 react with 1 gram-equivalent of Na2S2O3 (1 mole K2Cr2O7 react with 6 moles Na2S2O3). Determination of peroxide value. Weigh 3.00 g oil (with precision of 0.001 g) into a 250 ml Erlenmeyer flask. Add 10 ml chloroform and swirl to dissolve oil. Add 15 ml acetic acid,
This reaction is carried out by adding a solution of reactant hydrochloric acid from a burette to a solution of sodium hydroxide until just sufficient of hydrochloric acid has been added to react with all of the sodium hydroxide. If the concentration and volume of hydrochloric acid is known the number of moles of sodium hydroxide can be calculated, if the equation for the reaction is known. This procedure is known as a titration and the point at which sufficient volume of hydrochloric acid has been added to the sodium hydroxide to complete the reaction is called the end point. An indicator which changes colour at the equivalence point is often used to indicate the titration end point. This standardized solution of sodium hydroxide can then be used to determine the concentration of acid in the sample of gastric juice.
Titration Aim Part A: To prepare a primary standard and use it to determine the concentration of a sodium hydroxide solution. Part B: To monitor the neutralisation of dilute vinegar by a standardised sodium hydroxide solution to determine the concentration of acetic acid in dilute vinegar. Equipment • 250mL volumetric flask • Oxalic acid dehydrate crystals • Beaker (150mL) • Small funnel • Phenolphthalein • Burette • Wash bottle with distilled water • Electronic balance • Pipette (25mL) • 2 x Beaker 50mL • Burette clamp and stand • Pipette filler • Spatula • Glass rod • pH meter and data logger • Standardised NaOH solution • Diluted vinegar (150mL diluted into 1L with distilled water) • Sample of 0.1mol/L sodium hydroxide solution • Magnetic stirrer with stirrer • 100mL measuring cylinder Method Part A: Preparation of Standard Solution 1. The molar weight (M) of oxalic acid dehydrate was calculated. 2.
The Ka expression, Ka=H+In-HIn [1] (1) is the equilibrium for the dissociation of the weak acid, where HIn is the acid and In- is the conjugate base. This is represented by the chemical equation: HIn ⇌H++ In- [1]Figure 1: Chemical equation for the dissociation of an acid-base indicator. Methyl red is a monoprotic organic acid. Figure 2 is a structural model of methyl red. Figure 2: Chemical structure of methyl red By plotting the data as the pH versus the log term of the Henderson-Hasselbach Equation, pH=pKa+logIn-HIn [2] (2) the pKa was
(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.
In each trial, the initial reading, final reading and the volume of HCl used was recorded down as quantitative results. The average volume of hydrochloric acid was found to be 12.03mL. The amount of sodium carbonate in the 10.00ml of solution was found to b 0.05 mol. The amount of hydrogen chloride that was dissolved in the average volume of acid is 0.365g. Through these calculations, the concentration of hydrochloric acid was found to be 8.3 mol•L-1.