Add 5 mL of copper (II) sulphate solution to a test tube. Add 5 mL of sodium carbonate in another test tube. Record the appearance. 2. Write a hypothesis on what you think will happen when mixed.
This solution was placed in a burette and 18.4 cm3 was required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Deduce the molecular formula of the acid and hence the value of n. 5. Sodium carbonate exists in hydrated form, Na2CO3.xH2O, in the solid state. 3.5 g of a sodium carbonate sample was dissolved in water and the volume made up to 250 cm3. 25.0 cm3 of this solution was titrated against 0.1 moldm-3 HCl and 24.5 cm3 of the acid were required.
In the first part, five 100 mL flasks of 5 mL ligand solution, 5 mL 2 M sodium acetate, 4 mL 3 M NH2OH, and 1-5 mL Fe2+ solution are diluted with water. The absorption spectrum for varying concentrations of Fe2+ are measured using a spectrophotometer and the data is graphed in Excel. The slope of the line is ε in the Beer-Lambart equation A = εcl. In the second part of the experiment, eleven flasks containing diluted stock solutions of Fe2+ and ligand are mixed with 5 mL 2 M sodium acetate and 4 mL 3 M NH2OH and diluted with water. The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel.
This reaction can be summed up using the following formula: 5Fe2++8H++MnO4- →5Fe3++Mn2++4H2O After standardization, the potassium permanganate solution is then titrated with 3 different magnesium oxalate solutions. To find the concentration of the C2O42- the balanced net ionic redox reaction formula is used: 5C2O42-+16H++2MnO4- →10CO2+2Mn2++8H2O It is important to note the addition of sulfuric acid (9M H2SO4) in performing this experiment because of the following reasons: 1) Sulfuric acid keeps the iron (II) from air oxidizing into iron (III) 2) Sulfuric acid keeps the iron (II) from hydrolyzing into Fe(OH)2 3) Sulfuric
Computer Additivity of Heats of Reaction: Hess’s Law 18 (1) Solid sodium hydroxide dissolves in water to form an aqueous solution of ions. (2) Solid sodium hydroxide reacts with aqueous hydrochloric acid to form water and an aqueous solution of sodium chloride. NaOH(s) + H+(aq) ) + Cl–(aq) → H2O(l) + Na+(aq) + Cl–(aq) ∆H2 = ? OBJECTIVES • • • • In this experiment, you will Combine equations for two reactions to obtain the equation for a third reaction. Use a calorimeter to measure the temperature change in each of three reactions.
Separation of the components of Extra-Strength Excedrin I: Acid-Base extraction Introduction The purpose of this experiment is to analyze the purity of Extra-Strength Excedrin® by utilizing thin-layer chromatography and determine the percent recoveries of its components. Three active ingredients will be extracted and collected from two tablets of Extra-Strength Excedrin® by utilizing acid-base extraction method. Three active ingredients of Extra-Strength Excedrin® are acetylsalicylic acid(aspirin), acetaminophen and caffeine, and their structures are: In addition, there is a binding material, which binds other three components together. These compounds can be separated by acid-base extraction because of their different acidities. A binding material can be separated by dissolving the tablet in ether since three active ingredients are soluble.
The following data were obtained when a sample of barium chloride hydrate was analyzed as described in the Procedure section. Calculate (a) the mass of the hydrate, (b) the mass of water lost during heating, and (c) the percent water in the hydrate. Mass of empty test tube 18.42 g Mass of test tube and hydrate (before heating) 20.75 g Mass of test tube and anhydrous salt (after heating) 20.41 g. Mass of the Hydrate is 2.33g. Loss (H2O) is 0.34g. Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3.
ABSTRACT In the “Density, Accuracy, Precision and Graphing” experiment, the purpose was to determine the density of water and the concentration of a saline solution as well as to compare the accuracy and precision of a graduated cylinder and a graduated pipet. Based on the instructions of the lab manual, Fundamentals of Chemistry, the experiment was performed in three parts, Part A: Density of Water-The density of water was calculated by measuring the mass of three different volumes: 10mL, 30mL and 50mL. Part B: Accuracy and Precision was performed using a 100mL beaker, 10mL graduated pipet and deionized water. The experiment was performed three times; each time, 10mL of water was added to the beaker and recalculated. Part C: Density of Sodium Chloride (NaCl) Solution, a sample of NaCl was obtained and measured using a 100mL beaker and a 10mL pipet to determine the concentration of the solution.
Introduction In this experiment copper chloride and iron chloride are separately reacted with sodium hydroxide to determine what their charge is. The copper chloride can be either copper (I) or copper (II) chloride. The iron chloride can either be iron (II) or iron (III) chloride. By completing a double replacement reaction with the sodium hydroxide the formulas of the iron and copper chlorides can be found. Objective The objective of this lab is to find the formula of an ionic compound.
In this lab we synthesized and analyzed potassium aluminum sulfate (KAl(SO4)12H2O) using a multiple different tests. These test included flame test, melting point, potassium test, sulfate test, and aluminum test. We also determined the number of waters of hydration in Alum. Experimentally and empirically potassium aluminum sulfate is a dodecahydrate (4). The purpose of the laboratory is to determine the number of waters of hydration in aluminum potassium sulfate as well as the purity of the Alum we produce.