The synthesis of NaCl further identified the ionic compound by reacting sodium hydroxide and hydrochloric acid and obtaining solid sodium chloride. The synthesized compound formed was used to perform another flame test and the chloride anion test, which further solidified the identification of NaCl as the ionic compound. Introduction The purpose of the experiment was to identify unknown ionic compound
The goal of this lab was to discover the unknown group 1 metal (M) of the compound M2CO3 by dissolving the compound in water and adding a solution of calcium chloride, CaCl2 to the solution in order to precipitate the carbonate ions to reveal the molar mass of the unknown element, thus determining the identity of the unknown element. The initial hypothesis was that the metal carbonate would be potassium carbonate, or K2CO3, because potassium is a group 1 element that is very similar to calcium, but there are many other group 1 elements that
AP Chemistry P2 Experiment 2: Formula of a Hydrate 9/24/2013 Purpose: Calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate. Procedure: 1) Set up ring stand with ring clamp, clay triangle, crucible with lid, and burner. Adjust the height of the ring stand. 2) Dehydrating Procedures: 3. Measure approximately 1 g of Copper(II) Sulfate Hydrate into the crucible and crucible and lid.
Indirect Gravimetric Determination of a Hydrated Compound in a Mixture Morgan Dufer I. The purpose of this lab was to find the percent of BaCl2*2H2O in a sample of unknown composition by using gravimetric analysis. II. Pre-lab Questions 1. What mass of MgCO3 is contained in a 2.750g solid sample consisting of only MgCO3 and MgO if heating to decompose all the MgCO3 according to the following equation leaves a solid residue weighing 2.160g?
Now that we have filtered the precipitate, we will then place the resulting precipitate into a test tube to measure the weight. By using the information above in our experiment, we were then able to determine that one of these ionic compounds are not soluble in Water and in turn, produced a resulting precipitate which is the evidence that a reaction has occurred. We then identified the anion and cation for these ionic compounds. The Potassium Chromate-
Synthesis of Colloidal Ag Colloidal silver is made by adding an excess of the reducing agent sodium borohydride, NaBH4 to silver nitrate, AgNO3 . AgNO3 + NaBH4 → Ag + 1/2H2 + 1/2B2H6 + NaNO3 The method used in the procedure for this experiment produces nanoparticles that are about 10-14 nm in diameter. The transmission electron microscope (TEM) image shown corresponds to a sample of silver nanoparticles with diameters that are 12± 2 nm. (The length bar is 20 nm.) Particle size can also be determined using visible spectroscopy.
TITRATION OF AN ACID (A PREPARED STANDARD SOLUTION OF KH₅O₄C₈) AGAINST A BASE (NAOH) USING PHENOLPHTHALEIN AS AN INDICATOR BY GRACE The aim of this experiment is to prepare a standard solution of potassium hydrogen phthalate (KH₅O₄C₈) and then use it to calculate the concentration of sodium hydroxide by titrating the acid (KH₅O₄C₈) against the base (NaOH). Before the whole experiment could take place, some apparatus were needed which included the following; A weighing balance, burette, pipette, a conical flask, clamp and then the setup was as below; THEORY To calculate for the moles of KH₅O₄C₈, I used n (mol) =m (g)/M (gmol⁻ⁱ (JOHN GREEN AND SADRU DAMJI, PG 6 OF CHAPTER 1.THIRD EDITION). Whereby m=mass of the acid, M=molar mass of the acid and n=number of moles. Molar mass of KH₅O₄C₈ is 204.1g/mol and its mass is 1g Therefore=1g/204.1gmol⁻ⁱ n=0.0048996mol Further more, to calculate for the concentration of the acid, I used C(moldm⁻3.) =n (mol)/v (dm3) Whereby c=concentration, n=number of moles and v=volume used.
The Empirical Formula of an Oxide, Purpose: The purpose of this lab was to determine the empirical formula of magnesium oxide. To do this, we measured the weight of the magnesium before the reaction with oxygen, and then measure it after it had bonded with the oxygen. After the mass of the items were collected, the data was calculated in empirical formula. Background: The empirical formula of a compound is the whole number ratio of the elements in a compound. For example, the empirical formula of water is H2O meaning for every 1 O atom there are 2 H atoms.
Introduction A titration was carried out in this experiment to find the concentration of hydrochloric acid is an unknown solution. The aim of this experiment is to determine the number of moles of sodium hydroxide in hydrochloric acid and then to determine the number of moles of sodium hydroxide present in gastric juices. Titration, or volumetric analysis, is a common laboratory procedure for the analysis of substances and solutions. In a titration, the analyst determines the volume of a solution, called a titrant, that reacts exactly with a known weight or volume of another substance. 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.
Experiment 15: Molar Mass Determination by Freezing Point Depression Introduction The purpose of this experiment is to determine the molar mass of camphor by determining the freezing point depression of cyclohexane. In this experiment a sample of the solvent cyclohexane was cooled to its freezing point and a cooling curve was constructed. A known mass of camphor was added to the known mass of camphor and the freezing point of the solution was determined using equations 1 and 2. From the freezing point depression the molality of the camphor can be calculated and then the molar mass, by using equation 3. If Tf(solvent) is defined as the freezing point of the pure solvent, and if Tf(solution) is defined as the freezing point of the solution, then the freezing point depression (in °C) is given by equation 1: ΔTf = Tf(solvent) - Tf(solution) (1) The freezing point depression ΔTf is related to m, the molality of the solution particles, given in equation 2: ΔTf = Kf m (2) If a known mass of a solute is placed into a known mass of solvent, and the freezing point depression relative to the pure solvent determined, then the molar mass (MM) of the solute can be determined by using the appropriate Kf value for the solvent, equation 3: ΔTf = Kf (mol/kg solvent) = Kf (g solute/MM solute) / kg solvent (3) Procedure Determination of the Freezing Point of Cyclohexane A 20 x 50 mm test tube was rinsed clean with cyclohexane.