0.00079 moles EDTA4- c. 0.00079 moles ZnI2 d. 0.0517 grams of ZnI2 are in the sample e. 0.0517/0.237= 21.8% f. Error Is 6.34% Lab Report: Part 1: In this lab we used the following supplies: * Zinc Iodide * Na2H2EDTA(s) * Calmagite indicator solution * pH 10 buffer solution * 6M Acetic Acid * Unknown Zinc Compound The main purpose for this part of the lab was to determine the amount of zinc ion in a sample of ZnI2 by titration. The two types of zinc: * Zinc iodide made by zinc and iodine * Commercially purchased zinc iodide (the
0.00512g ZnI2/mL of solution 0.00512g/319.18 g/mol=1.6*10-5 mol 1.6*10-5 mol/(1*10-3L)=0.016M c. 0.00806 moles of ZnI2/500 mL of solution 0.00806mol/(500*10-3)L=0.016M d. 0.0161 moles of ZnI2/L of solution 0.0161mol/1L=0.016M Exercise 4: a. The moles of ZnI2: 0.25M*(250*10-3)L=0.0625mol b. 0.25M*(250*10-3)L=0.0625mol The mass of ZnI2: 0.0625mol*319.18 g/mol=19.95g c. 0.25M*(500*10-3)L=0.125mol 0.125mol*319.18 g/mol=39.9g ZnI2 d. 0.0125mol/0.25M=0.05L Exercise 5: a. 0.125M*(100*10-3)L=0.0125mol b. 0.0625mol/0.125M=0.5L=500mL Calculation for preparing the EDTA solution Exercise 6 a.
Write the Molecular Formula for Each of the Following: a. A compound with a molecular mass of 70g/mol and an empirical formula of CH2. b. A compound with a molecular mass of 46.0g/mol and an empirical formula of NO2 Molecular Formula Worksheet Write the molecular formulas of the following compounds: 1) A compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole. 2) A compound with an empirical formula of C4H4O and a molar mass of 136 grams per mole.
2 marks 4 Draw the structural formula of Compound G. 1 mark 5 Using the chemical shift correlation for 13C NMR, predict the number of peaks for Compound G and draw in the position of the peaks on the blank spectrum below, annotating each peak with its corresponding structure. (2 marks) 6 Draw the structural formula for 2-chloro but-2-ene. Below this draw a structural formula of an isomer of 2-chloro but-2-ene and name this substance.
We used 1g of Na2CO3 -Sodium Carbonate. This would allow for the full precipitate to form. 4) Procedure: Refer to CHE 111 lab manual, experiment Stoichiometry of a Precipitation Reaction on page #104 5) Data / results. We used 1g of Na2CO3 -Sodium Carbonate in combination with 1g CaCl2·2 H2O-Calcium Chloride, Dihydrate to form the precipitate reaction. Na2CO3 aq + CaCl2*2H2O aq = CaCO3 s + 2 NaCl aq + 2 H2O aq Molar Mass: Ca = 40.08 Cl2 = (35.45) x 2 = 70.9 2H2O = (18.02) x 2 = 36.04 40.08 + 70.90 + 36.04 = 147.02 g/mol CaCl2*2H2O Theoretical yield: 1g CaCl•2H2O x 1 mol CaCl•2H2O x 1 mol CaCO3 x 100.09g CaCO3 = 0.68 g CaCO3 147.02g CaCl•2H2O 1 mol CaCl•2H2O 1 mol CaCO3 Mass of weighing dish = 0.6g Mass of filter paper =
1. An introduction for this experiment. Refer to your lab manual on pages x-xi for what an introduction should include and an example. In this experiment, the molecular weight of an unknown solid is determined through the depression of the freezing point of pure p-xylene. When p-xylene is mixed with another substance the freezing point lowers.
A. 600 mm Hg B. 314 mm Hg C. 34.9 mm Hg D. 69.8 mm Hg _____ 6. For first-order reactions, the rate constant, k, has the units A. M s-1 B. M-1 s-1 C. M-2 s-1 D. s-1 _____ 7. For second-order reactions the slope of a plot of 1/[A] versus time
EXPERIMENT 6 Title Kinetics of Chemical Reaction – Iodination of Cyclohexanone Aim To determine the value of the rate constant, k and order of reaction, a, b and c, and also to suggest a mechanism which agrees with the rate equation that has been obtained. Background Theory The basis of the theory of absorbance is as follows: Io ―――――→ sample ―――――→I if Io = I, no absorbance occur Io > I, the sample absorbs certain amount of light wave Io < I, the sample emits certain amount of light of certain wave length. THE HALOGENATION (IODINATION) OF KETONES (CYCLOHEXANONE) This experiment examined the rate of iodination of cyclohexanone in an aqueous medium. To increase the amount of iodine in the solution, iodine is converted to a more soluble complex ion, I3- by the addition of excess iodide ion: I2 + I- →I3- One of the characteristic reactions of ketones is the substitution of a halogen for one of the hydrogen is adjacent to the ketone group. The net reaction is: This reaction has been studied extensively and occurs for a wide variety of ketones.
In order to find the concentration of NaOH we need to tag along the following steps: a- note down the balanced chemical equation for the reaction C8H5O5K+NaOH→C8H4O4KNa+H2O b- pull out applicable information from the experiment: C8H5O5K V=0.025 dm3 C=0.2M NaOH V=0.021 dm3 C= ?? c- calculate number of moles
The values found for KH+ for the reaction using HCl as the acid were found to be (i)KH+ = 4.96x10-5, (ii)KH+ = 1.24x10-5, (iv)KH+ = 1.84x10-5. The KHA value for the reaction using ClCHCOOH as the acid was found to be (iii) KHA = 2.985. Introduction: The aim of this experiment is to perform a titration of an acid, HCl/ClCHOOH against Na2S2O3. Form plotting the results we then want to find Kobs for each reaction and KH+/KHA for the reactions. Kobs is the slope on the graph plotting Vol of NaaS2O3 against time.