Exp 21 Reactivities of Some ALkyl Halides Summary: * The reactivities of several substrate types will be examined under both SN1 and SN2 reaction conditions in this experiment. * Sodium Iodide or Potassium Iodide in Acetone: A reagent composed of sodium iodide or potassium iodide dissolved in acetone is useful in classifying alkyl halides according to their reactivity in an SN2 reaction. * Silver Nitrate in Ethanol: A reagent composed of silver nitrate dissolved in ethanol is useful in classifying alkyl halides according to their reactivity in an SN1 reaction. Procedure: * Part A. Sodium Iodide in Acetone: * The Experiment: * Label ten test tubes from1 to 10.
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
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.
of moles of NaOH in 4.95 mL = 5.039 ×10-4 mol Concentration of NaOH = (5.039 ×10-4) ÷ (4.95÷ 1000) = 0.1018 M 1.2. Titration Set 2: Standardization of HCl 1.3.3 Results of Titration of HCl against NaOH Titration | 1 | 2 | Final Volume of Titrant/mL | 29.20 | 39.95 | Initial Volume of Titrant/mL | 18.50 | 29.25 | Volume of Titrant used/mL | 10.70 | 10.70 | | | | Indicator used | Methyl Orange | Colour Change at Endpoint | Red to Yellow | 1.3.4 Calculations Average volume of NaOH titrant used = 10.70 mL No. of moles of NaOH used = (10.70 ÷ 1000) × 0.1018 = 1.089 ×10-3 mol Chemical Equation of Reaction: HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) HCl reacts with NaOH in a 1:1 ratio, thus No.
How do you go from calculated/measured values to accomplishing stated purpose? (4 pts) The purpose of this lab is to determine the exact concentration of an unknown acetic acid solution. Titrations for two different reactions will be performed. Controlled volumes of one reagent are added to a flask containing the other reagent until the equivalence point of the reaction is reached, one between sodium hydroxide (NaOH) and potassium hydrogen phthalate (KHP) and the other between NaOH and acetic acid (CH3COOH). NaOH (aq) + KHP (aq) —› Na+ (aq) + K + (aq) + P2- (aq) + H2O (l) NaOH (aq) + CH3COOH (aq) —› Na+ (aq) + CH3COO- (aq) + H2O (l) The titration of NaOH with KHP will identify the concentration of the NaOH provided.
Results Sheet, Experiment 13 Brand of Vinegar used:________________ Acetic Acid % from bottle label_____________ | Initial NaOH Reading(estimate to 0.1 mL) | Final NaOH Reading(estimate to 0.1 mL) | Volume NaOH used(Final – Initial) | Trial 1 | 9.5 | 1.3 | 8.2 | Trial 2 | 9.6 | 1.4 | 8.2 | Trial 3 | 9.7 | 1.4 | 8.3 | Average Volume of NaOH used | 8.2 | Calculations: Normality of the acetic acid: .82 Mass of acetic acid: 49.2 % acetic acid (divide the grams, above, by the volume you used to get g/L): 4.92 Answer questions A-G in the lab manual: A. What is the average % acetic acid in your vinegar sample? Standard vinegar is 5% acetic acid. How does your result compare with the standard? The average was 4.92 which is pretty close comparably to the standard.
Calculate the molarity of the original vinegar solution and its concentration in gdm-3, given that it reacts with NaOH in a 1:1 ratio. 7. 2.5 g of a sample of ethanedioic acid, H2C2O4.nH2O, was dissolved in water and the solution made up to 250 cm3. This solution was placed in a burette and 15.8 cm3 were required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Given that ethanedioic acid reacts with NaOH
Methylene chloride: ethanol (1:1 solution) What solvent system will you be using to "develop" your TLC plates in the TLC of Analgesics lab? ethyl acetate with 0.5% solution of acetic acid How will you be visualizing your TLC plates in the TLC of Analgesics Lab? an UV lamp or a UV light What is the name of the hydrogenation catalyst used in the Hydrogenation of Olive Oil Lab? 10% Palladium on
EXPERIMENT ( 3 ) Topic : The preparation of Phenyl Benzoate from benzoyl chloride Introduction : The preparation of phenyl benzoate (ester) from phenol and benzoyl chloride is an esterification. In this experiment, you are requested to prepare and purify phenyl benzoate by some techniques. Chemicals : Phenol, Benzoyl chloride, Dilute NaOH, Methanol Procedures : 1. Dissolve 1 g phenol in 15 cm3 dilute NaOH using a 50 cm3 quickfit flask. 2.
Chempocalypse Now! Chapter 05 – Mass Spectrometry Page 1 Chapter 05 – Mass Spectrometry Topic A4 from the IB HL Chemistry Curriculum Assessment Statement Determine the molecular mass of a compound from the molecular ion peak. Analyze fragmentation patterns in a mass spectrum to find the structure of a compound. Obj 3 Teacher’s Notes A.4.1 A.4.2 3 Examples of fragments should include: + (Mr – 15) loss of CH3 + (Mr – 17) loss of OH + (Mr – 29) loss of C2H5 or CHO + (Mr – 31) loss of CH3O + (Mr – 45) loss of COOH Determining the molecular mass of a compound The mass spectrometer was introduced in Chapter 04, where we saw it was used to find the mass of individual atoms and the relative abundances of different isotopes. The instrument can be used in a similar way to find the relative molecular mass of a compound.