intramolecular forces. 8. What is a dipole-dipole force? 9. What are hydrogen bonds? 10. a) Why is the melting and boiling point of H2O significantly higher than H2S? b) Predict and explain the relative melting and boiling points of HF‚ HCl‚ HBr and HI. 11. What are London or dispersion forces? How are they affected by molecular size? 12. Which is expected to have the higher boiling point‚ C8H18 or C22H46? Explain. 13. What type of solid contains particles held together primarily
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Edexcel Level 3 BTEC Nationals in Applied Science (Forensic Science) Unit 01 – Fundamentals of Science Assignment 01-01‚ Volumetric Analysis Date set: Sept 2010 Date due: Oct 2010 This assignment addresses the following Criteria… Unit 1 – Fundamentals of Science Assessment and grading criteria To achieve a pass grade the evidence must show that the learner is able to: To achieve a merit grade the evidence must show that‚ in addition to the pass criteria‚ the learner is able to: To
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(7)plus holder and tray - Copper sulphate solution (CuSO4) - White dropping ray - tripod stand and mesh -stopwatch - Biuret͛s solution - Sodium Hydroxide solution (NaOH) (or Potassium Hydroxide solution) - Hydrochloric Acid (HCl) - Sodium Hydrogencarbonate (NaHCO3) - Iodine Solution(I2) (or Potassium Iodide solution) - Ethanol (C2H5OH) - distilled water (H2O) Test Method Reducing Sugars 2cm3 of solutions A-G were placed into separate‚ labelled test tubes using separate measuring
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activator of Peroxidase because salt contains Na ions which attaches tothe allosteric site changing the shape of the enzyme to fit a substrate. Materials: • Peroxidase (enzyme in potato) • Hydrogen peroxide‚ 3% • A strong acid‚ pH3 (lemon juice‚ or HCL) 0.5 • A strong base‚ pH 10 (drain cleaner‚ NaOH) 0.5 mol/L • A weak acid‚ pH 6 (vinegar‚ acetic acid( CH3COOH)) 0.5
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acid ionizes only slightly‚ perhaps 3-5%. Hydrochloric acid is a strong acid. When a HCl(g) molecule is dissolved in water‚ the covalent bond holding the H and Cl atoms together is broken. The hydrogen atom forms a new bond with an oxygen atom of water‚ making a hydronium ion. The chlorine atom keeps the two electrons of its bond with hydrogen‚ making a chloride ion. The process is shown in the equation below. All HCl molecules or
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Reaction | A | NaHCO3 and HCI - C02 | The mixture didn’t look any different amongst the contrast of each colored background. | B | HCI and BTB | The mixture is orange. The color doesn’t change amongst the contrast of each colored background. | C | NH3 and BTB | The mixture is blue. I expected the mixture to turn orange | D | HCI and blue dye | The mixture is green. | E | Blue dye and NaOCI | Prior to adding the HCl the mixture was light blue‚ after the addition of HCl the mixture turns
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Chemical Changes Lab Report Expectations: Data Table 1: What you Expected to happen Well #/ Question Chemicals Reaction A NaHCO3 and HCI - C02 A bubble occurrence B HCI and BTB A deep yellow C NH3 and BTB A purple color D HCI and blue dye A deep blue E Blue dye and NaOCI A greenish color F NaOCI and KI A bright red G KI and Pb(NO3)2 A yellow
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it undergo damage due to eating chocolates and sweets? Q4. Name the gas usually liberated when a dilute acid reacts with a metal. What happens when a burning candle is brought near this gas? Q5. What are the products obtained on heating NaHCO3. Write the chemical equation for the reaction involved in the above. What is the colour of CuSO4 crystals before heating and after heating the crystals? What is meant by water of crystallization of a substance? Describe an activity to show that copper
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electronegativity and how that determines solubility of ionic compounds. This demonstration is beneficial to use in both the Solution and Solubility‚ and Chemical Reactions units. | Materials | distilled water – saturated sodium bicarbonate (NaHCO3) – 20% sodium carbonate solution (Na2CO3) - phenolphthalein indicator – saturated barium chloride (BaCl2) – sodium dichromate crystals – concentrated hydrochloric acid – water glass – wine glass – milk glass – beer mug | Safety | All chemicals
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Extraction and Evaporation: Separating the Components of "Panacetin" Submitted- July 17‚ 2012 Introduction The purpose of this lab is to investigate the composition of a compound suspected to be Panacetin‚ a type of pain-killer. Panacetin is typically made up of sucrose‚ aspirin‚ and acetaminophen‚ but the third component in this experiment is unknown. The unknown component is suspected to be a chemical relative of acetaminophen‚ either acetanilide or phenacetin. Using techniques such as
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