CuSO4 4. What is the molar mass for anhydrous (without water) copper(II) sulfate? 159.62 g/mol Result: Observation: Some gray white substances precipitated from the water in the crucible. Data: * Mass of purified crucible and lid 30.59g * Mass of crucible and lid and hydrate 31.57g * Mass of hydrate alone 31.57g- 30.59g = .98g * Mass of crucible and lid and dehydrate 31.11g * Mass of dehydrate alone .52g This lab shows that hydrates are made up of crystal solids and water,
When in flame it produces gas rapidly and bubbles. Liquid turns into gas quickly. When liquid disappears solution (now a solid) turns white | 4 | A Initial temperature is 15 degrees Celsius and the final temperature is 17 degrees Celsius. BThe blue hydrated copper sulphate turned white, evidence of condensation of a clear liquid present on the inside of the test tube.C concentrated sulphuric acid turns black on paper towel and is clear on the white cottonD Carbon pillar grows cause of air bubbles, it is brittle, it is both corrosive with a hole and there is evidence of carbon produced | 5 | No temperature change and iodine brown/yellow gas produced | Properties of Sulphuric acid results table Aim: To investigate and observe the properties of sulphuric acid through five different experiments where we will determine its extent of ionisation in aqueous solution, reaction of sulfate ions, action as a strong acid, affinity for water and action as an oxidising agent. Background: Sulfuric acid (H2SO4) is a diprotic acid (can donate 2 protons to a base).
This product, dibromocholesterol, was washed and debrominated by an elimination reaction using zinc dust. Percent yield and recovery evaluated the efficiency of this synthesis. Melting point and thin layer chromatography (TLC) analysis assessed the purity of commercial cholesterol, dibromocholesterol, and synthesized cholesterol by physical analysis. Chemical tests evaluated the purity of these samples by assessing the presence of specific functional groups. Silver nitrate tested for 2o and 3o alkyl halides expected in dibromocholesterol and sulfuric acid tested for alkenes expected in cholesterol.
Repeat the titration until there are two titres within 0.1cm3 of each other. Record results in a suitable table. Results: Rough Titre: 7.653 First Run: 6.553 Second Run: 6.453 Third Run: 6.553 Calculations: During the titration, iron(II) ions are oxidised to iron(III) ions and manganate(VII) ions are reduced to manganese(II) ions. The equation is as follows: 5Fe2+(aq) + MnO4-(aq) + 8H+(aq) ? 5Fe3+(aq) + Mn2+(aq) + 4H2O(l) The above equation shows that one mole of manganate(VII) ions reacts with 5 moles of iron(II) ions in acid solution.
A. ethanoic acid B. ethyl ethanoate C. hexane D. hex-1-ene 8. A compound boils at –33oC. It also dissolves in water to give an alkaline solution. Which type of bonding is present within the compound? A. metallic B. covalent (polar) C. ionic D. covalent (non-polar) 9.
Calculate the exact normality of Na2S2O3 knowing that in this chemical reaction 1 gram-equivalent of K2Cr2O7 react with 1 gram-equivalent of Na2S2O3 (1 mole K2Cr2O7 react with 6 moles Na2S2O3). Determination of peroxide value. Weigh 3.00 g oil (with precision of 0.001 g) into a 250 ml Erlenmeyer flask. Add 10 ml chloroform and swirl to dissolve oil. Add 15 ml acetic acid,
W = Wa + 1.06 Wa/1000 Table. Density of water at various temperatures. Temperature (°C ) 26 27 28 29 30 31 32 33 34 Density of water ( g mL-1) 0.99681 0.99654 0.99626 0.99597 0.99567 0.99537 0.99503 0.99473 0.99440 How to use a pipette 1 Rinse a 25-mL pipette with two or three small volumes of distilled water, and then with a complete volume of distilled water. 2 Do not immerse the tip of the pipette too deep into the water. The tip should not be above the water level so as to avoid any mishap during the suction of the water into the pipette via the pipette filler or suction bulb.
(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.
| 3 drops of 1% dimethylglyoxime solution. | [Ni(NH3)6]2+ + 2H2DMG→ Ni(HDMG)2 + 2NH4+ + 4NH3 | 9 Al3+ | By heating the solution in the hot water bath. | A black gelatinous precipitate was changed to colorless. | 6M NH3 | [Al(OH)4]- + 4H+ → Al3+ + 4H2O | 10 | Centrifuge the solution. | Colorless solution.
Chemistry Lab Types of Chemical Reactions OBSERVATION DATA TABLE Step|Name of Reactants|Description of Reactants|Description of reaction taking place (evidence of chemical reaction)|Description of Products| 1|Zn|Solid, small chunky bits, Silvery-grey, dull|As the Zinc and Sulfur heated up it expanded in the test tube and shot out Zinc Sulfide.-light and heat are produced|White powder was created and the leftovers of the reactions was a black powder.| |S|Solid, resembles powder, Off-yellowOpaque||| 2|KI|-dull yellow liquid-transparent|Instantaneously changed colour to a bright yellow.|-Bright yellow liquid-Opaque| |Pb(NO3)2|-liquid, transparent, very clear-bubbly||| 3|H2O2|-liquid-clear-transparent|A dark grey bubbling liquid was created. It got hotter as it reacted.gas test observations:The splint relit. Oxygen was present.|Oxygen gas was created and a dark grey opaque liquid was left behind in the test tube. | |MnO2|-solid-powder-black||| 4|AgNO3|A clear, transparent liquid.|As the copper reacted with the Silver Nitrate, the ball of Copper changed colour to grey and subsequently developed a ‘furry-like’ characteristic on its coating.|-Clear liquid-Copper changes to a grey colour, ‘furry-like’.| |Cu|-brown/red-solid-stringy||| 5|HCl|A clear, transparent liquid.|When the Magnesium was inserted the HCl liquid started to bubble and fizz releasing Hydrogen. The Magnesium strip dissolved in the process and the test tube got hotter.