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.
a) mass c. color b) density d. boiling point 4) An example of an element is . a) sugar c. water b) soil d. oxygen 5) An example of a heterogeneous mixture is . a) salt c. mud b) nitrogen d. air 6) Which process is a chemical change? a) heating to boiling b) dissolving in alcohol c) burning in air d) slicing into two pieces 7) Water boiling at 100°C is an example of a(n) . a) chemical property c. physical property b) extensive property d. chemical change 8) Every pure chemical compound consists of two or more elements .
By dehydrating it using fire. The contrast mass between pure solid and solid with water gives the mass of water. 3. What is the formula for copper(II) sulfate? CuSO4 4.
Dipole-dipole forces are permanent dipoles due to different electronegativity. Hydrogen bonding is a strong dipole that forms when H bonds to N, O, or F. [7] Nitric acid (HNO3) is a colorless, toxic, oxidizing, and corrosive liquid commonly used as laboratory reagent and for the manufacture of fertilizers and explosives. [8] It is completely miscible and has a dipole moment of 2.17D[2]. It contains one hydrogen bond and is a polar molecule. Water (H2O) is colorless liquid that’s the basis of life on Earth.
Which one is not a pure substance? A) water B) oxygen C) air D) chlorine 6. Passing an electric current through a certain substance produces oxygen and sulfur. This substance cannot be a(n) A) compound B) mixture C) element D) pure substance 7. The symbol for the element potassium is A) K B) Kr C) P D) Pt E) Po 8.
A. barium sulphate B. calcium carbonate C. silver chloride D. sodium nitrate 3. An element X forms a hydroxide, which dissolves, both in acids and in alkalis. What could X be? A. aluminium B. calcium C. copper D. iron 4. In which reaction is dilute sulphuric acid not behaving as an acid?
(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.
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).
The reduction of permanganate requires strong acidic conditions. Introduction: In this experiment a purple colored solution of potassium permanganate, with an approximate concentration of 0.025M, will be added to a solution containing Fe2+ ions. The manganese is reduced from a 7+ oxidation state in the permanganate ion to form colorless Mn2+ ions. The equivalence point is indicated at the point when all of the Fe2+ ions in the solution are oxidized and the colorless mixture retains a purple tint. Procedure: Fill a buret and tip with KMnO4.