cool hot vapors or liquids Test Tube A small cylindrical glass used for heating small amounts of liquid open at the top‚ usually with a rounded U-shaped bottom. Test tubes are widely used by chemists to hold‚ mix‚ or heat small quantities of solid or liquid chemicals Evaporating Dish A porcelain used in evaporating chemical solutions Evaporating dishes are used to evaporate excess solvents Beaker Thin glass vessel used as container and heating liquids It is used for stirring‚ mixing
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Chemistry Lab Report Practical #1 Title: The Densities of Liquids and Solids Date: 29th of August 2014 Session: Friday 1 p.m. Student’s name: Alua Sarybay Lab partner’s name: Gulzhauhar Nurdildayeva Tutor’s name: Eugene Douglass Introduction The matter can be observed by determining‚ measuring and monitoring its chemical and physical properties. In this experiment the densities of liquids and solids will be determined. The density is an intensive property of matter that does not depend
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determined by observing its crystals and finding its melting point. The melting point is usually expressed as a range. The first number is the temperature at which melting is first observed and the second number is the temperature at which the solid is completely melted. Pure substances will have a higher melting point and a narrower melting point range closer to the literature value versus impure substances which will have a lower melting point and a larger range. The literature melting
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I. DATA AND OBSERVATIONS Table 1. Description of reagents. Reagents Description Salicylic acid Fine powdery white solid crystals 95% ethanol Clear colorless liquid Acetyl chloride Clear colorless liquid with gas escaping from container FeCl3 Clear colorless liquid Commercial aspirin Fine powdery white solid crystals I2/KI Deep black liquid KMnO4 Brownish liquid Phosphoric acid Clear colorless liquid Table 2. Preparation of Aspirin. Description Salicylic acid + Acetyl
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CHAPTER 10 Liquids and Solids 1. Order the intermolecular forces (dipole-dipole‚ London dispersion‚ ionic‚ and hydrogen-bonding) from weakest to strongest . a) dipole-dipole‚ London dispersion‚ ionic‚ and hydrogen-bonding b) London dispersion‚ dipole-dipole‚ hydrogen-bonding‚ and ionic c) hydrogen-bonding‚ dipole-dipole‚ London dispersion‚ and ionic d) dipole-dipole‚ ionic‚ London dispersion‚ and hydrogen-bonding e) London dispersion‚ ionic‚ dipole-dipole‚ and hydrogen-bonding Ans: b 2. Hydrogen
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height above sea level. Boiling When a liquid vaporises. Capillary action When water is drawn up between close fitting surfaces. Compression force A crushing force. Condensation When a gas turns into a liquid. Conduction Method by which solids transfer heat. Convection Method by which liquids and gases transfer heat. Corrosion The deterioration of metals that occurs on contact with liquids. Ductility Ductility is the ability of a material to withstand distortion without fracture‚
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2009). Freezing point is the fixed temperature at which a pure liquid converted into crystalline solid. Melting point is the fixed temperature at which a crystalline solid converted to a liquid (Ebbing & Gammon‚ 2010). The melting point of a solid and the freezing point of its liquid is the same. It is the temperature at which the rate of freezing of its liquid is the same as the rate of melting of a solid under a given applied pressure (Whitten‚ Davis & Peck‚ 2009). A change of state involves the removal
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An alloy is a solid solution or homogeneous mixture of two or more elements where a material with better or different properties is produced. The range of alloys produced depends on the solubility of the constituents and the proportion of them. The number of possible alloy combinations is almost endless since any metal can be alloyed in pairs or in multiples. Alloys can be classified into two main categories:Interstitial alloy. It is when smaller elements‚ such as boron‚ carbon‚ nitrogen‚ or silicon
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Unit-1 THE SOLID STATE QUESTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. 2. 3. 4. 8. 9. What are anistropic substances. Why are amorphous solids isotropic in nature? Why glass is regarded as an amorphous solid? Define the term ’crystal lattice.’ Define the term voids. What type of stochiometric defect is shown by (i) ZnS and (ii) CsCl? [Hint. : (i) Frenkel defect (ii) Schottky defect] *10. If the formula of a compound is A2B‚ which sites would be occupied by A ions? [Hint. : Number of A ions is
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eutectic point. Melting point of a solid is the temperature at which the solid and its liquid form are in equilibrium‚ i.e.‚ molecules move back and forth between the two states at the same rate‚ so both phases remain present. If the temperature of a solid is measured carefully as the solid is heated‚ the temperature will be observed to rise until the melting point (m.p.) of the solid is reached‚ and then the temperature will remain almost constant while the solid melts. The heat absorbed during melting
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