Peter Wothers: Just Add Water

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Partner:: Australian Broadcasting Corporation
Location:: Australian National University
Canberra, Australia
Event Date:: 08.18.09
Speaker:: Peter Wothers
Tags:: water; chemistry; experiment

Summary: Water covers three quarters of our planet and makes up 70% of our bodies, but how much do we really know about H20?

In this literally explosive demonstration, Dr. Peter Wothers, from the department of chemistry at Cambridge University, examines the properties of water.

Bio

Peter Wothers

Dr. Peter Wothers is currently Director of Studies in Chemistry at St Catharine's College, Cambridge (UK).

He also sits on the Committee for the Chemistry Olympiad for the Royal Society of Chemistry and has spent the past 10 years passing on his knowledge and enthusiasm for science to a wider audience.

Chapters

: Watch Full Program

57 min 31 sec

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01.: The Commonness of Water

02 min 39 sec

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02.: Water and the Human Body

02 min 49 sec

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03.: How Water Aids Chemical Reactions

04 min 14 sec

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04.: Water and Digestion

02 min 23 sec

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05.: Dehydrating a Carbohydrate

03 min 21 sec

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06.: Hydrogen and Oxygen: The Building Blocks of Water

04 min 07 sec

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07.: Mixing Hydrogen and Oxygen

02 min 55 sec

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08.: Other Experiments with Hydrogen and Oxygen

05 min 07 sec

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09.: The Physics of Liquid Water

04 min 54 sec

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10.: The Physics of Solid Water

02 min 30 sec

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11.: The Physics of Gaseous Water

04 min 15 sec

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12.: Experiments with Boiling Water

04 min 14 sec

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13.: Boiling Point, Elevation, and the Egg Experiment

05 min 12 sec

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14.: How Air Pressure Affects Boiling Point

02 min 10 sec

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15.: Why Salt Dissolves in Water

01 min 47 sec

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16.: Results of the Egg Experiment

01 min 26 sec

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17.: Putting Out a Grease Fire

03 min 22 sec

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: Watch Full Program

57 min 31 sec

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Dr. Peter Wothers: Why Humans Need Water

01 min 54 sec

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Watch Full Program

57 min 31 sec

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Encyclopædia Britannica Article

water: Inorganic compound composed of hydrogen and oxygen (H2O), existing in liquid, gas (steam, water vapour), and solid (ice) states. At room temperature, water is a colourless, odourless, tasteless liquid. One of the most abundant compounds, water covers about 75% of Earth's surface. Life depends on water for virtually every process, its ability to dissolve many other substances being perhaps its most essential quality. Life is believed to have originated in water (the world's oceans or smaller bodies), and living organisms use aqueous solutions (including blood and digestive juices) as mediums for carrying out biological processes. Because water molecules are asymmetric and therefore electric dipoles, hydrogen bonding between molecules in liquid water and in ice is important in holding them together. Many of water's complex and anomalous physical and chemical properties (high melting and boiling points, viscosity, surface tension, greater density in liquid than in solid form) arise from this extensive hydrogen bonding. Water undergoes dissociation to the ions H+ (or H3O+) and OH-, particularly in the presence of salts and other solutes; it may act as an acid or as a base. Water occurs bound (as water of hydration) in many salts and minerals. It has myriad industrial uses, including as a suspending agent (papermaking, coal slurrying), solvent, diluting agent, coolant, and source of hydrogen; it is used in filtration, washing, steam generation, hydration of lime and cement, textile processing, sulfur mining, hydrolysis, and hydraulics, as well as in beverages and foods. See also hard water; heavy water.; water on britannica.com