Haruki Sato Un Official Fan Site Tribute

Haruki Sato : This Is An Un Official Fan Site Tribute
Haruki Sato
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Movie Title Year Distributor Notes Rev Formats Banned Onanie Hole 2013 Moodyz Before My Wedding 2012 Akinori Big Breast Splash Instructor 2013 Wanz Bukkake Fan Thanksgiving Festival Swimsuit Version 2011 Soft on Demand Facial Creampie Into Big Breast Girl 2012 Momotoro Japan Creampie Creampie Soapland 2013 Soft on Demand Creampie Cute Little Incontinent Sweetheart: Haruki Sato 2013 Moodyz Pee Drunk Girl 2012 E-Body Erotic Busty Soaplady 2012 Soft on Demand Fully Nude Oil Kat Fight 2 2014 Rocket LezOnly Squirt Pee Get the Gal's Body 2012 Soft on Demand Glory Body 2012 Moodyz Group Creampie Rape 2013 Moodyz Creampie Hand Job Clinic 2012 Soft on Demand Hand Job Clinic 15 2013 Soft on Demand Haruki Sato Climax Special 2012 Soft on Demand Heaven for Masochist Man 2 2013 Moodyz I'll Give You My 48 Hours 2012 Soft on Demand Lewd Diva 2012 Soft on Demand Madam Lesbian Swimming Lesson 2012 Soft on Demand LezOnly Maximum Exposure Fishing For Men: Haruki Sato 2012 Moodyz Squirt Milky Sport 2011 Soft on Demand My Best's Friend Mother 2012 Soft on Demand Nude Maid Dispatch Center, Big Tits Division, Haruki Sato Speaking 2015 Nadeshiko Facial Creampie Platinum Ticket for Sex with Haruki Sato 2012 Soft on Demand
Premature Ejaculation Camp Training 2012 Soft on Demand Raped at Hot Spring 2011 Moodyz Raped Beautiful Secret Investigators 2013 Moodyz Raped Police Investigator 2012 Hibino Rich Kiss and Sex 2013 IdeaPocket Sex School 2012 Soft on Demand Splash DX 2011 Soft on Demand Splash Idol 2012 Soft on Demand Splash Instructor 2012 Soft on Demand Stalker (II) 2012 Soft on Demand Super Boin Player 2012 Moodyz Tentacle Acme 11 2012 Soft on Demand The Customer Is Always Right My Part-Time Job 2011 K.M. Produce Facial True Love Lesbian 2012 Soft on Demand LezOnly Whole Body Sapping Esthetic Salon 2012 Soft on Demand Young Wife and Father-In-Law 2012 Hibino penetration [23] and is widely observed in common situations including fluid absorption into paper and rising damp in concrete or masonry walls. For a bar shaped section of material with cross-sectional area A that is wetted on one end, the cumulative volume V of absorbed liquid after a time t is {\displaystyle V=AS{\sqrt {t}},}V = AS\sqrt{t}, where S is the sorptivity of the medium, in units of m·s-1/2 or mm·min-1/2. This time dependence relation is similar to Washburn's equation for the wicking in capillaries and porous media.[30] The quantity

{\displaystyle i={\frac {V}{A}}}i = \frac{V}{A} is called the cumulative liquid intake, with the dimension of length. The wetted length of the bar, that is the distance between the wetted end of the bar and the so-called wet front, is dependent on the fraction f of the volume occupied by voids. This number f is the porosity of the medium; the wetted length is then {\displaystyle x={\frac {i}{f}}={\frac {S}{f}}{\sqrt {t}}.}x = \frac{i}{f} = \frac{S}{f}\sqrt{t}. Some authors use the quantity S/f as the sorptivity.[31] The above description is for the case where gravity and evaporation do not play a role. Sorptivity is a relevant property of building materials, because it affects the amount of rising dampness. Some values for the sorptivity of building materials are in the table below. Sorptivity of selected materials (source:[32]) Material Sorptivity (mm·min-1/2) Aerated concrete 0.50 Gypsum plaster 3.50 Clay brick 1.16 Mortar 0.70 Concrete brick 0.20 See also Bond number Bound water Capillary fringe Capillary pressure Capillary wave Capillary bridges Damp-proof course Darcy's law Frost flowers Frost heaving Hindu milk miracle Krogh model Needle ice Surface tension Washburn's equation Water Wick effect Young–Laplace equation Water is an inorganic, transparent, tasteless, odorless, and nearly colorless chemical substance, which is the main constituent of Earth's hydrosphere and the fluids of all known living organisms. It is vital for all known forms of life, even though it provides no calories or organic nutrients. Its chemical formula is H2O, meaning that each of its molecules contains one oxygen and two hydrogen atoms, connected by covalent bonds. Water is the name of the liquid state of H2O at standard ambient temperature and pressure. It forms precipitation in the form of rain and aerosols in the form of fog. Clouds are formed from suspended droplets of water and ice, its solid state. When finely divided, crystalline ice may precipitate in the form of snow. The gaseous state of water is steam or water vapor. Water moves continually through the water cycle of evaporation, transpiration (evapotranspiration), condensation, precipitation, and runoff, usually reaching the sea. Water covers 71% of the Earth's surface, mostly in seas and oceans.[1] Small portions of water occur as groundwater (1.7%), in the glaciers and the ice caps of Antarctica and Greenland (1.7%), and in the air as vapor, clouds (formed of ice and liquid water suspended in air), and precipitation (0.001%).[2][3] Water plays an important role in the world economy. Approximately 70% of the freshwater used by humans goes to agriculture.[4] Fishing in salt and fresh water bodies is a major source of food for many parts of the world. Much of the long-distance trade of commodities (such as oil, natural gas, and manufactured products) is transported by boats through seas, rivers, lakes, and canals. Large quantities of water, ice, and steam are used for cooling and heating, in industry and homes. Water is an excellent solvent for a wide variety of substances both mineral and organic; as such it is widely used in industrial processes, and in cooking and washing. Water, ice and snow are also central to many sports and other forms of entertainment, such as swimming, pleasure boating, boat racing, surfing, sport fishing, diving, ice skating and skiing. Contents 1 Etymology 2 History 3 Chemical and physical properties 3.1 States 3.1.1 Density 3.1.2 Phase transitions 3.1.3 Triple and critical points 3.1.4 Phases of ice and water 3.2 Taste and odor 3.3 Color and appearance 3.4 Polar molecule 3.5 Hydrogen bonding 3.6 Self-ionisation 3.7 Electrical conductivity and electrolysis 3.8 Mechanical properties 3.9 Reactivity 4 On Earth 4.1 Water cycle 4.2 Fresh water storage 4.3 Sea water and tides 5 Effects on life 5.1 Aquatic life forms 6 Effects on human civilization 6.1 Health and pollution 6.2 Human uses 6.2.1 Agriculture 6.2.2 As a scientific standard 6.2.3 For drinking 6.2.4 Washing 6.2.5 Transportation 6.2.6 Chemical uses 6.2.7 Heat exchange 6.2.8 Fire considerations 6.2.9 Recreation 6.2.10 Water industry 6.2.11 Industrial applications 6.2.12 Food processing 6.2.13 Medical use 7 Distribution in nature 7.1 In the universe 7.1.1 Water vapor 7.1.2 Liquid water 7.1.3 Water ice 7.1.4 Exotic forms 7.2 Water and habitable zone 8 Law, politics, and crisis 9 In culture 9.1 Religion 9.2 Philosophy 9.3 Dihydrogen monoxide parody 10 See also 11 References 12 Further reading 13 External links Etymology The word water comes from Old English wæter, from Proto-Germanic *watar (source also of Old Saxon watar, Old Frisian wetir, Dutch water, Old High German wazzar, German Wasser, Old Norse vatn, Gothic wato), from Proto-Indo-European *wod-or, suffixed form of root *wed- ("water"; "wet").[5] Also cognate, through the Indo-European root, with Greek ?d?? (ýdor), Russian ????´ (vodá), Irish uisce, Albanian ujë. History Main articles: Origin of water on Earth § History of water on Earth, and Properties of water § History Chemical and physical properties Main article: Properties of water See also: Water (data page) and Water model Water (H 2O) is a polar inorganic compound that is at room temperature a tasteless and odorless liquid, nearly colorless with a hint of blue. This simplest hydrogen chalcogenide is by far the most studied chemical compound and is described as the "universal solvent" for its ability to dissolve many substances.[6][7] This allows it to be the "solvent of life":[8] indeed, water as found in nature almost always includes various dissolved substances, and special steps are required to obtain chemically pure water. Water is the only common substance to exist as a solid, liquid, and gas in normal terrestrial conditions.[9] States The three common states of matter Along with oxidane, water is one of the two official names for the chemical compound H 2O;[10] it is also the liquid phase of H 2O.[11] The other two common states of matter of water are the solid phase, ice, and the gaseous phase, water vapor or steam. The addition or removal of heat can cause phase transitions: freezing (water to ice), melting (ice to water), vaporization (water to vapor), condensation (vapor to water), sublimation (ice to vapor) and deposition (vapor to ice).[12] Density Water differs from most liquids in that it becomes less dense as it freezes.[14] In 1 atm pressure, it reaches its maximum density of 1,000 kg/m3 (62.43 lb/cu ft) at 3.98 °C (39.16 °F).[15] The density of ice is 917 kg/m3 (57.25 lb/cu ft), an expansion of 9%.[16][17] This expansion can exert enormous pressure, bursting pipes and cracking rocks (see Frost weathering).[18] In a lake or ocean, water at 4°C sinks to the bottom and ice forms on the surface, floating on the liquid water. This ice insulates the water below, preventing it from freezing solid. Without this protection, most aquatic organisms would perish during the winter.[19] Phase transitions At a pressure of one atmosphere (atm), ice melts or water freezes at 0 °C (32 °F) and water boils or vapor condenses at 100 °C (212 °F). However, even below the boiling point, water can change to vapor at its surface by evaporation (vaporization throughout the liquid is known as boiling). Sublimation and deposition also occur on surfaces.[12] For example, frost is deposited on cold surfaces while snowflakes form by deposition on an aerosol particle or ice nucleus.[20] In the process of freeze-drying, a food is frozen and then stored at low pressure so the ice on its surface sublimates.[21] The melting and boiling points depend on pressure. A good approximation for the rate of change of the melting temperature with pressure is given by the Clausius–Clapeyron relation: {\displaystyle {\frac {dT}{dP}}={\frac {T\left(v_{\text{L}}-v_{\text{S}}\right)}{L_{\text{f}}}},}{\displaystyle {\frac {dT}{dP}}={\frac {T\left(v_{\text{L}}-v_{\text{S}}\right)}{L_{\text{f}}}},} where {\displaystyle v_{\text{L}}}{\displaystyle v_{\text{L}}} and {\displaystyle v_{\text{G}}}{\displaystyle v_{\text{G}}} are the molar volumes of the liquid and gas phases, and {\displaystyle L_{\text{f}}}{\displaystyle L_{\text{f}}} is the molar latent heat of melting. In most substances, the volume increases when melting occurs, so the melting temperature increases with pressure. However, because ice is less dense than water, the melting temperature decreases.[13] In glaciers, pressure melting can occur under sufficiently thick volumes of ice, resulting in subglacial lakes.[22][23] The Clausius-Clapeyron relation also applies to the boiling point, except now the vapor phase has a much lower density than the liquid phase, so the boiling point increases with pressure.[24] Water can remain in a liquid state at high temperatures in the deep ocean or underground. For example, temperatures exceed 205 °C (401 °F) in Old Faithful, a geyser in Yellowstone National Park.[25] In hydrothermal vents, the temperature can exceed 400 °C (752 °F).[26] At sea level, the boiling point of water is 100 °C (212 °F). As atmospheric pressure decreases with altitude, the boiling point decreases by 1 °C every 274 meters. High-altitude cooking takes longer than sea-level cooking. For example, at 1,524 metres (5,000 ft), cooking time must be increased by a fourth to achieve the desired result.[27] (Conversely, a pressure cooker can be used to decrease cooking times by raising the boiling temperature.[28]) In a vacuum, water will boil at room temperature.[29] Triple and critical points Phase diagram of water simplified On a pressure/temperature phase diagram (see figure), there are curves separating solid from vapor, vapor from liquid, and liquid from solid. These meet at a single point called the triple point, where all three phases can coexist. The triple point is at a temperature of 273.16 K (0.01 °C) and a pressure of 611.657 pascals (0.00604 atm);[30] it is the lowest pressure at which liquid water can exist. Until 2019, the triple point was used to define the Kelvin temperature scale.[31][32] The water/vapor phase curve terminates at 647.096 K (373.946 °C; 705.103 °F) and 22.064 megapascals (3,200.1 psi; 217.75 atm).[33] This is known as the critical point. At higher temperatures and pressures the liquid and vapor phases form a continuous phase called a supercritical fluid. It can be gradually compressed or expanded between gas-like and liquid-like densities, its properties (which are quite different from those of ambient water) are sensitive to density. For example, for suitable pressures and temperatures it can mix freely with nonpolar compounds, including most organic compounds. This makes it useful in a variety of applications including high-temperature electrochemistry and as an ecologically benign solvent or catalyst in chemical reactions involving organic compounds. In Earth's mantle, it acts as a solvent during mineral formation, dissolution and deposition

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