Which one of the following is a correct definition of a base that is not dependent upon the  solvent?
813376
bases are proton aceptors.
680075
A SOLUTE IS A SUBSTANCE WHICH IS DISSOLVED IN WATER\nA SOLVENT IS THE SECOND COMPONENT WHICH DISSOLVES THE SOLUTE.
1042768
Weak bases are good leaving groups (strong conjugate acids, don’t want to associate with protons or +ve charge as much as strong bases).And Mostly strong nucleophiles for example methoxide ions are strong nucleophile but a weak base as a leaving group
954718
IF substance contains both hydrophobic and hydrophilic parts:\n  Make the part that is soluble in polar solvents i.e the part having polarity in water and rest in some nonpolar solvent.\n\nIFsubstance is purely ionic represent it as ions in water.
865364
Solvent is a very generic term.  Basically, all it means is "a liquid that can dissolve a substance.\n\nWhether a particular liquid can dissolve a particular substance is based on the properties of the solvent and the substance you want to dissolve.\n\nExample:  \nWater is very good solvent for salts (not just NaCl - a salt is defined as any molecule held together by an ionic bond).  The partial charge on the oxygen and hydrogen in the water molecules disrupt this ionic bond - there by 'dissolving' salts.\n\nBut water is a poor solvent for any type of oil.  Oil is hydrophobic, and water will actually force oil molecules closer (thus the separation of oil in water).\n\nAcetone is another well known solvent.  As you probably know, it dissolves fingernail polish.  Water doesn't take off fingernail polish because the chemistry between the two substances doesn't support it.\n\nI hope this helps.\n\nSilk Dragon
592402
I agree with the first poster on C and E, but I'm not sure if A is also.  A solute dissolving in a solvent seems like a chemical process to me, but I don't remember for sure.
682358
basically, we call it an acid if the compound can be resolved into existing H+ and OH- ions. if this can be resolved then it is called acid and base. \n\nThis is pH. amount of H+ ions and amound of OH- ions. more the amount of free H+ ions in the compund more the acidic nature.\nmore the OH more the basic nature and less is the acidic nature.\n\nIt also depends on the medium in which the compound is present. some act as acids in aqueous medium. and so on....\n hope it was helpful. \nAny doubts u can ask further.
385549
a cell is organic, an atom is not.  a cell is made from atoms.
561562
polar.\n\nThe best way to think of it is in terms of water solubility.  Non polar organic molecules usually have lots of hydrogens, and usually no oxygens.
242245
This is the definition of a buffer.  It will control the pH against extreme changes.  If you add a small amount of strong acid, the weak base will neutralize it, bringing the pH back near the initial condition.  The reverse is true for adding strong base.
638442
The Bronstead-Lowry definition of an acid and a base is that\nAcids - are a substance that can transfer a proton to another substance\nBase - are a  substance that can accept a proton from another substance\nThese definitions emphasize proton transfer, and can include solvents other than water (aqueous solutions are not part of the definition, proton transfer is the key feature)\nThe definition was developed independently in 1923 by Johannes Brønstead and Thomas Lowry.\nThis web site will help you calculate your concentrations.\nhttp://www.saskschools.ca/~chem30_dev/5_acids_bases/acids2_3.htm
332944
The ability to be a proton donor is the Bronsted-Lowry definition of acids.  The Lewis definition of an acid is an electron pair acceptor, which covers molecules like BF3.  (Exactly what kind of chemistry do they teach at NIU?)\n\nThe ability to accept a pair of electrons is what is common to all acids, not the ability to be a proton donor.
925986
1. Bronsted-Lowry and Lewis\n\n2. Water pH=7 (neutral) neither acid nor base\n\n3. pH scale is the scale to determine the acidity or the basicity of a solution.\n\n4. Søren Peter Lauritz Sørensen, a Danish Biochemist.
713150
In the Brønsted-Lowry classification, any chemical species, ionic or molecular, capable of accepting or receiving a proton (hydrogen ion) from another substance. The other substance acts as an acid in giving up the proton. A substance may act as a base, then, only in the presence of an acid. The greater the tendency to accept a proton, the stronger the base. The hydroxyl ion acts as a strong base. Substances that ionize in aqueous solutions to produce the hydroxyl ion (OH), such as potassium hydroxide (KOH) and barium hydroxide [Ba(OH)2], are also conventionally called bases.\n\nAny compound having highly basic properties, strong acrid taste, and ability to neutralize acids. Aqueous solutions of alkalies are high in hydroxyl ions, have a pH above 7, and turn litmus paper from red to blue. Caustic alkalies include sodium hydroxide (caustic soda), the sixth-largest-volume chemical produced in the United States, and potassium hydroxide. They are extremely destructive to human tissue; external burns should be washed with large amounts of water. The milder alkalies are the carbonates of the alkali metals; these include the industrially important sodium carbonate (soda ash) and potassium carbonate (potash), as well as the carbonates of lithium, rubidium, and cesium, and the volatile ammonium hydroxide. Sodium bicarbonate is a still milder alkaline material.\n\nIn Summary base is a general word (carbonates, hydroxides ...of alkali metals, alkaline earth metals, Transition metals) and alkali is used specifically for carbonates, hydroxides... of alkali group metals.
320845
Having equal amounts of positive and negative charges.\n\nOr\n\nA mixture of equal acid and base with pH=7.00000
749204
acids are proton donors ^^ the guy above is dead wrong bases produce hydroxide ions, acids produce hydronium ions, but that depends on the solvent so ur answer is proton donors
684681
C because the solution is SATURATED with solute, meaning no more solute can be dissolved by the solvent in the solution.