Exam Review – Part 1
... • For a chemical equation to be completely accurate, it must follow the law of conservation of mass. • Based on the Law of Conservation of ...
... • For a chemical equation to be completely accurate, it must follow the law of conservation of mass. • Based on the Law of Conservation of ...
The Buffer Equation
... semipermeable membrane. This process tends to equalize the escaping tendency of the solvent on both sides of the membrane. Escaping tendency can be measured in terms of vapor pressure or the closely related colligative property osmotic pressure. Osmosis in some cases is believed to involve the passa ...
... semipermeable membrane. This process tends to equalize the escaping tendency of the solvent on both sides of the membrane. Escaping tendency can be measured in terms of vapor pressure or the closely related colligative property osmotic pressure. Osmosis in some cases is believed to involve the passa ...
Acids, bases and ions in aqueous solution
... significance in terms of acidic behaviour in aqueous solution. Each of the hydrogen halides is monobasic: for X =Cl, Br and I, the equilibrium lies far to the right-hand side, making these strong acids ( Ka > 1 ↔ pKa = - log(Ka) < 0 ). ...
... significance in terms of acidic behaviour in aqueous solution. Each of the hydrogen halides is monobasic: for X =Cl, Br and I, the equilibrium lies far to the right-hand side, making these strong acids ( Ka > 1 ↔ pKa = - log(Ka) < 0 ). ...
Document
... Group 3A elements, such as BF3 and AlCl3, are Lewis acids because they have unfilled valence orbitals and can accept electron pairs from Lewis bases Transition-metal compounds, such as TiCl4, FeCl3, ZnCl2, and SnCl4, are Lewis acids Organic compounds that undergo addition reactions with Lewis bases ...
... Group 3A elements, such as BF3 and AlCl3, are Lewis acids because they have unfilled valence orbitals and can accept electron pairs from Lewis bases Transition-metal compounds, such as TiCl4, FeCl3, ZnCl2, and SnCl4, are Lewis acids Organic compounds that undergo addition reactions with Lewis bases ...
2. In aqueous solution, sodium hydroxide is a strong base and
... 6. 2 H2O (l) ↔ H3O+ (aq) + OH – (aq) The equilibrium constant for the reaction above is 1.0 x 10‐14 at 25°C and 2.1 x 10‐14 at 35°C. What can be deduced from this information? A. [H3O+] decreases as the temperature is raised B. [H3O+] is greater than [OH‐] at 35°C C. Water is a stronger electrolyte ...
... 6. 2 H2O (l) ↔ H3O+ (aq) + OH – (aq) The equilibrium constant for the reaction above is 1.0 x 10‐14 at 25°C and 2.1 x 10‐14 at 35°C. What can be deduced from this information? A. [H3O+] decreases as the temperature is raised B. [H3O+] is greater than [OH‐] at 35°C C. Water is a stronger electrolyte ...
BH - hrsbstaff.ednet.ns.ca
... forms a hydronium ion (H3O) when mixed with. A strong acid will be 100% ionized when dissolved. If not, it is then called a weak acid. A base is a substance that will form a hydroxide ion when dissolved in water. To form a hydroxide ion molecular bases undergo ...
... forms a hydronium ion (H3O) when mixed with. A strong acid will be 100% ionized when dissolved. If not, it is then called a weak acid. A base is a substance that will form a hydroxide ion when dissolved in water. To form a hydroxide ion molecular bases undergo ...
Chapter 2: Aqueous Soln` H
... Lewis: (aqueous & non-aqueous soln’) Acid: substance accept electron pair Base: substance donate electron pair The Lewis definition encompasses the Bronsted-Lowry definition: In the reaction of H+ and OH-, H+ is a Lewis acid because it accepts an electron pair from the OH-. Since the OH- donates an ...
... Lewis: (aqueous & non-aqueous soln’) Acid: substance accept electron pair Base: substance donate electron pair The Lewis definition encompasses the Bronsted-Lowry definition: In the reaction of H+ and OH-, H+ is a Lewis acid because it accepts an electron pair from the OH-. Since the OH- donates an ...
Chapter 2 – Chemical Composition of the Body
... • These hydrogen bonds are very important because they alter the physical and chemical properties of many molecules (especially water).. ...
... • These hydrogen bonds are very important because they alter the physical and chemical properties of many molecules (especially water).. ...
Acids and Bases
... It is useful to specify the amount of weak acid that has dissociated in achieving equilibrium in an aqueous solution. The percent dissociation is defined as follows: amount dissociated ( M ) % dissociation ...
... It is useful to specify the amount of weak acid that has dissociated in achieving equilibrium in an aqueous solution. The percent dissociation is defined as follows: amount dissociated ( M ) % dissociation ...
Weak Acids and Bases Practice -- Chemistry 121A
... yield. It runs from 0% (all reactants) to 100% (all products). This is simply more convenient than Q, which runs from 0 to infinity. The way I look at it is this for a weak acid: %ionization = [A−]eq/[HA]o x 100% That is, the “final” concentration of A− at equilibrium divided by the “initial” concen ...
... yield. It runs from 0% (all reactants) to 100% (all products). This is simply more convenient than Q, which runs from 0 to infinity. The way I look at it is this for a weak acid: %ionization = [A−]eq/[HA]o x 100% That is, the “final” concentration of A− at equilibrium divided by the “initial” concen ...
Chapter 4
... • STRONG electrolytes: solutions that conduct electric current very efficiently • WEAK electrolytes: solutions that conduct a small electric current • NONelectrolytes: solutions that permit no current flow ...
... • STRONG electrolytes: solutions that conduct electric current very efficiently • WEAK electrolytes: solutions that conduct a small electric current • NONelectrolytes: solutions that permit no current flow ...
material safety data sheet
... MATERIAL SAFETY DATA SHEET I - IDENTIFICATION AND USE PRODUCT NAME: FLO-CLENE PRODUCT USE: LIQUID DRAIN OPENER SUPPLIER: ...
... MATERIAL SAFETY DATA SHEET I - IDENTIFICATION AND USE PRODUCT NAME: FLO-CLENE PRODUCT USE: LIQUID DRAIN OPENER SUPPLIER: ...
Title - Iowa State University
... 3) The end point for an acid-base titration is called: a) Equivalence point b) Static point c) acid point d) none of these 4) Which of the following is a strong electrolyte? a) CH3OH b) HCOOH c)KNO3 d) all of these 5) Which of the following would be insoluble? a) CaS b) KOH c) Pb(NO3)2 d) SrSO4 e)bo ...
... 3) The end point for an acid-base titration is called: a) Equivalence point b) Static point c) acid point d) none of these 4) Which of the following is a strong electrolyte? a) CH3OH b) HCOOH c)KNO3 d) all of these 5) Which of the following would be insoluble? a) CaS b) KOH c) Pb(NO3)2 d) SrSO4 e)bo ...
Lesson 4.4 acid base reactions
... Another simple property of acids and bases is their ability to cause color changes in certain dyes. An acid-base indicator is a dye used to distinguish between acidic and basic solutions by means of the color changes it undergoes in these solutions. Such dyes are common in natural materials. For ex ...
... Another simple property of acids and bases is their ability to cause color changes in certain dyes. An acid-base indicator is a dye used to distinguish between acidic and basic solutions by means of the color changes it undergoes in these solutions. Such dyes are common in natural materials. For ex ...
Acid
An acid (from the Latin acidus/acēre meaning sour) is a chemical substance whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals (like calcium) to form salts. Aqueous solutions of acids have a pH of less than 7. Non-aqueous acids are usually formed when an anion (negative ion) reacts with one or more positively charged hydrogen cations. A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.There are three common definitions for acids: the Arrhenius definition, the Brønsted-Lowry definition, and the Lewis definition. The Arrhenius definition defines acids as substances which increase the concentration of hydrogen ions (H+), or more accurately, hydronium ions (H3O+), when dissolved in water. The Brønsted-Lowry definition is an expansion: an acid is a substance which can act as a proton donor. By this definition, any compound which can easily be deprotonated can be considered an acid. Examples include alcohols and amines which contain O-H or N-H fragments. A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond. Examples of Lewis acids include all metal cations, and electron-deficient molecules such as boron trifluoride and aluminium trichloride.Common examples of acids include hydrochloric acid (a solution of hydrogen chloride which is found in gastric acid in the stomach and activates digestive enzymes), acetic acid (vinegar is a dilute solution of this liquid), sulfuric acid (used in car batteries), and tartaric acid (a solid used in baking). As these examples show, acids can be solutions or pure substances, and can be derived from solids, liquids, or gases. Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.