Study Notes
... Ex. Is mass conserved in the following chemical reactions? 2Na + Cl2 è 2NaCl Yes or No H2O + CO2è C6H12O6 + O2 Yes or No Catalyst : ...
... Ex. Is mass conserved in the following chemical reactions? 2Na + Cl2 è 2NaCl Yes or No H2O + CO2è C6H12O6 + O2 Yes or No Catalyst : ...
H 2 SO 4
... proposed a more broad definition. Their definition does not require that an acid be in an aqueous solution and includes more than just protons and hydroxide ions for acids and bases. ...
... proposed a more broad definition. Their definition does not require that an acid be in an aqueous solution and includes more than just protons and hydroxide ions for acids and bases. ...
Part1. Acid rain formation. 1. Discovery of acid rain.
... Nitric acid is more volatile and thus can exist in significant concentrations in the gas phase, while sulfuric acid has a very low vapor pressure under ambient conditions and hence exists in the form of particles. Nitric acid can relatively easily revolatilize even after forming the ammonium sal ...
... Nitric acid is more volatile and thus can exist in significant concentrations in the gas phase, while sulfuric acid has a very low vapor pressure under ambient conditions and hence exists in the form of particles. Nitric acid can relatively easily revolatilize even after forming the ammonium sal ...
Acids and Bases - Hobbs High School
... NH3 + H2O ↔ NH4+ + OH• This eqilibrium reaction is reversible, and at any one time about 99% of the ammonia is still present as ammonia molecules. Only about 1% has actually produced hydroxide ions. ...
... NH3 + H2O ↔ NH4+ + OH• This eqilibrium reaction is reversible, and at any one time about 99% of the ammonia is still present as ammonia molecules. Only about 1% has actually produced hydroxide ions. ...
Gas-forming Reactions
... Loss of the first hydrogen ion is virtually complete. So sulfuric acid is classified as strong. The second hydrogen is more difficult to remove and the bisulfate ion is only partially ionized. The bisulfate ion is a weak acid. A base is a substance that increases the concentration of aqueous OH– ion ...
... Loss of the first hydrogen ion is virtually complete. So sulfuric acid is classified as strong. The second hydrogen is more difficult to remove and the bisulfate ion is only partially ionized. The bisulfate ion is a weak acid. A base is a substance that increases the concentration of aqueous OH– ion ...
Word Pro
... leaving a residue of sodium carbonate. (h) Potassium chlorate is heated strongly with a catalyst to produce oxygen gas. (i) P4O10(s) react and dissolves in water to give a solution that turns blue litmus paper red. (j) Strontium oxide dissolves in water to give a solution that turns red litmus paper ...
... leaving a residue of sodium carbonate. (h) Potassium chlorate is heated strongly with a catalyst to produce oxygen gas. (i) P4O10(s) react and dissolves in water to give a solution that turns blue litmus paper red. (j) Strontium oxide dissolves in water to give a solution that turns red litmus paper ...
Incompatible Chemicals
... Acids – dissolves in water and gives solution hydrogen ion activity EXTREMELY STRONG ACIDS Fluoroantimonic acid (HSbF6) Magic Acid (FSO3HSbF5) Carborane superacid H(CHB11Cl11) Fluorosulfuric acid (FSO3H) Triflic acid (CF3SO3H) STRONG ACIDS (strongest to weakest) Perchloric acid (HClO4) Hydroiodic ac ...
... Acids – dissolves in water and gives solution hydrogen ion activity EXTREMELY STRONG ACIDS Fluoroantimonic acid (HSbF6) Magic Acid (FSO3HSbF5) Carborane superacid H(CHB11Cl11) Fluorosulfuric acid (FSO3H) Triflic acid (CF3SO3H) STRONG ACIDS (strongest to weakest) Perchloric acid (HClO4) Hydroiodic ac ...
The pH Scale…
... pH is the scale that tells you whether a substance is acidic, basic, or neutral. pH=“p” stands for power and “H” stands for hydrogen. The values correspond to the concentration of the hydronium ions. ...
... pH is the scale that tells you whether a substance is acidic, basic, or neutral. pH=“p” stands for power and “H” stands for hydrogen. The values correspond to the concentration of the hydronium ions. ...
File
... 2. The first element in the formula is named first, using the full element name. 3. The second element is named using the suffix ‘-ide.’ 4. Prefixes are used to denote the numbers of atoms present. See table below for prefixes. 5. The prefix ‘mono-’ is only used to name the second element. example: ...
... 2. The first element in the formula is named first, using the full element name. 3. The second element is named using the suffix ‘-ide.’ 4. Prefixes are used to denote the numbers of atoms present. See table below for prefixes. 5. The prefix ‘mono-’ is only used to name the second element. example: ...
Oregon State University, Summer 2009 Chemistry 121 Midterm
... Fill in the front page of the Scantron answer sheet with your last name, first name, middle initial, and student identification number. Leave the class section number and the test form number blank. This exam consists of 20 multiple-choice questions. Each multiple-choice question has 5 points associ ...
... Fill in the front page of the Scantron answer sheet with your last name, first name, middle initial, and student identification number. Leave the class section number and the test form number blank. This exam consists of 20 multiple-choice questions. Each multiple-choice question has 5 points associ ...
Chemical Reactions: Introduction to Reaction Types
... In a decomposition reaction, a compound is broken down into two or more substances. In general, decomposition reactions occur when a solid compound is heated. This type of reaction almost always produces a gas. The following are examples of decomposition reactions: Heating mercury (II) oxide produce ...
... In a decomposition reaction, a compound is broken down into two or more substances. In general, decomposition reactions occur when a solid compound is heated. This type of reaction almost always produces a gas. The following are examples of decomposition reactions: Heating mercury (II) oxide produce ...
SAMPLE PAPER -2 Time Allowed: 3 Hrs
... effect and withdraws electrons from the carbon of the carboxyl group as well as from the oxygen of the O-H bond. This decreases electron density at the oxygen atom of the O-H bond. Consequently, the O-H bond gets weakened and the release of H+ ion is favored. Moreover, the negative charge present on ...
... effect and withdraws electrons from the carbon of the carboxyl group as well as from the oxygen of the O-H bond. This decreases electron density at the oxygen atom of the O-H bond. Consequently, the O-H bond gets weakened and the release of H+ ion is favored. Moreover, the negative charge present on ...
- Palisades School District
... 1. Consider a sample of calcium carbonate in the form of a cube measuring 2.005 in. on each edge. If the sample has a density of 2.71 g/cm3, how many oxygen atoms does it contain? 2. If an automobile travels 225 miles with a gas mileage of 20.5 miles/gallon, how many kg of CO2 are produced, assuming ...
... 1. Consider a sample of calcium carbonate in the form of a cube measuring 2.005 in. on each edge. If the sample has a density of 2.71 g/cm3, how many oxygen atoms does it contain? 2. If an automobile travels 225 miles with a gas mileage of 20.5 miles/gallon, how many kg of CO2 are produced, assuming ...
KUT 101/2 – General Chemistry Practical I
... dissociation constant and molarity of unknown acid • Preparation of Ag2CrO4 salt • Measurement of absorbance using spectrophotometer • Obtaining a calibration curve ...
... dissociation constant and molarity of unknown acid • Preparation of Ag2CrO4 salt • Measurement of absorbance using spectrophotometer • Obtaining a calibration curve ...
Unit 12 Worksheet Answers
... 42. Given the reaction 2Al + 3FeO Al 2 O 3 + 3Fe; what is the mole to mole ratio between iron (II) oxide and aluminum oxide? a. ...
... 42. Given the reaction 2Al + 3FeO Al 2 O 3 + 3Fe; what is the mole to mole ratio between iron (II) oxide and aluminum oxide? a. ...
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.