Answers to 2017 Chemistry Exam Review Compounds and
... Or it can act as a base by accepting a proton: HCO3- + H2O = H2CO3 + OH- . (Notice that water is also amphoteric – acting as a base in the first example and an acid in the second.) 59. Kw = [H3O+][OH-] = 1.0 x 10-14 This is a very small number, meaning water rarely selfionizes. 60. [H+] = 1.0 x 10-1 ...
... Or it can act as a base by accepting a proton: HCO3- + H2O = H2CO3 + OH- . (Notice that water is also amphoteric – acting as a base in the first example and an acid in the second.) 59. Kw = [H3O+][OH-] = 1.0 x 10-14 This is a very small number, meaning water rarely selfionizes. 60. [H+] = 1.0 x 10-1 ...
Chapters 6, 8
... Noble gases are the only elements with a stable electronic configuration. All other elements have electronic configuration that is more or less unstable. To attain the electronic configuration of the closest noble gas, the element produces compounds. An element can produce a compound by: 1. Forming ...
... Noble gases are the only elements with a stable electronic configuration. All other elements have electronic configuration that is more or less unstable. To attain the electronic configuration of the closest noble gas, the element produces compounds. An element can produce a compound by: 1. Forming ...
Module 3 Exam Review 1. Organic chemistry is the study of which
... Module 3 Exam Review 1. Organic chemistry is the study of which element? carbon 2. The molecular formula for glucose, fructose and galactose is C6H12O6. Because they all have different molecular structures, they are _____. isomers 3. Carbon is unique because it can form a wide variety of compounds. ...
... Module 3 Exam Review 1. Organic chemistry is the study of which element? carbon 2. The molecular formula for glucose, fructose and galactose is C6H12O6. Because they all have different molecular structures, they are _____. isomers 3. Carbon is unique because it can form a wide variety of compounds. ...
4 • Reactions In Aqueous Solution
... Which of the following is incorrect? a) all salts containing NH4+ are soluble. b) all salts containing NO3– are soluble. c) all fluorides are soluble. d) all sulfates (except those of Ca2+, Sr2+, Ba2+, and Pb2+) are soluble. e) most hydroxides are insoluble, except those of Ca2+, Sr2+, Ba2+, the alk ...
... Which of the following is incorrect? a) all salts containing NH4+ are soluble. b) all salts containing NO3– are soluble. c) all fluorides are soluble. d) all sulfates (except those of Ca2+, Sr2+, Ba2+, and Pb2+) are soluble. e) most hydroxides are insoluble, except those of Ca2+, Sr2+, Ba2+, the alk ...
Chapter 4 - Colby College Wiki
... concentration. If it takes 17.8 mL of the potassium hydroxide solution to turn the indicator (phenolphthalein) slightly pink, what is the concentration of the hydrobromic acid solution? • The above process is known as a titration – the careful addition of one solution to another until one component ...
... concentration. If it takes 17.8 mL of the potassium hydroxide solution to turn the indicator (phenolphthalein) slightly pink, what is the concentration of the hydrobromic acid solution? • The above process is known as a titration – the careful addition of one solution to another until one component ...
1A - The changing atom History of the atom • The model of the atom
... The ions in a chemical formula must add up to zero. Use subscripts after an ion in a formula to double/triple that ion so the sum=0. eg. CuCl 2 If you are double/tripling ions that consist of more than one element brackets must be used. eg. Ca(OH)2 If Roman numeral numbers follow a metal ion in brac ...
... The ions in a chemical formula must add up to zero. Use subscripts after an ion in a formula to double/triple that ion so the sum=0. eg. CuCl 2 If you are double/tripling ions that consist of more than one element brackets must be used. eg. Ca(OH)2 If Roman numeral numbers follow a metal ion in brac ...
Acid Base Equilibria
... dissociates. These hydroxides are not very soluble, but what amount that does dissolve completely dissociates into ions. Example: Ba (OH)2(aq) → Ba2+(aq) + 2OH-(aq) A 0.000100 M Ba(OH)2 solution will be 0.000200 M in OH- ions (as well as 0.000100 M in Ba2+ ions) and will have a pH of 10.3. Weak Base ...
... dissociates. These hydroxides are not very soluble, but what amount that does dissolve completely dissociates into ions. Example: Ba (OH)2(aq) → Ba2+(aq) + 2OH-(aq) A 0.000100 M Ba(OH)2 solution will be 0.000200 M in OH- ions (as well as 0.000100 M in Ba2+ ions) and will have a pH of 10.3. Weak Base ...
CVB101 – Lecture 3 Chemical Bonding • Chemical bonding
... o It is possible to make very concentrated solutions on NaCl Other compounds are not very soluble e.g. AgCl o If AgCl solid is placed in water, only very small amount will dissolve. The rest stays as a solid Saturated solution – a solution in which no more solute will be dissolved Ionic Equation ...
... o It is possible to make very concentrated solutions on NaCl Other compounds are not very soluble e.g. AgCl o If AgCl solid is placed in water, only very small amount will dissolve. The rest stays as a solid Saturated solution – a solution in which no more solute will be dissolved Ionic Equation ...
acids, bases and solution equilibria
... A more complete understanding of how species act as acids or bases requires greater knowledge of molecular orbital theory, but we will touch upon some examples here. -acceptor ligands (-acids) CO, CN, O2. Ligands such as these use their anti-bonding -orbitals as acceptor orbitals. ...
... A more complete understanding of how species act as acids or bases requires greater knowledge of molecular orbital theory, but we will touch upon some examples here. -acceptor ligands (-acids) CO, CN, O2. Ligands such as these use their anti-bonding -orbitals as acceptor orbitals. ...
Chap. 4 - Chemical Reactions
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
Chemical Equation Reactions
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
... In the previous single replacement reaction example, we have written the molecular equation for the reaction. Although this equation shows the reactants and products of the reaction, it does not give a very clear picture of what truly occurs in solution. In fact, such an aqueous solution actually co ...
Untitled
... Place 50 green beads in the plastic box. Simulate a collision by choosing two beads. Then apply the following rules: a. If both beads are green, remove them and replace with one red and one blue b. If one is red and the other blue, remove them and replace with 2 green c. If the beads are any other c ...
... Place 50 green beads in the plastic box. Simulate a collision by choosing two beads. Then apply the following rules: a. If both beads are green, remove them and replace with one red and one blue b. If one is red and the other blue, remove them and replace with 2 green c. If the beads are any other c ...
IPC Semester Exam Review – Chemistry Topics
... Jose measured out 1 quart of distilled water and added to it 2 tablespoons of salt. He then brought the water to a boil and measured its maximum temperature. Jose ran two more trials using 2 tablespoons of salt. He then ran 3 trials each with 4 tablespoons of salt and 6 tablespoon of salt. For each ...
... Jose measured out 1 quart of distilled water and added to it 2 tablespoons of salt. He then brought the water to a boil and measured its maximum temperature. Jose ran two more trials using 2 tablespoons of salt. He then ran 3 trials each with 4 tablespoons of salt and 6 tablespoon of salt. For each ...
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.