AP Chemistry—Chapter 15: Applications of Aqueous Equilibria
... (b) Write the correctly balanced net ionic equation for the reaction that occurs when NaOCl is dissolved in water and calculate the numerical value of the equilibrium constant for the reaction. (c) Calculate the pH of a solution made by combining 40.0 milliliters of 0.14-molar HOCl and 10.0 millilit ...
... (b) Write the correctly balanced net ionic equation for the reaction that occurs when NaOCl is dissolved in water and calculate the numerical value of the equilibrium constant for the reaction. (c) Calculate the pH of a solution made by combining 40.0 milliliters of 0.14-molar HOCl and 10.0 millilit ...
Give reasons for the following: (i) Bond enthalpy of F2
... Bond enthalpy of F2 is lower than that of Cl2 because F atom is small in size and due to this the electron-electron repulsions between the lone pairs of F-F are very large. Thus, the bond dissociation energy of F2 is lower than that of Cl2. (ii) PH3 has lower boiling point than NH3 because NH3 molec ...
... Bond enthalpy of F2 is lower than that of Cl2 because F atom is small in size and due to this the electron-electron repulsions between the lone pairs of F-F are very large. Thus, the bond dissociation energy of F2 is lower than that of Cl2. (ii) PH3 has lower boiling point than NH3 because NH3 molec ...
1. (a) Propan-1ol, C2H5CH2OH can be oxidised to propanoic acid
... Benzocaine reacts with dilute acids to form the ion C9H12O2N+ and with ethanoyl chloride to form C11H13O3N. When benzocaine is heated under reflux with aqueous sodium hydroxide and the solution obtained is neutralised, two compounds X and Y are formed. X has a formula of C7H7O2N and is a solid ...
... Benzocaine reacts with dilute acids to form the ion C9H12O2N+ and with ethanoyl chloride to form C11H13O3N. When benzocaine is heated under reflux with aqueous sodium hydroxide and the solution obtained is neutralised, two compounds X and Y are formed. X has a formula of C7H7O2N and is a solid ...
GC-Final-Review-2014
... a. a solid that falls out of solution when two aqueous solutions are mixed together b. A solution that holds more solute that it theoretically hold at a given temp c. Amount of solute that dissolves in a solvent at a given temperature to produce a saturated solution d. Contains less solute that a sa ...
... a. a solid that falls out of solution when two aqueous solutions are mixed together b. A solution that holds more solute that it theoretically hold at a given temp c. Amount of solute that dissolves in a solvent at a given temperature to produce a saturated solution d. Contains less solute that a sa ...
study material class X (science)
... Ans. (a) marble chips react with dilute hydrochloric acid to form calcium chloride and carbon dioxide .it is a double displacement reaction CaCO3+2HCl CaCl2 + H2O +CO2 (b) Zinc granules react with dilute hydrochloric acid to give hydrogen gas. it is a displacement reaction Zn(s)+2HCl ZnCl2(aq)+H ...
... Ans. (a) marble chips react with dilute hydrochloric acid to form calcium chloride and carbon dioxide .it is a double displacement reaction CaCO3+2HCl CaCl2 + H2O +CO2 (b) Zinc granules react with dilute hydrochloric acid to give hydrogen gas. it is a displacement reaction Zn(s)+2HCl ZnCl2(aq)+H ...
Reactions in Aqueous Solution (Brown 13th-Fossum
... • The solvent is present in greatest abundance. • All other substances are solutes (they are dissolved in the solvent). Dissociation • When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them (dissociation). KCl(aq) = K+ (aq) + Cl- (aq) CuS ...
... • The solvent is present in greatest abundance. • All other substances are solutes (they are dissolved in the solvent). Dissociation • When an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them (dissociation). KCl(aq) = K+ (aq) + Cl- (aq) CuS ...
honors chem 6 day review packet
... Calculate the quantity of heat energy (to the nearest calorie) required to convert 50.0 g of ice at 0°C to steam at 110°C. Be sure to draw a diagram showing the temperature and phase changes and the heat energy increases. Specific heats: water = 1.00 cal/g·°C steam = 0.480 cal/g·°C ∆Hvap = 540 cal/g ...
... Calculate the quantity of heat energy (to the nearest calorie) required to convert 50.0 g of ice at 0°C to steam at 110°C. Be sure to draw a diagram showing the temperature and phase changes and the heat energy increases. Specific heats: water = 1.00 cal/g·°C steam = 0.480 cal/g·°C ∆Hvap = 540 cal/g ...
Acid + Base Class # 1
... 69. Hydronium ion: a theoretical model for acids, whereby the hydrogen ions become one with water and exists as H3O+1 ...
... 69. Hydronium ion: a theoretical model for acids, whereby the hydrogen ions become one with water and exists as H3O+1 ...
Single Replacement Reactions
... chemically combined in a compound. The tendency of a particular element to combine with other substances is a measure of the activity of the element. The more active an element is, the more likely it is to combine. In a single replacement reaction, an uncombined element replaces a less active elemen ...
... chemically combined in a compound. The tendency of a particular element to combine with other substances is a measure of the activity of the element. The more active an element is, the more likely it is to combine. In a single replacement reaction, an uncombined element replaces a less active elemen ...
summer fun - West Windsor-Plainsboro Regional School District
... The solubility of a solute is the amount that can be dissolved in a given quantity of solvent at a given temperature. For example, the solubility of lead (II) nitrate is 56 g/100 mL at 20oC. The solubilities of ionic solids in water vary over a wide range of values. For convenience, we divide compou ...
... The solubility of a solute is the amount that can be dissolved in a given quantity of solvent at a given temperature. For example, the solubility of lead (II) nitrate is 56 g/100 mL at 20oC. The solubilities of ionic solids in water vary over a wide range of values. For convenience, we divide compou ...
2012 Coaches Institute Presentation
... The percentage of acid molecules that ionize in water is another measure of the strength of an acid % Ionization = M(ionized acid) x ...
... The percentage of acid molecules that ionize in water is another measure of the strength of an acid % Ionization = M(ionized acid) x ...
Welcome to AP Chemistry! I am glad that you decided to take on the
... You need to memorize the general equations for the different types of reactions in the chemical equations review. The AP Chemistry Exam requires students to be able to write balanced net ionic chemical equations for several different sets of reactants Do not start on this packet except the ion list ...
... You need to memorize the general equations for the different types of reactions in the chemical equations review. The AP Chemistry Exam requires students to be able to write balanced net ionic chemical equations for several different sets of reactants Do not start on this packet except the ion list ...
2011 Chem Facts Key
... 35. Nonpolar covalent bonds form when two atoms of the same element bond together. 36. Polar covalent bonds form when the electronegativity difference between two bonding atoms is less than 1.7. 37. Hydrogen bonds are attractive forces that form when hydrogen bonds to the elements N, O, or F and giv ...
... 35. Nonpolar covalent bonds form when two atoms of the same element bond together. 36. Polar covalent bonds form when the electronegativity difference between two bonding atoms is less than 1.7. 37. Hydrogen bonds are attractive forces that form when hydrogen bonds to the elements N, O, or F and giv ...
Lewis Acids and Bases Hard and Soft Acid/Base Theory
... a complex. Lewis theory puts the emphasis on the donation and acceptance of electrons; this is appropriate, because it is the give and take of electrons (+ seeks – and avoids +) that drives all of chemistry. As we will see, there is often a change in stereochemistry at the acceptor atom when the add ...
... a complex. Lewis theory puts the emphasis on the donation and acceptance of electrons; this is appropriate, because it is the give and take of electrons (+ seeks – and avoids +) that drives all of chemistry. As we will see, there is often a change in stereochemistry at the acceptor atom when the add ...
A Review of High School Chemistry
... are strong acids and bases and which are weak acids and bases. Remember that something is defined as an acid or base in water ...
... are strong acids and bases and which are weak acids and bases. Remember that something is defined as an acid or base in water ...
Chapter 4: Chemical Reactions Elements can be characterized as
... Examples: SO2 – sulfur dioxide; SO3 – sulfur trioxide; As4O6 – tetraarsenic hexoxide Learn the common prefixes (pg. 142)- 2 (di), 3 (tri), 4(tetra), etc…. Binary acids HCl – Hydrogen chloride ...
... Examples: SO2 – sulfur dioxide; SO3 – sulfur trioxide; As4O6 – tetraarsenic hexoxide Learn the common prefixes (pg. 142)- 2 (di), 3 (tri), 4(tetra), etc…. Binary acids HCl – Hydrogen chloride ...
Ionic Bonding - petersonORHS
... electricity. Ions can move! • These solutions are called “Electrolytes” • Ionic compounds have very high melting points • When melted “molten” they conduct electricity. Ions can move! (melted salts are conductors) • Exist as crystals in a “crystal lattice.” ...
... electricity. Ions can move! • These solutions are called “Electrolytes” • Ionic compounds have very high melting points • When melted “molten” they conduct electricity. Ions can move! (melted salts are conductors) • Exist as crystals in a “crystal lattice.” ...
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.