Chapter 10 - U of L Class Index
... When a base accepts a proton, it is said to be ____________________. When an acid gives up a proton, it is said to be ____________________. The Arrhenius definition of acids and bases is almost identical to the Brønsted-Lowry definition. The only difference is that it looks at their behaviour in wat ...
... When a base accepts a proton, it is said to be ____________________. When an acid gives up a proton, it is said to be ____________________. The Arrhenius definition of acids and bases is almost identical to the Brønsted-Lowry definition. The only difference is that it looks at their behaviour in wat ...
Chemistry II Exams and Keys 2013 Season
... Answer the following questions on the answer sheet provided. Each correct response is worth 4 points. Use the letters in parentheses for your answers. Choose the letter that best completes or answers the item. Be certain that erasures are complete. Please PRINT your name, school area code, and which ...
... Answer the following questions on the answer sheet provided. Each correct response is worth 4 points. Use the letters in parentheses for your answers. Choose the letter that best completes or answers the item. Be certain that erasures are complete. Please PRINT your name, school area code, and which ...
AP syllabus
... 2. Kinetic theory of ideal gases 3. Pressure units and conversions between units 4. Solving problems using Dalton’s Law of Partial Pressures 5. Solving problems using Boyle’s, Charles’, Gay-Lussac’s and combined gas laws 6. Solving gas law problems when the gas is collected over water 7. Solving pro ...
... 2. Kinetic theory of ideal gases 3. Pressure units and conversions between units 4. Solving problems using Dalton’s Law of Partial Pressures 5. Solving problems using Boyle’s, Charles’, Gay-Lussac’s and combined gas laws 6. Solving gas law problems when the gas is collected over water 7. Solving pro ...
View - University of Southampton
... becomes an actiVe solvent. Here, the interactions between solute and solvent molecules are very strong, and complex formation can result. Thus, a number of solvent molecules will take on an active role in any chemical reaction. To calculate the properties of such systems then requires the use of sup ...
... becomes an actiVe solvent. Here, the interactions between solute and solvent molecules are very strong, and complex formation can result. Thus, a number of solvent molecules will take on an active role in any chemical reaction. To calculate the properties of such systems then requires the use of sup ...
Chromatography and Instrumentation
... phase and mobile phase, the components of the mixture which have a better affinity with the mobile phase will move more easily with the water than those that have a better affinity with the stationary phase ...
... phase and mobile phase, the components of the mixture which have a better affinity with the mobile phase will move more easily with the water than those that have a better affinity with the stationary phase ...
VCAA Study Design - Chemistry Education Association
... • difficulty in using the electrochemical series to predict possible redox reactions • lack of awareness of the differences between discharging and recharging in terms of the direction of electron flow, and that electrons always move from the site of oxidation (anode) to the site of reduction (catho ...
... • difficulty in using the electrochemical series to predict possible redox reactions • lack of awareness of the differences between discharging and recharging in terms of the direction of electron flow, and that electrons always move from the site of oxidation (anode) to the site of reduction (catho ...
Honors Chemistry I
... i. This is an EXOTHERMIC reaction because it releases energy as heat c. Example: N2O4 + ENERGY 2NO2 i. This is an ENDOTHERMIC reaction because energy must be absorbed by N2O4 in order to form NO2 2) Molecules and atoms must come into contact for them to chemically react. a. As an example: A match ...
... i. This is an EXOTHERMIC reaction because it releases energy as heat c. Example: N2O4 + ENERGY 2NO2 i. This is an ENDOTHERMIC reaction because energy must be absorbed by N2O4 in order to form NO2 2) Molecules and atoms must come into contact for them to chemically react. a. As an example: A match ...
Section 4.8: Acid-Base Reactions
... Once a solution is standardized, it may be used as a secondary standard for determining the concentration of other solutions with which it reacts. For example, KHP (potassium hydrogen phthalate) is a solid primary standard used to standardize sodium hydroxide (NaOH) solutions. A standardized NaOH so ...
... Once a solution is standardized, it may be used as a secondary standard for determining the concentration of other solutions with which it reacts. For example, KHP (potassium hydrogen phthalate) is a solid primary standard used to standardize sodium hydroxide (NaOH) solutions. A standardized NaOH so ...
Expt 3-2 Freezing Point Depression
... After the Arrhenius theory of ionization of salts in aqueous solutions became accepted, comparisons were made of experimental values of colligative properties (ΔTF, osmotic pressure, etc) of aqueous salt solutions with the values expected if the salts were completely dissoc ...
... After the Arrhenius theory of ionization of salts in aqueous solutions became accepted, comparisons were made of experimental values of colligative properties (ΔTF, osmotic pressure, etc) of aqueous salt solutions with the values expected if the salts were completely dissoc ...
Electrochemistry
... Cell Potentials and Free-Energy Changes for Cell Reactions Electromotive Force (emf): The force (or electrical potential) that pushes the negatively charged electrons away from the anode (– electrode) and pulls them toward the cathode (+ electrode). ...
... Cell Potentials and Free-Energy Changes for Cell Reactions Electromotive Force (emf): The force (or electrical potential) that pushes the negatively charged electrons away from the anode (– electrode) and pulls them toward the cathode (+ electrode). ...
Solutions Powerpoint
... A saline solution is a solution of salt and water. The solute is salt. The solvent is water. A dilute solution is a solution with little solute. A concentrated solution is a solution with a lot of solute. ...
... A saline solution is a solution of salt and water. The solute is salt. The solvent is water. A dilute solution is a solution with little solute. A concentrated solution is a solution with a lot of solute. ...
ANALYSIS OF THE SILVER GROUP CATIONS
... a large number of ions, the usual approach is to use a chemical method to separate the mixture into subgroups that consist of just a few ions. Then it may be possible to test for one particular ion in the presence of just one or two others. Alternatively, each subgroup of just a few ions may be sepa ...
... a large number of ions, the usual approach is to use a chemical method to separate the mixture into subgroups that consist of just a few ions. Then it may be possible to test for one particular ion in the presence of just one or two others. Alternatively, each subgroup of just a few ions may be sepa ...
Topic 8-Solubility-Modified
... the molar heat of fusion (ΔHf).The molar heat of fusion is the amount of heat absorbed when the solid melts. An ideal solution is one which the heat of solution is equal to the heat of fusion. The equation to explain the fact that temperature, melting point, and molar heat of fusion effect the solub ...
... the molar heat of fusion (ΔHf).The molar heat of fusion is the amount of heat absorbed when the solid melts. An ideal solution is one which the heat of solution is equal to the heat of fusion. The equation to explain the fact that temperature, melting point, and molar heat of fusion effect the solub ...
Ionic strength effect on the deprotonation of para
... considering the well-known Specific Ion Interaction Theory (SIT).15–19 In the original SIT model, the activity coefficient of ion i with charge zi in a solution of ionic strength I (on the molal scale) at 25 °C can be expressed by the equation: ...
... considering the well-known Specific Ion Interaction Theory (SIT).15–19 In the original SIT model, the activity coefficient of ion i with charge zi in a solution of ionic strength I (on the molal scale) at 25 °C can be expressed by the equation: ...
Equilibrium chemistry
Equilibrium chemistry is a concerned with systems in chemical equilibrium. The unifying principle is that the free energy of a system at equilibrium is the minimum possible, so that the slope of the free energy with respect to the reaction coordinate is zero. This principle, applied to mixtures at equilibrium provides a definition of an equilibrium constant. Applications include acid-base, host-guest, metal-complex, solubility, partition, chromatography and redox equilibria.