Review Station Ideas
... Ammonia, NH3, is a weak base. Cabbage juice would turn _blue_ with NH3. NH3(aq) would be considered a _weak (strong | weak | non) electrolyte. In water, NH3 can be described by the equation: NH3(aq) + H2O(l) NH4+(aq) + OH Indicate one conjugate acid-base pair: _NH3_ and _NH4+__ (or H2O/OH–) NH3 f ...
... Ammonia, NH3, is a weak base. Cabbage juice would turn _blue_ with NH3. NH3(aq) would be considered a _weak (strong | weak | non) electrolyte. In water, NH3 can be described by the equation: NH3(aq) + H2O(l) NH4+(aq) + OH Indicate one conjugate acid-base pair: _NH3_ and _NH4+__ (or H2O/OH–) NH3 f ...
Multiple Choice Practice. A) P B) S C) Cl D) Li E) 1 F 1. Has the
... When the half reaction above is balanced, how many moles of electrons are needed for every mole of I2 formed by this half-reaction? A) 2 B) 6 C) 8 D) 10 E) 12 30. Which of the following is always true at the triple point of a pure substance? A) The vapor pressure of the solid phase equals the vapor ...
... When the half reaction above is balanced, how many moles of electrons are needed for every mole of I2 formed by this half-reaction? A) 2 B) 6 C) 8 D) 10 E) 12 30. Which of the following is always true at the triple point of a pure substance? A) The vapor pressure of the solid phase equals the vapor ...
Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions
... 1. Gravimetric Analysis – based on the measurement of mass (Section 4.6) 2. Titration - solution of known concentration is added to solution of unknown concentration until chemical reaction is complete (endpoint) ...
... 1. Gravimetric Analysis – based on the measurement of mass (Section 4.6) 2. Titration - solution of known concentration is added to solution of unknown concentration until chemical reaction is complete (endpoint) ...
Chemical Equilibrium – Le Chatelier`s Principle
... complete. If the color does not change, try another reagent. Remember to record all your results in your laboratory notebook. 3. Select a 6 M reagent which will cause the equilibrium to shift back and return the solution to its original color (that is, the color of methyl violet in water). Add it c ...
... complete. If the color does not change, try another reagent. Remember to record all your results in your laboratory notebook. 3. Select a 6 M reagent which will cause the equilibrium to shift back and return the solution to its original color (that is, the color of methyl violet in water). Add it c ...
Name ……………………………..………...… …….. Index No
... Name the type of polymerization these monomers would undergo to form a polymer.(1mk) ...
... Name the type of polymerization these monomers would undergo to form a polymer.(1mk) ...
pH and pOH (cont.)
... • The ion product constant for water, Kw, equals the product of the H+ ion concentration and the OH– ion concentration. Kw = [H+][OH–] • The pH of a solution is the negative log of the hydrogen ion concentration. The pOH is the negative log of the hydroxide ion concentration. pH plus pOH equals 14. ...
... • The ion product constant for water, Kw, equals the product of the H+ ion concentration and the OH– ion concentration. Kw = [H+][OH–] • The pH of a solution is the negative log of the hydrogen ion concentration. The pOH is the negative log of the hydroxide ion concentration. pH plus pOH equals 14. ...
Classwork – Nature, Properties, and Classification of Matter
... 3. Why are we able to multiply coefficients in a chemical equation? 4. Why must we multiply each coefficient by the same amount? 5. Explain why we must always balance a chemical equation. 6. Define “one mole.” 7. Show two ways to convey the balanced equation for the production of methanol from carbo ...
... 3. Why are we able to multiply coefficients in a chemical equation? 4. Why must we multiply each coefficient by the same amount? 5. Explain why we must always balance a chemical equation. 6. Define “one mole.” 7. Show two ways to convey the balanced equation for the production of methanol from carbo ...
Saturday Study Session 1 1st Class Reactions
... Answer the following questions that relate to chemical reactions. (a) Iron(III) oxide can be reduced with carbon monoxide according to the following equation. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) A 16.2 L sample of CO(g) at 1.50 atm and 200.°C is combined with 15.39 g of Fe2O3(s). (i) How many mo ...
... Answer the following questions that relate to chemical reactions. (a) Iron(III) oxide can be reduced with carbon monoxide according to the following equation. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) A 16.2 L sample of CO(g) at 1.50 atm and 200.°C is combined with 15.39 g of Fe2O3(s). (i) How many mo ...
Chemical Equilibrium Review Ch 13-14 2015
... Assume this reaction is initially at equilibrium and then predict any changes in direction that may occur based on the following adjustments to the environment. b) The pressure inside the container is doubled by the addition of helium gas. c) Carbon monoxide is removed from the container. d) The tem ...
... Assume this reaction is initially at equilibrium and then predict any changes in direction that may occur based on the following adjustments to the environment. b) The pressure inside the container is doubled by the addition of helium gas. c) Carbon monoxide is removed from the container. d) The tem ...
Writing Formulas
... Writing Ionic Formulas When writing the chemical formula for ionic compounds put the cation first followed by the anion and use subscripts to indicate the number of each ion present. Remember the algebraic sum of the ions' oxidation numbers must equal zero. (Balance) Learn the polyatomic ions. ...
... Writing Ionic Formulas When writing the chemical formula for ionic compounds put the cation first followed by the anion and use subscripts to indicate the number of each ion present. Remember the algebraic sum of the ions' oxidation numbers must equal zero. (Balance) Learn the polyatomic ions. ...
Practice MSL Multiple Choice 1. Compared to the charge and mass
... When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients? a. b. c. d. ...
... When this equation is completely balanced using the smallest whole numbers, what is the sum of the coefficients? a. b. c. d. ...
Name ______ Write formulas for the reactants and predicted
... A piece of nickel metal is immersed in a solution of copper(II) sulfate. Ni + Cu2+ ...
... A piece of nickel metal is immersed in a solution of copper(II) sulfate. Ni + Cu2+ ...
(p. 522)
... b. (p. 651) a. H3C—CH2—OH and H3C—O—CH3 c. alcohol and ether d. The alcohol will have the higher boiling point; it will have hydrogen bonding while the ether does not. 4. You are required to determine the energy of activation (Ea) of a reaction. Briefly describe the experimental measurements you wou ...
... b. (p. 651) a. H3C—CH2—OH and H3C—O—CH3 c. alcohol and ether d. The alcohol will have the higher boiling point; it will have hydrogen bonding while the ether does not. 4. You are required to determine the energy of activation (Ea) of a reaction. Briefly describe the experimental measurements you wou ...
Various Types of RXNS
... NOTE: Not all of the following chemical reactions are balanced. They have been intentionally left unbalanced for your practice. ...
... NOTE: Not all of the following chemical reactions are balanced. They have been intentionally left unbalanced for your practice. ...
chemistry basics note - bramalea2010-msmanning
... Water is probably the most ______________molecule on earth. Water makes up about _______ ________of your bodies mass. Water is composed of _________________________________________________. Hydrogen bonds form between water molecules and are difficult to break and are responsible for waters ...
... Water is probably the most ______________molecule on earth. Water makes up about _______ ________of your bodies mass. Water is composed of _________________________________________________. Hydrogen bonds form between water molecules and are difficult to break and are responsible for waters ...
PH
In chemistry, pH (/piːˈeɪtʃ/) is a numeric scale used to specify the acidity or alkalinity of an aqueous solution. It is the negative of the logarithm to base 10 of the activity of the hydrogen ion. Solutions with a pH less than 7 are acidic and solutions with a pH greater than 7 are alkaline or basic. Pure water is neutral, being neither an acid nor a base. Contrary to popular belief, the pH value can be less than 0 or greater than 14 for very strong acids and bases respectively.pH measurements are important in medicine, biology, chemistry, agriculture, forestry, food science, environmental science, oceanography, civil engineering, chemical engineering, nutrition, water treatment & water purification, and many other applications. The pH scale is traceable to a set of standard solutions whose pH is established by international agreement.Primary pH standard values are determined using a concentration cell with transference, by measuring the potential difference between a hydrogen electrode and a standard electrode such as the silver chloride electrode.The pH of aqueous solutions can be measured with a glass electrode and a pH meter, or indicator.pH is the negative of the logarithm to base 10 of the activity of the (solvated) hydronium ion, more often (albeit somewhat inaccurately) expressed as the measure of the hydronium ion concentration.The rest of this article uses the technically correct word ""base"" and its inflections in place of ""alkaline"", which specifically refers to a base dissolved in water, and its inflections.