Solutions
Kinetics
Equilibrium/LeChateliers Principle
Strong Acids & Bases
Weak Acids & Bases/Titrations
100
A homogenous mixture of a solute dissolved in a solvent
What is a solution
100
The series of steps by which an overall chemical reaction takes place is called?
What is Reaction Mechanism
100
Reactions that are reversible, that is they proceed in both directions.
What is an Equilibrium Reaction.
100
Acids give away H+, Bases accept H+ from acid
What is the Bronsted Lowry Theory of Acids and Bases
100
They do not dissociate 100%, they only partially dissociate or ionize in solution.
What is Weak Acids and Bases.
200
An intermolecular force that occurs in molecules that have dipoles (differing electronegativity's).
What is a Dipole-Dipole Force.
200
As the concentration increases, the number of particles increases. More particles result in a greater chance of the particles colliding. Therefore more collisions means a higher rate of reaction.
What is the reason that the rate of a chemical reaction increases as the concentration of the reactants increases?
200
What explains what happens when a change happens (a stress is applied) to a reaction already at equilibrium
What is LeChateliers Principle
200
What are these: 1) The theory cannot explain the basic properties of NH3. 2) H^+ will always be attracted to the oxygen ions in a water molecule and they interact with the hydronium ions that don't exist independently. 3) Doesn't predict an acid or base correctly all the time. 4) Theory assumes that water is always there but its not there all the time, need to have it for the theory to be true.
What is the 4 limitations of Arrhenius Theory.
200
An experimental method used to determine the concentration of substances, usually acids and bases.
What is a Titration.
300
Salt is an electrolyte and can conduct electricity when dissolved in water, and Sugar is a non-electrolyte so it dissolves and cannot conduct electricity.
What is the reason as to why a salt solution can conduct electricity but a sugar solution cannot
300
The amount of energy required to activate atoms or molecules to a state in which they can undergo a chemical reaction.
What is Activation Energy.
300
1)For concentration what direction shows that its increasing 2)For concentration what direction shows that its decreasing
What is 1) shifts up and goes away 2) shifts down and goes towards
300
Two molecules or ions that are related by the transfer of a proton (H+) are called conjugate acid base pairs. Show example of the conjugate acid base pairs.
What is HCl(aq) + H2O(l) <---> H3O^+(aq) + Cl^-(aq) Acid Base Conj. Acid Conj. Base
300
Write an dissociation equation for HBr and HC2H3O2.
What is -HBr(aq) + H2O(l) --> Br^-(aq) + H3O^+ (aq) -HC2H3O2(aq) + H2O(l) <--> C2H3O2^-(aq) + H3O^+(aq)
400
The Net Ionic Equation for 2Na^1+(aq) + SO4^2-(aq) + Ba^2+(aq) + 2Cl^1-(aq) ---> 2Na^1+(aq) + 2Cl^1-(aq) + BaSo4(s) is?
What is Ba^2+(aq) + SO4^2-(aq) ---> BaSO4(s)
400
1)Increasing Temperature, results in increasing rates for what kind of reaction? 2)Decreasing Temperature, results in increasing rates for what kind of reaction?
What is 1) Endothermic, 2)Exothermic.
400
A 4.00L reaction vessel contained 0.140mol of H2, 0.300mol of Br2, and 0.357mol of HBr. Assuming that the substances are already at equilibrium, write an equilibrium constant expression and find the value of Kc. H2(g) + Br2(g) <---> 2HBr(g)
What is H2= 0.140mol =0.035M Kc=[HBr]^2 ------------ ---------- 4.00 [H2][Br2] Br2=0.300mol =0.075M Kc =(0.089)^2 ------------ ------------ 4.00L (0.035)(0.075) HBr=0.357mol =0.089M Kc= 3.02 ------------ 4.00L
400
Which ones a property of an Acid and Base: 1) -Electrolytes 2) -Electrolytes -pH < 7 -pH > 7 -Turns blue litmus paper red -Turns red litmus paper blue -Tastes sour -Tastes bitter
What is 1)Acid, 2)Base
400
C7H7NH2(aq) has an initial concentration of 0.25M and pH of 11.38. What is the Kb value? C7H7NH2(aq) + H2O(l) <---> C7H7NH3^+(aq) + OH^-(aq)
What is C7H7NH2 H2O C7H7NH3 OH ________________________________________ I 0.25M / 0 0 ________________________________________ C -x / +x +x _________________________________________ E 0.25-x / x x Kb= (x)(x) pOH=14-11.38=2.62 ______ 0.25 [OH]=10^(-2.62)= Kb=(2.4x10^(-3))^2 _______________ 2.4x10^(-3) (0.25-2.4x10^(-3) Kb= 2.3x10^(-5)
500
Solve: what's the volume of concentrated hydrochloric acid, containing 11.9M hydrogen chloride, that is needed in an experiment that requires 2.00L of 0.200M hydrochloric acid solution?
What is (C1)(V1) = (C2)(V2) (11.9M)(V1) = (0.200M)(2.00L) V1= (0.200M)(2.00L) ______________ (11.9M) V1= 0.034L
500
The overall reaction described by this mechanism is: Step 1: H^(+) + H2O2 ---> H3O2^(+) (Fast) Step 2: H3O2^(+) + I^(-) ---> H2O + HOI (Slow) _____________________________ Overall:
What is H^(+) + H2O2 + I^(-) ---> H2O + HOI
500
When 1.00 mol of CO and 3.00mol of H2 are placed in a 10.00L vessel and allowed to come to equilibrium, the mixture is found to contain 0.387mol of H2O. How many moles of each substance are present at Equilibrium? CO(g) + 3H2(g) <--> CH4 + H2O
What is CO H2 CH4 H2O ------------------------------------------------- I 1.00mol 3.00mol 0 0 ------------------------------------------------- C -x -3x +x +x ------------------------------------------------- E 1.00-x 3.00-3x x x ------------------------------------------------- 1.0-(0.387) 3.0-3(0.387) =0.387 =0.387 =0.613mol =1.84mol mol mol
500
The 6 Strong Acids are: The Strong Bases are:
What is 6 Strong Acids: Strong Bases: -HCl -Group 1 & 2 (Except -HBr Be) bonded with OH -HI -H2SO4 -HNO3 -HClO4
500
What's the difference between theoretical and experimental endpoint?
What is Theoretical endpoint is when the moles of titrants equals the moles of the solution and experimental endpoint is when the indicator changes color, which means that there might be more titrant in the solution.
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