A substance that donates a hydrogen ion (a proton).
What is a Bronsted-Lowry acid?
100
When the rate of the forward reaction equals the rate of the reverse reaction.
What is equilibrium?
100
The negative log of the hydrogen (hydronium) ion concentration.
What is pH?
100
If the pOH of a solution is 5.6, is the solution acidic or basic?
basic
100
The process in which an acid-base neutralization reaction is used to determining the concentration of a solution.
What is titration?
200
This type of substance contains an ionizable hydroxide group.
What is an Arrhenius base?
200
The ratio of the molar concentrations of the products to the molar concentration of the products with each concentration raised to the power equal to its coefficient in the balanced chemical equation.
What is the equilibrium constant?
200
In each condition, state which is favored, reactants or products.
Keq < 1,
Keq > 1,
Keq = 1
Keq < 1 reactants are favored,
Keq > 1 products are favored,
Keq = 1 concentration of reactants and products is equal
200
If the pH of a solution is 5, what is the pOH? What is [H3O+]?
pOH = 9, [H3O+]= 1x10-5 M
200
A method for diluting a concentrated solution without creating much waste.
What is a serial dilution?
300
A solution that resists changes in pH.
What are buffers?
300
A statement that describes how an equilibrium system shifts in response to a stress or disturbance.
What is Le Chatelier's Principle?
300
Ag+(aq) + Cl-(aq) ⇄ AgCl(s) Will the equilibrium shift to the left or the right if Ag+ added? Will the equilibrium shift to the left or the right if AgCl is removed?
Right, right
300
A stock solution has a 5M concentration. Three 1:10 dilutions are performed, starting with the stock solution. What is the concentration of the final solution?
5x10-3 M
300
The point in a titration where the concentration of the acid and the added base (or the base and the added acid) are equal.
What is the equivalence point?
400
Lemon juice, vinegar, and HCl are all examples of what type of solution? What is the possible pH range for this type of solution?
Acidic solutions, < 7
400
Would the equilibrium constant of a strong acid be a very large number, or a very small number?
very large number
400
2 SO2(g) + O2(g) ⇄ 2 SO3(g) + heat
Will the equilibrium shift to the left or the right if the temperature is increased? Will the equilibrium shift to the left or right if the pressure is decreased?
left, left
400
Write the equilibrium expression for the following reaction, and solve for the equilibrium constant.
At equilibrium, a 2.0L flask contains: 0.075 mol of PCl5, 0.050 mol of H2O, 0.750 mol of HCl, 0.500 mol of POCl3
PCl5 (s) + H2O (g) ⇄ 2 HCl (g) + POCl3 (g)
Keq = 0.14 M^2
400
Substances that change color in response to pH changes.
What are pH indicators?
500
Baking soda, ammonia, NaOH, and soap are all examples of what type of solution. What is the pH range for this type of solution?
Basic solutions, > 7
500
Would the equilibrium constant of a weak base be a very large number or a very small number?
very small number
500
A definition of the prefix "amphi" is: "both or of both kinds." Give an example of an amphiprotic substance.
water
500
If it takes 15ml of 0.1M NaOH to turn 30ml of monoprotic acidic solution with phenolphthalein pink, what is the concentration of the acidic solution?
0.05 M
500
Daily Double: What is the purpose of the ethanol in the lab "Determination of the pKa of aspirin?"
Because part of the aspirin molecule is hydrophobic, it dissolves poorly in water. Ethanol is used as an alternative solvent to water to help dissolve the aspirin as it is somewhat hydrophobic as well. Remember, "Like dissolves like."