End of Module 14 Quiz

In the Bronsted – Lowry definition of acids and bases, an acid ___________

In the Bronsted – Lowry definition of acids and bases, a base  ___________

In the following reaction in aqueous solution, the acid reactant is __________ and its conjugate base ________

CH3NH2 (aq)    +   HSO4 –  (aq)      CH3NH3 +  (aq)  +     SO4  2-  (aq)

In the following reaction in aqueous solution, the acid reactant is __________ and its conjugate base _________

CH3COOH (aq)    +   NH3 (aq)      CH3COO  –  (aq)  +     NH4 + (aq)

Which of the following is the conjugate acid of the hydrogen phosphate ion, HPO4 2-?

Which of the following is Not a conjugate acid – base pair?

Which one of the following is a strong acid?

Which of the following compound cannot be a Bronsted – Lowry base?

When [H +] = 1.0 x 10 -3 M in water at 25 oC, then ____________

What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8 x 10 -8?

The concentration of acetic acid (pKa = 4.75) in vinegar is about 1.0 M. With this information, what do you predict the pH of vinegar to be?

What is the concentration of [OH  –] in a 0.20 M solution of ammonia? The Kb value for ammonia 1.8 x 10 -8

What is the hydronium ion concentration in a 0.20 M solution of ammonia? The Kb value for ammonia 1.8 x 10 – 10

Three acids found in food are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The pKa values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has the conjugate bases of these acids in order of decreasing strength?

Phosphoric acid is a triprotic acid, ionizing in the following sequential steps:

Which equilibrium is most import in determining the pH of a solution of sodium phosphate?

What is the pH of a 0.20 M solution of sodium acetate? The Kb for acetic acid is 1.8 x 10 -5.

What is the pH of a 0.10 M solution of weak acid triethyl chloride? The pKa = 4.13 for it’s conjugate triethyl amine

The pH of an aqueous solution fluoride NaF solution is ___________ because _________

Which of the following salts’ combination, consist of salts that all form basic solution in water?

The pOH of a solution of NaOH is 11.30. What is the [H+] for this solution?

The [H3O+] in a 0.050 M solution of Ba(OH)2 is:

What is the approximate pH of a solution labeled 6 x 10–5 M HBr?

What is the pH of 500 mL of solution containing 0.0124 grams of Ca(OH)2?

The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution?

A solution in which [H+] = 10–8 M has a pH of ___ and is ___.

The pH of a 0.02 M solution of an unknown weak acid is 3.7. what is the pKa of this acid?

What is the approximate pH of a solution labeled 0.050 M HClO? Ka of HClO can be looked up from the internet.

What is the pH of a solution labeled 0.30 M (CH3)3N? Kb of CH3)3N can be looked up from the internet.

Which of the following solutions has the lowest pH at 25oC? (No calculations required.)

A 0.10 M solution of a weak acid, HX, is 0.059% ionized. Evaluate Ka for the acid.

What is the percent ionization of an 1.2 M HF solution?

Which of the following weak acids ionizes to give the strongest conjugate base?

Which of the following is true about a 0.10 M solution of a weak acid, HX?

Calculate the hydrolysis constant for the cyanide ion, CN–.

Calculate the pH of a 0.50 M solution of NaNO2.

What is the concentration of a sodium acetate solution if the pH of the solution is 9.19?

What is the pH of 0.060 M NH4Cl?

What is the concentration of ammonium chloride in a solution if its pH is 4.80?

The pH of 0.15 M trimethylammonium chloride, (CH3)3NHCl, a salt, is 5.34. What is the percent hydrolysis?

Arrhenius defined an acid as:

In the Bronsted-Lowry system, a base is defined as:

In the equation: HF + H 2 O  H 3 O + + F –

For the system shown here: HOBr + OH–    H2O  +  OBr–
Bronsted would classify the base species as:

Which is the strongest acid?

Which of these species is probably the weakest acid?

Consider the neutralization reactions between the following acid-base pairs in dilute aqueous solutions:

For which of the reactions is the net ionic equation: H+  +  OH–     H2O ?

Which one of the following represents the net ionic equation for the reaction of nitric acid with aluminum hydroxide?

Which one of the following is an amphoteric metal hydroxide?

According to the Lewis theory, a base _____ .

1. For the following reaction, which of the following is a conjugate acid-base pair?

HC2O4– (aq)  + H2O (l)   H3O+ (aq)  +  C2O4 2– (aq)

1. Which of the following is true of the following system?

                   CH3NH3 + (aq)  +  OH– (aq) CH3NH2 (aq)  +  H2O (l)

For the following reaction, which of the following is a conjugate acid-base pair?

                   H2PO4– (aq) + NH3 (aq) HPO42- (aq) + NH4+ (aq)

What is the conjugate base of HCO3 –?

Which one of the following is a weak acid?

Which salt is not derived from a strong acid and a strong soluble base?

Which one of the following is a strong electrolyte?

In a sample of pure water, only one of the following statements is always true at all conditions of temperature and pressure. Which one is always true?

If Kw is 2.9 x 10–15 at 10 oC, what is the pH of pure water at 10oC?