Chapter 9 Chem

Identify the Brønsted acid(s) in the reaction. HIO3(aq) + H2O (l) H3O+ (aq) + IO3 - (aq)

HIO3 and H3O+

Phosphoric acid, H3PO4, undergoes three dissociation reactions. Which of the three acids is the weakest?

HPO 2/4-

In the following reaction, all substances are soluble, and all dissociate except H2O. Identify the spectator ions. HCl + KOH KCl + H2O

K+ and Cl

Which of the following substances could behave as an Arrhenius base?

KOH

The expression for the Ka of the weak acid HF would be which of the following?

Ka = [F-][H+] / [HF]

What salt would be produced by the reaction of H2SO4 with LiHCO3?

Li2SO4

Antacids contain a substance that neutralizes hydrochloric acid. What is a candidate for use as an antacid?

MgCO3

Which of the following would you expect to be a weak electrolyte?

More than one answer is correct.

Identify all Brønsted base(s) in the reaction. N3 - (aq) + H2O (l) HN3 (aq) + OH- (aq)

N3- and OH-

A 10-8 M solution of HCl is prepared. It would be expected to be _____.

acidic

A solution for which [OH] = 3.0 1010 is classified as _____ .

acidic

It has been proposed that atmospheric CO2 could be reduced by absorption in to the Earth's oceans. Which of the following reactions would be involved?

all of the above

pH changes can be determined with a(n)___.

all of the above

Which of the following is present in pure water?

all of them

When your liver detoxifies ethyl alcohol, the concentration of the hydrogen ion increases. This will result in

respiratory acidosis

Which of the following mixtures would represent a buffer?

sodium formate/formic acid

Which of the following is a property of acid solutions?

sour taste

The term, strong acid, refers to

the ability for the acid to completely dissociate in solution.

When an acid is analyzed by adding a measured quantity of base, the point at which all the acid has reacted is correctly called

the equivalence point

The classification of an acid or base as weak or strong is based upon

the extent of dissociation of the acid or base.

The procedure commonly used to determine the amount of base in a solution by adding a measured quantity of acid is called _____ .

titration

Some salts isolated by evaporation retain water that is called

water of hydration

What is the function of H2 C6 H5 O-7 in the first ionization of citric acid?

The ion serves as the conjugate base of the acid, H3C6H5O7.

According to the Brønsted Theory, a conjugate pair is composed of a Brønsted acid and a Brønsted base.

True

Ammonium chloride in water will produce an acidic solution.

True

Gastroesophageal reflux disease (GERD) is the result of a malfunctioning muscle that allows stomach to enter the esophagus.

True

KOH is a strong base.

True

Most acids are weak acids.

True

NaH2PO4 alone in a water solution could behave as a buffer.

True

SO 2/4- is a stronger base than HSO-4.

True

The pH of a solution of baking soda, NaHCO3, would be expected to be above 7.

True

The pH of blood must remain stable between 7.35 and 7.45. One of the blood components is the bicarbonate ion, HCO-3 . Bicarbonate takes part in two reactions that are: H2CO3(aq) H+(aq) + HCO-3(aq) HCO-3(aq) + H+(aq) This set of equations indicates that this system is a good candidate to act as a buffer system used to hold the pH of blood reasonably stable.

True

The pH of household ammonia is expected to be above 7 because household ammonia is NH4OH.

True

The reason pure water has a pH of 7 is that there is the same concentration of hydrogen and hydroxide ions on the self-ionization of water.

True

The salt of a strong acid and a weak base will give an acidic solution.

True

The salt of a weak base with a weak base could behave as a buffer.

True

Water is able to act not only as a solvent but as and acid or base.

True

When an inorganic acid and an inorganic base, as defined by Arrhenius, react, the products are salt and water.

True

A patient comes to you suffering from a battery acid burn (sulfuric acid). What is the best thing to use to neutralize the acid, while you continue to run cool water over the affected area?

a 1 M sodium bicarbonate solution (NaHCO3)

The cation (positive ion) in a salt comes from _____ .

a base

A higher pH corresponds to _____ .

a lower [H+]

When a strong acid is added to a weak base and mixed, which of the following would not be produced?

conjugate base

A reaction in which an acid and a base react completely, leaving only a salt and water, is referred to as a(n)

neutralization reaction

Identify the substance with the lowest pH.

orange juice

A 25.00 mL sample of hydrochloric acid solution, HCl, is titrated with 0.0512 M NaOH solution. The volume of NaOH solution required is 21.68 mL. What is the molarity of the HCl solution?

0.0444

A 25.00 mL sample of H2SO4 acid solution requires 17.35 mL of 0.118 N base for titration. What is the normality of the acid solution?

0.0819 N

How many equivalents are contained in 0.25 moles of H2SO4?

0.50

How many meq are contained in 25.00 mL of a 0.225 M solution of CaCl2?

1.12 x 10^1 meq

A solution has a pH of 8.72. What is the value of [H+]?

1.9 x 10-9

A solution has a pH of 11.60. The value of [H+] is _____ .

2.5 x 10-4

To determine the number of equivalents of Al(NO3)3 in a 0.750 M solution, the conversion factor would be which of the following?

3 eqAl (NO3)3 / 1 molAl (NO3)3

A solution for which [H+] = 1.0 103 will have a pH of _____ .

3.00

Consider the following list of pKa values for a series of acids. Which is the strongest acid?

3.21

During a field trip to study the problem of acid rain, you test one lake that had observed a major fish kill. It was found to have a pH of 5.37. What is the [H+]?

4.3 x 10-6

What is the pKa of an acid with a Ka of 1.82 x 10-5?

4.74

What volume of 6.0 M HNO3 would be needed to make 500 mL of 0.50 M solution?

42 mL

The molar concentration of OH in a water solution is 1.0 x 10-9. The pH of the solution is _____ .

5.00

Which salt shifts the pH when dissolved in water?

Al(NO3)3

HCl will react with

All three are correct.

Which of the following sets of reactants could be used to prepare CaI2?

Any of these could be used.

Sodium phosphate can be used as a driveway degreaser. When added to water, the following equilibrium is attained. Sodium phosphate is acting as a(n) ______. Na3PO4 (aq) + 3H2O (l) H3PO4 (aq) + 3OH-(aq)

Brønsted base

A Brønsted base is a proton donor.

False

Citrus fruits are high in both citric acid and ascorbic acid (Vitamin C). As such, eating or drinking large amounts of citrus fruits helps strengthen teeth.

False

HPO2/4- is a stronger acid than H2PI-4.

False

NaCl is an example of a good buffer.

False

Nitric acid, HNO3, is a weak acid.

False

Sodium nitrate in water will produce a basic solution.

False

Solutions with a pH less than 7.00 are basic.

False

The goals of an acid/base titration is to reach neutrality.

False

The major difference between the Arrhenius Theory and the Brønsted Theory is that there is no hydrogen in the Brønsted Theory.

False

The salt of a strong acid with a strong base could behave as a buffer.

False

According to the Arrhenius theory, what is produced when an acid dissolves in water?

H+

In the Brønsted theory, both acids and bases are defined in terms of how substances lose or gain

H+

When a solution of HNO3 is added to a solution of NaHCO3, the net ion equation for reaction that occurs is which of the following?

H+ (aq) + HCO3- (aq) → H2O(I) + CO2 (g)

Which of the following is a weak acid?

H2CO3

Identify two Brønsted base(s) in the reaction. HIO3 (aq) + H2O (I) H3O+ (aq) + 103 - (aq)

H2O, IO3-

The dissociation reaction for the weak acid, H2PO3- would be which of the following?

H2PO3 → HPO3^2- + H+

In a buffer solution made up of equal concentrations of acetic acid and sodium acetate, NaC2H3O2, which component is used to buffer against added OH?

HC2H3O2

Which of the following salts would produce a basic solution (pH higher than 7) upon being dissolved in pure, distilled water?

Na2CO3

Which of the following statements is true for neutral solutions in which water is the solvent?

Neutral solutions contain H3O+ and OH ions in equal concentrations.

Seageroic acid has a pKa of 8.23, whereas slabaughic acid has a pKa of 18.65. From these facts, which of the following is true?

Seageroic acid is a stronger acid than slabaughic acid.

What are the missing products in the following reaction when it is written as a full equation? 2HBr + SrCO3 ____ + ____ + H2O

SrBr2 + CO2

A water solution is found to have a molar OH concentration of 3.2 x 10-5. The solution would be classified as _____ .

basic

The molar concentration of H+ ions in a solution is 5.8 x 10-9. The pH is _____ .

between 8.00 and 9.00

The buffer capacity is the amount of ____ that can be absorbed without causing significant changes in pH.

either acid or base

Many cleaning agents contain bases because bases react with _____ .

fats or oils

If a solution of acetic acid (a weak acid) is titrated with NaOH solution, what will be the pH at the equivalence point?

higher than 7

What would be the pH of a solution of NH4Cl in pure water?

lower than 7