Question 1

Which of the following substances can react with both HCl and NaOH?.

Accepted Answer

A)  Ca(HCO3)2 
B)  KCl 
C)  CH3CH2NH2 
D)  H2C2O4 
A)  Ca(HCO3)2 
B)  KCl 
C)  CH3CH2NH2 
D)  H2C2O4

Question 2

A solution composed of HCl and NaCl would produce an effective buffer.

Accepted Answer

A) True 
 B)False

Question 3

When NaOH reacts with HCl, the net ionic equation for the reaction is:

Accepted Answer

A)  H+ + OH- → H2O 
B)  Na+ + Cl- → NaCl 
C)  NaOH + HCl → NaCl + H2O 
D)  NaOH → Na+ + OH- 
E)  HCl → H+ + Cl- 
A)  H+ + OH- → H2O 
B)  Na+ + Cl- → NaCl 
C)  NaOH + HCl → NaCl + H2O 
D)  NaOH → Na+ + OH- 
E)  HCl → H+ + Cl-

Question 4

Consider the following reaction.   + H2O   HN3 + OH− This reaction indicates that:

Accepted Answer

A)    is a weak base. 
B)    is a strong base. 
C)    is a weak acid. 
D)    is a strong acid. 
A)    is a weak base. 
B)    is a strong base. 
C)    is a weak acid. 
D)    is a strong acid.

Question 5

The buffer solution in the flask was prepared using one of the substances shown below. citric acid (pKS1U1B1aS1U1B0 3.08)
NaHS1U1B12S1U1B0POS1U1B14S1U1B0 (pKS1U1B1aS1U1B0 7.21)
NHS1U1B14S1U1B0Cl (pKS1U1B1aS1U1B0 9.25)
Using the pH meter and solution shown in the image below,   complete the following statements using one of the terms below.
 increase
decrease
remain constant
citric acid
NaHS1U1B12S1U1B0POS1U1B14S1U1B0
NHS1U1B14S1U1B0Cl
-If HNO were added to the buffer solution the pH of the solution would __________.

Accepted Answer

The answer of The buffer solution in the flask was...

Question 6

Which of the following will determine the pH of a buffer made using acetic acid (HC2H3O2) and sodium acetate (NaC2H3O2)?

Accepted Answer

A)  the amount of water present 
B)  the concentration of C2H3O2- 
C)  the concentration of HC2H3O2 
D)  the ratio of the concentrations of C2H3O2- and HC2H3O2 
A)  the amount of water present 
B)  the concentration of C2H3O2- 
C)  the concentration of HC2H3O2 
D)  the ratio of the concentrations of C2H3O2- and HC2H3O2

Question 7

A solution is 0.10 M in ascorbic acid (Vitamin C), H2C6H6O6, and 0.10 M in sodium ascorbate, NaHC6H6O6. When base is added to the solution, H2C6H6O6 neutralizes the added base.

Accepted Answer

A) True 
 B)False

Question 8

When carbonated beverages are bottled or canned, the partial pressure of carbon dioxide above this liquid is maintained at a high pressure. This procedure cause the pH of the beverage to

Accepted Answer

A)  increase. 
B)  decrease. 
C)  remain constant. 
A)  increase. 
B)  decrease. 
C)  remain constant.

Question 9

Write the equation for the ionization of weak base hydrazine, N2H4, in water.

Accepted Answer

N₂H₄(aq) + H

Question 10

Excess phosphorus is excreted by the kidneys. What effect does this have on the pH of blood plasma?

Accepted Answer

A)  causes an increase 
B)  causes a decrease 
C)  has no effect 
A)  causes an increase 
B)  causes a decrease 
C)  has no effect

Question 11

In a solution of phosphoric acid all of the following species are present. Which is the least abundant?
PO43-
H2PO4-
HPO42-

Accepted Answer

Question 12

Very rapid breathing can lead to a condition know as respiratory acidosis.

Accepted Answer

A) True 
 B)False

Question 13

Using the above table, fill in the blank with the appropriate integer (1 ,2, 3,...) indicating the buffer and/or the letter indicating the formula below.
-Buffer ______________________ would be the most effective buffer in basic solutions.

Accepted Answer

The answer of   Using the above table, fill...

Question 14

The pKa of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.

Accepted Answer

A) True 
 B)False

Question 15

Consider the following three buffer reactions. Buffer 1: protein-HS1U1P1+S1S1P0 and protein
Buffer 2: HS1U1B12S1U1B0COS1U1B13S1U1B0 and HCOS1U1B13S1U1B0S1U1P1-S1S1P0
Buffer 3: HS1U1B12S1U1B0POS1U1B14S1U1B0S1U1P1-S1S1P0 and HPOS1U1B14S1U1B0S1U1P12-S1S1P0
Fill in the blank with the appropriate integer (1, 2, or 3) to indicate the buffer system described.
-Buffer______________________can have a variable pKa value.

Accepted Answer

Question 16

Which of the following pH's corresponds to a highly acidic solution?

Accepted Answer

A)  2.1 
B)  6.8 
C)  7.2 
D)  11.2 
A)  2.1 
B)  6.8 
C)  7.2 
D)  11.2

Question 17

Below is the structure for the amino acid alanine.   Alanine can undergo an internal acid-base reaction.   In this reaction, the -NH2 group functions as a base.

Accepted Answer

A) True 
 B)False

Question 18

The range of breaths per minute, also known as respiratory rate, for a normal, healthy adult is 12-20 breaths per minute. A breathing rate of higher than this is termed hyperventilation.

Accepted Answer

A) True 
 B)False

Question 19

Oxalic acid (H2C2O4) is weak acid found in the leaves of rhubarb. Which of the following solutions will have the highest pH?

Accepted Answer

A)  1.0 M H2C2O4 
B)  0.5 M H2C2O4 
C)  1.0 × 10-4 M H2C2O4 
D)  0.00075 M H2C2O4 
A)  1.0 M H2C2O4 
B)  0.5 M H2C2O4 
C)  1.0 × 10-4 M H2C2O4 
D)  0.00075 M H2C2O4

Question 20

The following reaction represents the self-ionization of ammonia (NHS1U1B13S1U1B0). NHS1U1B13S1U1B0(aq) + NHS1U1B13S1U1B0(aq)   NHS1U1B12S1U1B0S1U1P1-S1S1P0(aq) + NHS1U1B14S1U1B0S1U1P1+S1S1P0(aq)
amide ammonium
Fill in the blanks with the appropriate terms from those listed below. 
ammonia
ammonium
amide
-In this reaction, the conjugate base of ammonia is the _______________________ ion.

Accepted Answer

The answer of The following reaction represents the self-ionization of...

Which of the following substances can react with both HCl and NaOH?.

A solution composed of HCl and NaCl would produce an effective buffer.

When NaOH reacts with HCl, the net ionic equation for the reaction is:

Consider the following reaction. + H₂O HN₃ + OH− This reaction indicates that:

Which of the following will determine the pH of a buffer made using acetic acid (HC₂H₃O₂) and sodium acetate (NaC₂H₃O₂)?

A solution is 0.10 M in ascorbic acid (Vitamin C), H₂C₆H₆O₆, and 0.10 M in sodium ascorbate, NaHC₆H₆O₆. When base is added to the solution, H₂C₆H₆O₆ neutralizes the added base.

When carbonated beverages are bottled or canned, the partial pressure of carbon dioxide above this liquid is maintained at a high pressure. This procedure cause the pH of the beverage to

Write the equation for the ionization of weak base hydrazine, N₂H₄, in water.

Excess phosphorus is excreted by the kidneys. What effect does this have on the pH of blood plasma?

In a solution of phosphoric acid all of the following species are present. Which is the least abundant? PO₄^3- H₂PO₄^- HPO₄^2-

Very rapid breathing can lead to a condition know as respiratory acidosis.

Using the above table, fill in the blank with the appropriate integer (1 ,2, 3,...) indicating the buffer and/or the letter indicating the formula below. -Buffer ______________________ would be the most effective buffer in basic solutions.

The pK_a of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.

Which of the following pH's corresponds to a highly acidic solution?

Below is the structure for the amino acid alanine. Alanine can undergo an internal acid-base reaction. In this reaction, the -NH₂ group functions as a base.

The range of breaths per minute, also known as respiratory rate, for a normal, healthy adult is 12-20 breaths per minute. A breathing rate of higher than this is termed hyperventilation.

Oxalic acid (H₂C₂O₄) is weak acid found in the leaves of rhubarb. Which of the following solutions will have the highest pH?

Measurements in Science and Medicine

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Hydrocarbons: an Introduction to Organic Molecules

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Exam 7: Acids and Bases

Which of the following substances can react with both HCl and NaOH?.

A solution composed of HCl and NaCl would produce an effective buffer.

When NaOH reacts with HCl, the net ionic equation for the reaction is:

Consider the following reaction. + H2O HN3 + OH− This reaction indicates that:

Which of the following will determine the pH of a buffer made using acetic acid (HC2H3O2) and sodium acetate (NaC2H3O2)?

A solution is 0.10 M in ascorbic acid (Vitamin C), H2C6H6O6, and 0.10 M in sodium ascorbate, NaHC6H6O6. When base is added to the solution, H2C6H6O6 neutralizes the added base.

When carbonated beverages are bottled or canned, the partial pressure of carbon dioxide above this liquid is maintained at a high pressure. This procedure cause the pH of the beverage to

Write the equation for the ionization of weak base hydrazine, N2H4, in water.

Excess phosphorus is excreted by the kidneys. What effect does this have on the pH of blood plasma?

In a solution of phosphoric acid all of the following species are present. Which is the least abundant? PO43- H2PO4- HPO42-

Very rapid breathing can lead to a condition know as respiratory acidosis.

Using the above table, fill in the blank with the appropriate integer (1 ,2, 3,...) indicating the buffer and/or the letter indicating the formula below. -Buffer ______________________ would be the most effective buffer in basic solutions.

The pKa of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.

Consider the following three buffer reactions. Buffer 1: protein-H+ and protein Buffer 2: H2CO3 and HCO3- Buffer 3: H2PO4- and HPO42- Fill in the blank with the appropriate integer (1, 2, or 3) to indicate the buffer system described. -Buffer______________________can have a variable pKa value.

Which of the following pH's corresponds to a highly acidic solution?

Below is the structure for the amino acid alanine. Alanine can undergo an internal acid-base reaction. In this reaction, the -NH2 group functions as a base.

The range of breaths per minute, also known as respiratory rate, for a normal, healthy adult is 12-20 breaths per minute. A breathing rate of higher than this is termed hyperventilation.

Oxalic acid (H2C2O4) is weak acid found in the leaves of rhubarb. Which of the following solutions will have the highest pH?

Measurements in Science and Medicine

Atoms, Elements, and Compounds

Chemical Bonds

Energy and Physical Properties

Solution Concentration

Chemical Reactions

Nuclear Chemistry

Hydrocarbons: an Introduction to Organic Molecules

Hydration, Dehydration, and Alcohols

Carbonyl Compounds and Redox Reactions

Organic Acids and Bases

Condensation and Hydrolysis Reactions

Proteins

Carbohydrates

Lipids and Membranes

Nucleic Acids, Protein Synthesis, and Heredity

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Consider the following reaction. + H₂O HN₃ + OH− This reaction indicates that:

Which of the following will determine the pH of a buffer made using acetic acid (HC₂H₃O₂) and sodium acetate (NaC₂H₃O₂)?

A solution is 0.10 M in ascorbic acid (Vitamin C), H₂C₆H₆O₆, and 0.10 M in sodium ascorbate, NaHC₆H₆O₆. When base is added to the solution, H₂C₆H₆O₆ neutralizes the added base.

Write the equation for the ionization of weak base hydrazine, N₂H₄, in water.

In a solution of phosphoric acid all of the following species are present. Which is the least abundant? PO₄^3- H₂PO₄^- HPO₄^2-

The pK_a of lactic acid is 3.86, an equimolar solution of lactic acid and potassium lactate will have a pH of 7.72.

Below is the structure for the amino acid alanine. Alanine can undergo an internal acid-base reaction. In this reaction, the -NH₂ group functions as a base.

Oxalic acid (H₂C₂O₄) is weak acid found in the leaves of rhubarb. Which of the following solutions will have the highest pH?