Deck 12: Solutions, Body Fluids, and Electrolytes

Question 1

The most important physiological characteristic of solutions is their ability to exert pressure.

Answer 1

True

Question 2

Which of the following is an isotonic solution?

A)0.09% NaCl
B)0.90% NaCl
C)9.00% NaCl
D)19.0% NaCl

Answer 2

B

Question 3

Which of the following is true regarding osmotic pressure?

A)Osmotic pressure depends on the number of particles in solution.
B)Osmotic pressure varies inversely with temperature.
C)Osmotic pressure is highest in dilute solutions.
D)Osmotic pressure varies inversely with tonicity.

Answer 3

A

Question 4

Which of the following is termed a physiologic solution?

A)isotonic
B)noncovalent
C)nonpolar covalent
D)polar electrovalent

Question 5

A 3% NaCl solution is called what?

A)hypertonic
B)hypotonic
C)isotonic
D)normotonic

Question 6

How is the gram-equivalent (gEq) weight of a substance computed?

A)dividing its gram atomic weight by its valence
B)dividing its valence by its gram atomic weight
C)multiplying its atomic number times its atomic weight
D)multiplying its gram atomic weight times its valence

Question 7

Gas transport in the body is most affected by changes in which of the following variables?

A)ambient pressure.
B)inspired gas temperature.
C)oxygen's solubility coefficient.
D)water vapor pressure of inspired gases.

Question 8

Positive ions are referred to as what?

A)anions
B)cations
C)covalents
D)electrolytes

Question 9

Which of the following is NOT true regarding solubility? 1.Nature of the solute. The ease with which substances go into a solution in a given solvent depends on the forces of the solute-solute molecules and varies widely.2.Nature of the solvent. A solvent's ability to dissolve a solute depends on the bonds of the solvent-solvent molecules, and also varies widely.3.Temperature. Solubility of most solids increases with increased temperature. However, the solubility of gases varies inversely with temperature.4.Pressure. The solubility of solids and liquids is not greatly affected by pressure. The solubility of gases in liquids, however, varies directly with pressure.

A)Gas solubility varies directly with pressure.
B)Gas solubility varies directly with temperature.
C)Solvents vary in their ability to dissolve substances.
D)The solubility of solids increases with temperature.

Question 10

What is the gEq weight of an acid?

A)amount of the acid containing 1 mol of replaceable H⁺ ions
B)amount of the acid containing 1 mol of replaceable OH^- ions
C)gram atomic weight of the acid times its valence
D)milligrams of acid per deciliter (dl) of normal solution

Question 11

The ease with which a gas dissolves into a solvent is at least partially determined by which of the following? 1.Nature of the solute. The ease with which substances go into a solution in a given solvent depends on the forces of the solute-solute molecules and varies widely.2.Nature of the solvent. A solvent's ability to dissolve a solute depends on the bonds of the solvent-solvent molecules, and also varies widely.3.Temperature. Solubility of most solids increases with increased temperature. However, the solubility of gases varies inversely with temperature.4.Pressure. The solubility of solids and liquids is not greatly affected by pressure. The solubility of gases in liquids, however, varies directly with pressure.

A)gas conductivity
B)gas temperature
C)level of 2,3-DPG
D)solvent conductivity

Question 12

The combination of red blood cells in plasma is a good example of what?

A)colloid
B)mixture
C)solution
D)suspension

Question 13

What is the affect of osmotic pressure on solutions of different solute concentrations, separated by a semipermeable membrane?

A)causes a net loss of fluid
B)equal distribution of solvent
C)has no effect in this situation
D)redistribution of the solute

Question 14

What is the attractive force of solute particles in a concentrated solution?

A)diffusion pressure
B)gas pressure
C)hydrostatic pressure
D)osmotic pressure

Question 15

What is a stable mixture of two or more evenly dispersed substances?

A)colloid
B)mixture
C)solution
D)suspension

Question 16

If your objective were to draw water out of cells or tissues, you would expose them to what type of solution?

A)hypertonic
B)hypotonic
C)isotonic
D)normotonic

Question 17

What is a uniform distribution of large molecules that attract and hold water?

A)colloid
B)mixture
C)solution
D)suspension

Question 18

A solution holding the maximum amount of solute in a given volume at a constant temperature is said to be what?

A)hypertonic
B)hypotonic
C)saturated
D)supersaturated

Question 19

If a 60% solution (A) were exposed to a 10% solution (B) across a semipermeable membrane, what would be the strength of each solution following equilibrium?

A)solution A 10%/solution B 60%
B)solution A 35%/solution B 35%
C)solution A 50%/solution B 20%
D)solution A 60%/solution B 10%

Question 20

In which of the following solutions do the molecules of solute remain intact?

A)electrolytic
B)electrovalent
C)nonpolar covalent
D)polar covalent

Question 21

What is the smallest fluid subcompartment of extracellular water?

A)interstitial
B)intraorganelle
C)intravascular
D)transcellular

Question 22

In which of the following types of solutions is the relationship of solute to solvent expressed as a proportion?

A)normal
B)percent
C)ratio
D)weight/volume

Question 23

What is a characteristic of an acid?

A)absorbs H⁺ ions
B)accepts a proton
C)is a proton donor
D)produces OH^- ions

Question 24

Intracellular water represents about what proportion of total body water?

A) $1 / 4$
B) $1 / 3$
C) $1 / 2$
D) $2 / 3$

Question 25

A serum value of 140 mEq/L of Na is equivalent to how many mg/dl?

A)14 mg/dl
B)70 mg/dl
C)280 mg/dl
D)322 mg/dl

Question 26

What is the relation between pure water and acid-base balance?

A)A solution with an OH^- concentration greater than that of water acts as an acid.
B)Pure water is slightly acidic solution.
C)The concentrations of both H⁺ and OH^- ions are equal.
D)The H⁺ concentration of water can be designated as 1 nmol/L.

Question 27

Supply the definition for a base substance.

A)compound that will donate a H⁺ ion
B)any compound that will accept a proton
C)only substances that contain a hydroxyl group
D)substances that contain Na⁺ ions

Question 28

You prepare a solution by combining 5 g of glucose with 95 g of water. What type of solution are you making?

A)normal
B)percent
C)ratio
D)weight/volume

Question 29

Which of the following describes an aspect of pH?

A)Any solution with a pH of 7 is neutral.
B)A pH of 7 describes an acidotic solution.
C)A pH change from 7 to 8 equals a 2-fold increase in H⁺ ion concentration.
D)The pH is the log of the OH^- ion concentration.

Question 30

Where does ammonia play its most important role as a base buffer?

A)kidney
B)liver
C)lung
D)vasculature

Question 31

Which of following is NOT a nonhydroxide base?

A)ammonia
B)carbonates
C)certain proteins
D)ammonium

Question 32

Which of the following is a facet of blood proteins?

A)Blood proteins are composed of amino acids held together by fatty acids.
B)Deoxygenated hemoglobin (Hb) is unable to accept H⁺ ions.
C)In an alkaline environment, blood proteins can act as bases.
D)The imidazole group on amino acids is the key binding site for other amino acids.

Question 33

How is pH defined?

A)log of the dissociation constant of the weak acid in a solution
B)negative logarithm of the H⁺ ion concentration of a solution
C)point at which an electrolyte solution is exactly 50% dissociated
D)ratio of a solution's weak acid concentration to its conjugate base pair

Question 34

Pick the correct statement as it relates to hemoglobin and acid-base buffering.

A)Deoxygenated hemoglobin acts as an acid at the tissue level.
B)Deoxygenated hemoglobin is a fairly strong base.
C)Hemoglobin contributes more H⁺ in the face of increased histidine.
D)In an alkaline environment, hemoglobin becomes an ineffective base.

Question 35

You prepare a solution by dissolving 5 g of glucose in 100 ml of solution. What type of solution are you making?

A)normal
B)percent
C)ratio
D)weight/volume

Question 36

What type of solution could have 1 mol of solute per L of solution?

A)molal
B)molar
C)normal
D)weight/volume

Question 37

Which of the following are true regarding water in the human body?
I .The more fatty tissue there is, the greater is the percentage of body water.
II.Total body water depends on an individual's weight and sex.
III.Water constitutes about 45% to 80% of an individual's body weight.
IV.Water content is highest in the aged.

A)I and II
B)II and IV
C)III and IV
D)II and III

Question 38

If a patient's pH were to drop from 7.40 to 7.10, the H⁺ concentration will increase by how much?

A)*2
B)*3
C)*5
D)*10

Question 39

What type of solution could have 1 gEq of solute per L of solution?

A)molal
B)molar
C)normal
D)weight/volume

Question 40

You add 50 ml of water to 150 ml of a 6% solution. What is the new concentration?

A)3.0%
B)4.5%
C)7.5%
D)12.0%

Question 41

By what process is water replenished?
I)absorption
II)ingestion
III)metabolism

A)I and II
B)I and III
C)II and III
D)I, II, and III

Question 42

During recovery from a serious surgery or trauma, how much water is likely to be produced in a 24-hour period by the catabolism of fat and proteins?

A)300 ml
B)500 ml
C)750 ml
D)1000 ml

Question 43

Water can be lost from the body through what organ systems?
I)gastrointestinal tract
II)liver
III)lungs
IV)skin

A)I, II, and III
B)I, III, and IV
C)II and IV
D)I, II, III, and IV

Question 44

What is the net affect of the hydrostatic pressure gradient between the capillary and interstitial space?

A)It tends to push water into the capillaries.
B)It tends to push water into the interstitial spaces.
C)The pressure gradient is zero so fluid movement is due to osmosis.

Question 45

Which of the following is FALSE regarding water balance and the gastrointestinal tract?

A)The gastrointestinal tract processes some 8 to 10 L of fluid per day.
B)The large intestine reclaims more than 98% of the daily gastrointestinal fluid volume.
C)Vomiting and diarrhea can cause large gastrointestinal tract fluid losses.
D)The gastrointestinal tract is responsible for the most sensible fluid loss.

Question 46

Pick the statement that best describes the relationship between infants and their body fluids?

A)Fluid loss or lack of intake depletes infants of water slower than it does adults.
B)Infants have proportionately less body water than do adults.
C)Infants' higher metabolic rates necessitate greater urinary excretion compared with adults.
D)Under normal circumstances, infants' water loses are three times those of adults.

Question 47

What is the average urine output in a healthy adult?

A)600 to 800 ml/day
B)800 to 1000 ml/day
C)1000 to 1200 ml/day
D)1200 to 1400 ml/day

Question 48

Which of the following is NOT a major extracellular electrolyte?

A)Cl^-
B)HCO₃^-
C)K⁺
D)Na⁺

Question 49

What maintains the volume and composition of body fluids?
I)filtration and reabsorption of sodium by the kidneys
II)regulation of water balance by vasopressin (ADH)III.gastrointestinal filtration and excretion of chloride

A)I and II
B)I and III
C)II and III
D)I, II, and III

Question 50

If airway humidification is inadequate, a patient with a tracheostomy can have additional water losses as high as what level?

A)100 ml/day
B)300 ml/day
C)500 ml/day
D)700 ml/day

Question 51

Insensible water loss occurs through what organs?
I)gastrointestinal tract
II)kidneys
III)lungs
IV)skin

A)III and IV
B)I, II, and IV
C)II and III
D)II and IV

Question 52

Which of the following is FALSE regarding body fluids and electrolytes?

A)Interstitial fluid contains substantially more protein than does plasma.
B)Intravascular and interstitial fluid have similar electrolyte compositions.
C)Osmotic pressure helps to determine fluid distribution between compartments.
D)Proteins account for the high colloid osmotic pressure of plasma.

Question 53

What establishes the capillary colloidal osmotic pressure?

A)presence of electrolytes in plasma
B)presence of plasma proteins in blood
C)presence of RBCs in whole blood
D)presence of WBCs in whole blood

Question 54

What best describes an aspect of the movement of fluid and solutes between the capillaries and the interstitial space?

A)At the tissue level, osmotic pressure tends to draw water into the interstitial space.
B)Electrolytes move freely across the capillary wall into the interstitium.
C)The capillary and interstitial hydrostatic pressures are approximately equal.
D)The interstitial fluid has a relatively high protein concentration.

Question 55

An adult's insensible water loss averages what level?

A)300 ml/day
B)500 ml/day
C)700 ml/day
D)900 ml/day

Question 56

What does the Donnan effect describe?

A)how Cl^- exchanges for HCO₃^- in RBCs at the tissue level
B)how proteins attract cations, which increase capillary osmotic pressure.
C)relationship between colloidal osmotic pressure and fluid movement at tissue
D)relationship between osmotic and hydrostatic pressure at the capillary

Question 57

What are the main intracellular electrolytes?
I)K⁺
II)Na⁺
III)phosphate
IV)sulfate

A)I, III, and IV
B)II, III, and IV
C)I and II
D)I, II, III, and IV

Question 58

About how much additional fluid does an adult lose for each degree of temperature above 99° F that persists for 24 hours?

A)500 ml
B)1000 ml
C)1500 ml
D)2000 ml

Question 59

An adult's insensible water through the lungs averages what level?

A)100 ml/day
B)200 ml/day
C)300 ml/day
D)400 ml/day

Question 60

Patients with what condition are prone to evaporative water loss through the lungs?
I)artificial airways
II)hypothermia
III)increased ventilation

A)I and II
B)I and III
C)II and III
D)I, II, and III

Question 61

According to the Starling equilibrium equation, which of the following will NOT facilitate fluid filtration from the capillaries into the interstitial space?

A)high capillary hydrostatic pressure
B)high capillary permeability
C)low capillary osmotic pressure
D)low interstitial osmotic pressure

Question 62

What cation is the most prominent in the intracellular compartment?

A)Ca²⁺
B)K⁺
C)Li⁺
D)Na⁺

Question 63

What is the most prominent anion in the body?

A)Cl^-
B)HCO₃^-
C)phosphate
D)sulfate

Question 64

What is the role of kidneys when a patient experiences acute respiratory alkalosis?

A)Cl^- shift enhances the body's compensatory mechanisms.
B)HCO₃^- is eliminated in the urine.
C)It dumps Cl^- so as to retain HCO₃^-.
D)The Hamburger phenomenon occurs.

Question 65

Which of the following correctly describes a facet of chloride?

A)A loss of Cl^- is equivalent to a gain in acid.
B)Cl^- is usually excreted with H⁺ as HCl.
C)Cl^- levels vary inversely with HCO₃^- levels.
D)Cl^- plays a key role in acid-base buffering.

Question 66

The alveolar interstitial region of the lungs remains relatively "dry" primarily because of what?

A)low capillary hydrostatic pressure
B)low capillary osmotic pressure
C)low capillary permeability
D)low interstitial osmotic pressure

Question 67

What can cause hypochloremia?
I)diuretics
II)gastrointestinal loss
III)metabolic acidosis

A)I and II
B)I and III
C)II and III
D)I, II, and III

Question 68

Which patients are prone to K⁺ depletion and hypokalemia?
I)postsurgical patients
II)those with renal disease
III)trauma victims

A)I and II
B)I and III
C)II and III
D)I, II, and III

Question 69

Describe the normal pressures or flows at the arterial end of the capillary.

A)Electrolytes move from the interstitium into the capillary.
B)Hydrostatic pressure is approximately 24 mm Hg.
C)Osmotic pressure is approximately 30 mm Hg.
D)Plasma minus the proteins flows into the interstitium.

Question 70

What is a normal range for serum Cl-^--?

A)3.5 to 4.8 mEq/L
B)98.0 to 106.0 mEq/L
C)137.0 to147.0 mEq/L
D)150.0 to 220.0 mEq/L

Question 71

Under normal circumstances, a small amount of fluid is filtered from the capillary in excess of that which is absorbed. What prevents edema from occurring under these conditions?

A)The lymphatic system absorbs it and returns it to the circulatory system.
B)Tissue cells absorb this fluid and use it in the metabolic process.
C)Wandering macrophages use this excess fluid in hydrolyzing invaders.
D)Waste products dilute this, maintaining eutonic conditions.

Question 72

Na⁺ reabsorption in the kidneys is governed mainly by the level of what hormone?

A)ADH
B)aldosterone
C)angiotensin
D)insulin

Question 73

Which of the following would NOT cause an abnormal loss of Na⁺ (hyponatremia)?

A)ascites
B)excessive sweating or fever
C)use of certain diuretics
D)steroid therapy

Question 74

Which of the following describe roles played by HCO₃^-?
I.HCO₃^-levels vary directly with Cl^- levels.
II.It is the primary vehicle for blood carbon dioxide transport.
III.It plays a key role in acid-base homeostasis.

A)I, II, and III
B)I and III
C)II only
D)II and III

Question 75

What is a normal K⁺ blood level?

A)3.5 to 5.0 mEq/L.
B)7.8 to 10.2 mEq/L
C)22 to 26 mEq/L
D)35 to 42 mEq/L

Question 76

Which answer best describes the relationship between K⁺ movement and acid-base balance?

A)Excess extracellular H⁺ ions are exchanged for intracellular K⁺.
B)Extracellular acidosis results in serum hypokalemia.
C)Low-K⁺ diets are required following nasogastric suctioning.
D)When the extracellular pH rises, K⁺ moves out of the cells.

Question 77

What is a normal range for serum sodium?

A)3.5 to 4.8 mEq/L
B)67.0 to 75.0 mEq/L
C)98.0 to 105.0 mEq/L
D)136.0 to 145.0 mEq/L

Question 78

Which of the following factors contributes to reabsorption of tissue fluid in dependent regions of the body?

A)hydrostatic pressure of 100 mm Hg.
B)low capillary permeability
C)low interstitial osmotic pressure
D)pumping action of skeletal muscles

Question 79

What is a common cause for pulmonary edema due to increased hydrostatic pressure?

A)alveolar-capillary damage
B)chronic liver disease
C)failing left ventricle
D)failing right ventricle

Question 80

What affect do metabolic acidosis and aldosterone have in common?

A)They both result in renal loss of K⁺.
B)There is a loss of HCO₃^-and Cl^-in the renal tubules.
C)There is retention of CO₂ and Cl^-.
D)They both cause renal retention of HCO₃^-.