Chapter 7 for Exam 3 Cardiopulmonary

7.34 to 7.45

Normal arterial pH range for people is_____________________.

pH > 7.45

Alkalosis pH is greater than?

pH < 7.34

Acidosis pH is less than?

1. Metabolism of body fats, 2. Transport of CO2 in blood as bicarbonate HCO3- liberates H+ ions & 3. Anaerobic metabolism of glucose

Most H+ ions in the body originate from: Name one of them.

Acids

Can react (dissolve) with many metals, Can "burn" hole through clothing, and substance that releases hydrogen ions [H+] in measurable amounts.

0

Defined as proton donors because hydrogen ion is only a hydrogen nucleus proton. How many neutrons does a hydrogen molecule have?

Free hydrogen

Acidity of the solution is directly related to the concentration of hydrogen protons.

Reflects only _______________________________________ions.

Hydrogen proton H+

Hydrochloric acid (HCl) found in stomach works to aid digestion and dissociates into a _____________________________ and a chloride ion:

Carbonic acid

____________________________ (H2CO3) is formed in small amounts when its anhydride, carbon dioxide (CO2), dissolves in water.

Free

Acidity of solution reflects only ______________________ hydrogen ions and not hydrogen ions still combined with anions. H+

Weak Acids

Do not dissociate completely in solution and have much smaller effect on pH, but do have very important role in resisting sudden pH changes

Bases

Proton acceptors and substance that takes up hydrogen ions {H+] in measurable amounts,

Bicarbonate (HCO3-)

____________________________________ is a negatively charged ion (HCO₃⁻) that plays a vital role in maintaining the body's acid-base balance. It acts as a buffer, helping to neutralize acids and stabilize pH levels in the blood and other bodily fluids.

Ammonia (NH3)

_________________________________ is a base and is a natural waste product of protein breakdown (digestion). It has pair of unshared electrons that strongly attract protons.

Ammonia (NH3)

When accepting a proton, ________________________________becomes ammonium ion (NH4+).

Urea Cycle

The ____________________________ cycle removes ammonia from the blood and makes urea, which is eventually excreted as urine.

Water (H2O)

Strong bases dissociate easily in ________________________________ and quickly tie up H+.

Weak bases

_____________________________________ dissociate incompletely and reversibly and are slower to accept Hydrogen protons.

Acidic

As concentration of hydrogen ions in solution increase, the more ____________________________ solution becomes H+

Basic Solution

As level of hydroxide ions increases, the more ___________________________, or alkaline, solution becomes. OH⁻

14

Clinically, concentration of hydrogen ions in body measured in units called pH units. pH scale runs from 0 to_____________ and is logarithmic.

tenfold

Each successive unit change in pH represents ______________change in hydrogen ion concentration.

hydroxide ions (OH-)

When pH is 7, the number of hydrogen ions precisely equals number of _______________________. This solution is said to be neutral.

Acidic

Pure water has neutral pH of 7. Solution with pH below 7 is _____________________.

False 10 times

A solution with pH of 6 has 20 times more hydrogen ions than solution with pH of 7. True or False

7

A solution with pH greater than_________________________ is alkaline, where the hydroxide ions outnumber hydrogen ions

True

A solution with pH of 8 has 10 times more hydroxide ions than solution with pH of 7. True or False

Chemical buffer system, Respiratory system, Renal system

Under normal conditions, both H+ and HCO3- ion (bicarbonate) concentrations in blood are regulated by three major systems: Name them!

HCO3- (bicarbonate)

Most of CO2 produced at tissue cells is carried to lungs in form of _____________________________________________.

Respiratory System

___________________________________acts within one to three minutes by increasing or decreasing breathing depth and rate to offset acidosis or alkalosis, respectively.

Acidosis

______________________________________ refers to high levels of acid in the body. If the body becomes too acidic or too alkaline, it can cause serious health problems.

Alkalosis

The buildup of excess base (lack of acids) in the body fluids.

HCO3- (bicarbonate)

______________________________ transformed back into CO2 and eliminated in alveoli.

Chemical Buffer Systems

First line of defense against pH changes.

Buffering

A variety of ______________________systems permits blood and other bodily fluids to maintain a narrow pH range, even in the face of perturbations. A buffer is a chemical system that prevents a radical change in fluid pH by dampening the change in hydrogen ion concentrations in the case of excess acid or base.

Increasing

When pH declines (e.g., metabolic acidosis caused by lactic acids), respiratory system responds by ___________________ breathing depth and rate.

Decreasing

When pH rises (e.g., metabolic alkalosis caused by hypokalemia), respiratory system responds by ______________________________ breathing depth and rate.

Renal System

_____________________________ is the body's most effective acid-base balance monitor and regulator but requires one day or more to correct abnormal pH concentrations.

Renal System

Only the _______________________________ system can rid body of acids such as phosphoric acids, uric acids, lactic acids, and ketone acids.

Increase

When extracellular fluids become acidic, renal system retains HCO3- and excretes H+ ions into urine

causing blood pH to ________________________.

Decrease

When extracellular fluids become alkaline, renal system retains H+ and excretes basic substances primarily HCO3- into urine causes blood pH to ___________________________.

Hyperventilation

_________________________________________ happens when you exhale more than you inhale. It causes symptoms like lightheadedness, chest pain and feeling like you're out of breath.