Save
Busy. Please wait.
Log in with Clever
or
show password
Forgot Password?
Don't have an account?  Sign up 
Sign up using Clever
or
Username is available taken
show password


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account. Your email address is only used to allow you to reset your password. See our Privacy Policy and Terms of Service.

Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.
focusNode
Didn't know it?
click below
 
Knew it?
click below
Don't Know
Remaining cards (0)
Know
0:00
edit
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

une ch 4

acidsbasesbuffers

QuestionAnswer
Define pH. pH is the negative log of the concentration of hydrogen ions (such concentration expressed in moles per liter [mol/L]) in a solution. This determines the acidity of the solution.
Given any hydrogen ion concentration, determine the pH and vice versa pH = -log[H+],
The normal [H+] of blood is 40nM. Calculate the pH. pH = -log (H+)= -log 40 x 10-9
Recognize the acids produced by the body during metabolism and be able to state the predominant form at pH = 7.4 (ic or ate, ammonium or ammonia). 1.)H2SO4 Sulfuric Acid 2.)HNO3 Nitric Acid 3.)HCl Hydrochloric Acid
To find if bicarbonate or carbonic acid predominates at pH=7.4, use the Henderson-Hasselbalch equation. Solve for the ratio of Bicarbonate to Carbonic Acid (pKa = 6.1): 7.4 = 6.1 + log ([Bicarbonate]/[Carbonic Acid])
Equation for its dissociation of a weak acid: HA = H+ + A- [HA]= weak acid concentration, [A-]= conjugate base concentration, [H+]= proton concentration
Be able to define the Ka for the acid. Ka=[H+][A-]/[HA] Ka: dissociation constant, ::[HA]= weak acid concentration, [A-]= conjugate base concentration, [H+]= proton concentration
Relationship between pKa and Ka pKa=-log(Ka)
Bicarbonate Buffer System equation: CO2 + H2O <---> H2CO3 <---> HCO3- + H+
The partial pressure of CO2 can be roughly converted to the concentration of Carbonic Acid in the bloodstream by doing what? multiplying [PaCO2] by .03. Example: (40 mm Hg CO2) X .03 = (1.2 milli moles Carbonic Acid) in the blood stream. (Reference range for CO2 in blood is 37-43 mm Hg).
Henderson-Hasselbalch Equation for bicarbonate buffer system pH = 6.1 + log([HCO3-]/[H2CO3])
Draw the dissociation of ammonium ion. If the pKa =9.3, what form is found at pH = 7? pH = pKa + log [salt]/[acid] pH = pKa + log[NH3]/[NH4+]
The equation for the dissociation of ammonium ion NH4+ <--> NH3 + H+
If pH > pKa, what predominates? salt is predominant
if pH < pKa, what predominates? acid is predominant
Created by: carolanimal
Popular Biochemistry sets

 

 



Voices

Use these flashcards to help memorize information. Look at the large card and try to recall what is on the other side. Then click the card to flip it. If you knew the answer, click the green Know box. Otherwise, click the red Don't know box.

When you've placed seven or more cards in the Don't know box, click "retry" to try those cards again.

If you've accidentally put the card in the wrong box, just click on the card to take it out of the box.

You can also use your keyboard to move the cards as follows:

If you are logged in to your account, this website will remember which cards you know and don't know so that they are in the same box the next time you log in.

When you need a break, try one of the other activities listed below the flashcards like Matching, Snowman, or Hungry Bug. Although it may feel like you're playing a game, your brain is still making more connections with the information to help you out.

To see how well you know the information, try the Quiz or Test activity.

Pass complete!
"Know" box contains:
Time elapsed:
Retries:
restart all cards