acidsbasesbuffers
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
|---|---|---|---|---|---|
| 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
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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
Normal Size Small Size show me how
Created by:
carolanimal
Popular Biochemistry sets