IPS1- B5-B7 - Buffer ➡️ Isotonic Solutions

Proverbs 16:3

Buffers

____ - are compounds or mixture of compounds, that by the presence in solution, resist pH changes upon addition of small quantities of acid or alkali.

Buffer action

The resistance to pH provided by buffers is known as __________?

• Weak acid + salt of weak acid or conjugate base

• Weak base + salt of weak base or its conjugate acid

Buffer pair can be ___ [2]

Henderson-Hasselbalch Equation

The buffer equation is mainly known as the _________ equation

Buffer Capacity

____ - is the magnitude of resistance of buffer to pH changes

Buffer Capacity

____-

• is the magnitude to resist pH

• how much the buffer action

Buffer Capacity

_____ - is different form buffer action → property

-ate

common suffix for salt = ___ ?

Koppel-Spiro Van Slyke’s

Equation for Buffer Capacity is by ____ [who]?

𝜷𝒎𝒂𝒙 = 0.576C

Give the Formula of maximum buffer capacity?

Koppel-Spiro Van Slyke's Equation

Exact equation for Buffer Capacity is the ____ ?

• Blood

• Lacrimal Fluid

• Urine

Biologic Buffer Systems [3]

7

Blood is maintained at pH ______?

Plasma

The Primary buffers of blood are found in _____?

• Carbonic acid/ Bicarbonate buffer

• Sodium (N)a salts of phosphoric acid buffer

Primary Buffer in plasma (2)

Erythrocytes

Secondary buffers of blood are found in __________

• Hemoglobin / Oxyhemoglobin

• Potassium (K) salts of phosphoric acid buffer

Secondary Buffer in erythrocytes (2)

pH < 6.9 or pH > 7.8

Life threatening pH levels of blood is ___ ?

pH 7.4

Lacrimal Fluid are maintained at pH __________?

pH < 6.6 and pH > 9

Lacrimal fluid induces discomfort and flow of tears at pH levels of _________?

average pH 6 (about 4.5 to 7.8)

What is the average pH of Urine ?

ophthalmic solutions

Pharmaceutical Buffers are frequently used in formulation of _____ solutions

• Boric acid + sodium carbonate

• (pH 5-9)

Gifford Buffer Formula and pH Range

• Salts of sodium phosphate + Sodium Chloride (NaCl)

• (pH 6-8)

Sorensen Buffer Formula and pH Range

Phosphate Buffered Saline (PBS)

Sorensen Buffer is also known as _____?

• Boric acid + Sodium borate + Sodium Chloride (NaCl)

• (pH 7-9)

Palitzsch buffer formula and pH Range

HCl and KCl

Clark-Lubs Mixture Formula of pH = 1.2-2.2

HCl and potassium hydrogen phthalate (KHC₈H₄O₄)

Clark-Lubs Mixture Formula of pH = 2.2-4.0

Sodium Hydroxide (NaOH) and potassium hydrogen phthalate (KHC₈H₄O₄)

Clark-Lubs Mixture Formula of pH = 4.2-5.8

Sodium Hydroxide (NaOH) and Potassium dihydrogen phosphate (KH₂PO₄)

Clark-Lubs Mixture Formula of pH = 5.8-8

Boric acid (H₃BO₃), Sodium Hydroxide (NaOH) , and Potassium chloride (KCl)

Clark-Lubs Mixture Formula of pH = 8.0- 10.0

1. Select a weak acid having pKa

2. Calculate the molar ratio of salt and weak acid.

3. Concentration of individual salt and acid of 0.05 to 0.5 M is sufficient.

4. Other factors: stability, compatibility, sterility, availability, safety, cost

5. Determine the pH and !. Adjust if necessary.

General Procedure for Preparing:

True

[T/F] Buffers work best when the pH is close to the pKa of the weak acid or weak base

0.05- 0.5

Conc. range of salt and acid = ____ ?

Colligative Properties

_____- are properties of solutions that depend mainly on the number rather than nature of the constituents

False ; Colligative Properties have 4 properties

[T/F] Colligative Properties have 3 properties

• Vapor Pressure Lowering

• Boiling Point Elevation

• Freezing Point Depression

• Osmotic Pressure

Four Colligative Properties such as ___ [4]

increase BP

Pure solution + non volatile = ____[increase/decrease] BP

decrease VP

increase BP = ____[increase/decrease] VP

decrease VP

Pure solution + non volatile = ____[increase/decrease] VP

LESS

The vapor pressure of a solution is ____ (more/less) than the pure solvent when non-volatile solute is added

Raoult's Law

Vapor Pressure Lowering is expressed by ___________ Law which states that the addition of non-volatile solute lowers the VP of pure water.

Raoult’s Law

____ - states that the addition of non-volatile solute lower the VP of pure water.

• Dalton

• Raoult

___ [who] = partial pressure

____[who] = partial vapor pressure

Dissociation Factor

For ELECTROLYTES, multiply the calculated values of colligative properties by its ______?

Increase

There will be an _____ (decrease/increase) in 100 deg C of pure water when a non-volatile solute is added forming a solution.

Molal elevation constant (Ebullioscopic constant)

Boiling Point Elevation:

• Kb is called the ___?

0.513 deg Kg/mol

Ebullioscopic constant of water is ___ ?

100 deg C

What is the BP of water ?

Ebullioscopic constant

Molal elevation constant (Kb) is aka ___?

Decrease

In Freezing point depression:

• There is always a _____ [decrease/increase] in the temperature for the freezing point of the solution compared to that for pure water whenever nonvolatile solute is added

Molal depression constant (Cryoscopic constant)

In Freezing point depression:

• Kf is called the _____?

Cryoscopic constant

Molal depression constant (Kf) is aka ____?

1.86 deg Kg/mol

Molal depression Constant (Cryoscopic constant) for water is ____?

Osmotic Pressure

____- is the pressure that results from osmosis

Osmosis

____- is the diffusion of the solvent through a semi-permeable membrane that allows only the solvent to pass through it.

• diffusion

• osmosis

• ___- solute is the one moving

• ____ - solvent is the one moving

Low to High conc.

Osmosis = ___ [Low to high or High to Low] ?

Isotonic Solution

[KIND OF SOLUTION] ____ - is a solution administered in the body

True

[T/F] In addition to carrying pH adjustment, pharmaceutical solutions that are meant for application to delicate membranes of the body should also be adjusted to approximately the same osmotic pressure with the body fluids.

Nasal Saline Solution (NSS) 0.9%

____ - is the standard isotonic solution

0.9%

What is the Percentage of Sodium Chloride (NaCl) that is considered to be isotonic with RBCs?

• Isotonic Solution

• Hypertonic Solutions

• Hypotonic Solutions

Type of Solutions [3]

Isotonic Solution

[Type of Solutions]

___-

• Causes no swelling or no contraction of tissues

• Has the same salt concentration, hence same osmotic pressure as the RBCs

a. Isotonic solution

0.9% NaCl solution Normal Saline Solution (NSS) is an Example of what Type of solution?

a. Isotonic solution

b. Hypertonic solution

c. Hypertonic solution

Hypertonic

[Type of Solutions]

____-

• This type of tonicity causes outward passage (Shrinkage/Crenation)

• > 0.9% NaCl

Hypotonic

[Type of Solutions]

_____-

• This type of tonicity causes leads to bursting (Hemolysis)

• inside is more diluted and concentrated

• < 0.9% NaCl

Isotonicity Value

___-refers to the concentration of aqueous NaCl solution having the same colligative properties as the solution in question.

1. Hemolytic Method

2. Colligative Properties

Measurement of Tonicity [2]

Hemolytic Method

[Measurement of Tonicity]

____-

• based on appearance of RBCs

  • when hypotonic → liberates oxyhemoglobin

Colligative Properties

[Measurement of Tonicity]

___-

• based on slight differences in vapor pressure, freezing point or boiling point

Class I

[Class I vs Class II]

• Cryoscopic Method

Class I

[Class I vs Class II]

• Addition / Adjust of Solute

Class I

[Class I vs Class II]

• Sodium chloride (NaCI) Equivalent Method

Class I

[Class I vs Class II]

• Freezing Point Depression

Class II

[Class I vs Class II]

• Addition/ Adjust of Solvent (water) then isotonic solution

Class II

[Class I vs Class II]

• White-Vincent Method

Class II

[Class I vs Class II]

• Sprowls Method

• Cryoscopic method

• Freezing point depression

D methods of adjusting tonicity (2)

Sodium Chloride (NaCl) Equivalent method

E method of adjusting tonicity [1]

Tonic equivalent

The Sodium chloride (NaCI) equivalent (E) of a drug is aka ___?

Sodium Chloride Equivalent (E)

____- refer to the amount of Sodium Chloride (NaCl) that is equivalent to 1 gram of the drug

1.9

[L-iso value]

• Nonelectrolytes = ___ ?

2

[L-iso value]

• Weak electrolytes = ___ ?

2

[L-iso value]

• Di-divalent electrolytes = ____ ?

3.4

[L-iso value]

• Uni-univalent electrolytes = ___ ?

4.3

[L-iso value]

• Uni-divalent electrolytes = ___ ?

4.8

[L-iso value]

• Di-univalent electrolytes =____ ?

5.2

[L-iso value]

• Uni-trivalent electrolytes = ___ ?

6

[L-iso value]

• Tri-univalent electrolytes = ___ ?

7.6

[L-iso value]

• Tetraborate electrolytes = ___?