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Pharmacy Practice Lab > Lab 7 > Flashcards

Lab 7 Flashcards

1
Q

common adverse effects observed in electrolyte formulations are related to what?

A

the high osmolarity (or osmolality) and/or local irritant effects

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2
Q

many drugs and excipients are ____ in the presence of electrolytes and minerals, resulting in _____

A

INCOMPATIBLE, resulting in PRECIPITATION

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3
Q

electrolyte solutions containing sodium, potassium salts of chloride and/or citrate are used to do what?

A

replenish electrolyte loss that results from dehydration and use of certain diuretics

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4
Q

electrolyte solutions can be prepared as ___ or as ____

A

powders for reconstitution or as concentrated solutions

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5
Q

highly hypertonic ORAL preparations must be …………. before administration to avoid _______

A

must be dissolved or diluted with the appropriate quantity of water before administration to avoid GI EFFECTS

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6
Q

hypertonic PARENTERAL solutions must be…………to avoid ………

A

must be diluted appropriately with IV fluids OR should be administered via large veins (ie: superior vena cava) to avoid LOCAL TISSUE IRRITATION AND OTHER ADVERSE EVENTS

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7
Q

____ can occur when highly concentrated electrolyte solutions are mixed with some drugs

A

incompatibilities such as PRECIPITATION and DEGREDATION

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8
Q

osmotic pressure is defined as….

A

pressure exerted by the molecules and ions present in solution on the SEMIPERMEABLE MEMBRANE

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9
Q

osmotic pressure is dependent on…

A

the number of dissolved particles (molecules and ions) in solution

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10
Q

what can you say about the osmotic pressure of NON electrolytes vs electrolytes

A

non-electrolytes do not dissociate.
therefore, the number of particles that affect osmotic pressure is DIRECTLY and only related to the number of moles

in the case of electrolytes, they dissociate into ions. therefore, osmotic pressure depends on IONIC CONCENTRATION

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11
Q

electrolytes dissociate into ions. therefore, osmotic pressure depends on ionic concentration

how is the ionic concentration calculated ??

A

using the percentage dissociation and molar concentration of the solutions

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12
Q

do insoluble ingredients (suspended in the solution) exert osmotic pressure?

A

NO

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13
Q

osmotic pressure is recorded in terms of ___ or ___

A

osmolarity or osmolality

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14
Q

define osmolarity

A

the concentration of osmotically active particles (molecules, ions) per unit VOLUME of SOLUTION (L)

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15
Q

define osmolality

A

the concentration of osmotically active particles (molecules, ions) per unit MASS (kg) of SOLVENT

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16
Q

true or false

mass does not change with temperature

A

true

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17
Q

true or false

volume does not change with temperature

A

FALSE — volume does change with temperature

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18
Q

which is more reliable —

osmolarity or osmolality

A

OSMOLALITY VALUES ARE MORE RELIABLE

this is so because volume changes with temperature while mass does not

19
Q

when are osmolarity and osmolality values used interchangeably?

A

when the density of the pharmaceutical solution is approximately 1

20
Q

substances that are NOT completely dissociated have a _____ osmotic pressure than those that are 100% dissociated.

WHY

A

substances that are NOT completely dissociated have a LOWER osmotic pressure than those that are 100% dissociated

this is so because the number of ions (particles) in the product is higher in those substances that are 100% dissociated

21
Q

tonicity is the measure of…..

A

the osmotic pressure gradient between 2 solutions separated by a semipermeable membrane

22
Q

TONICITY IS ONLY INFLUENCED BY…

A

solutes that cannot cross the semipermeable (plasma) membrane

23
Q

water readily diffuses through the plasma membrane.
why?

A

to maintain osmotic equilibrium on either side of the membrane

24
Q

in a cell, water moves in and out of the cell between the ___ and the ____ to maintain the osmotic pressure

A

ECF (extracellular fluid) and ICF (intracellular fluid)

25
Q

the normal osmolality of ICF and blood plasma ranges between____ -_____ mOsm/kg

A

285-290

26
Q

a solution is isotonic when…

A

its osmolality is similar to that of blood plasma

27
Q

when the solution is isotonic, explain the movement of water

A

the movement of water across the cell membrane is at equilibrium and the cell volume and size does not change significantly

28
Q

a solution is hypertonic when….

A

its osmolality is higher than that of blood plasma

water from the cell moves into the solution and the cell decreases in volume and size.
the cell will crenate

29
Q

a solution is hypotonic when…

A

its osmolality is lower than that of blood plasma

water from the solution moves into the cell and the cell increases in volume and size. the cell will eventually burst (hemolysis)

30
Q

what can contribute to osmotic pressure and tonicity of a pharmaceutical preparation?

A

both the API and the excipients

31
Q

hypertonic oral solutions can present issues such as ___ and _____

give examples of specific components that cause these issues

A

gastric intolerance (sorbitol and iron)

and osmotic diarrhea (sorbitol and glycerin)

32
Q

hypertonic injectable solutions can cause..

A

local irritation, thrombophlebitis, and hemolysis

33
Q

what is the osmolar range for the GI tract?

A

127-357 mOsm/kg

34
Q

what buffers the medication to a safe pH and osmolar range before it reaches the duodenum?

(therefore, for oral solutions less than 700mOsm, there is no serious problem)

A

saliva, mucus, and gastric juices

35
Q

what organ is exceptionally sensitive to hypertonic solutions and osmolar loads?

A

the small intestine

36
Q

osmotic diarrhea results due to what?

A

the movement of water into the gut

37
Q

oral solutions greater than ____mOsm/kg should not be administered undiluted

A

2000mOsm/kg

38
Q

what are minerals? give 2 examples

A

minerals are macronutrients essential for body function
ex: iron, calcium

39
Q

many mineral supplements are available OTC.
the content of these elements in the preparation must be expressed in terms of the elemental content.
WHY?

A

to avoid dosing errors

40
Q

an EQUIVALENT of an element is…

A

the number of moles of the element that combine with 1 mole of hydrogen

41
Q

the number of equivalents in an element or compound is calculated using ___ or ____

A

valency or chemical reaction

42
Q

true or false

the number of equivalents present in the element is generally equal to its valency

A

true

43
Q

the number of equivalents present in the COMPUND is generally equal to…..

A

the highest valency in the molecule

44
Q
A

Pharmacy Practice Lab (10 decks)

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