Pharmaceutical calculation Chapter 11 Isotonic solutions B.Pharmacy 1st Semester 2023 (2022-2023) Previous Year's Question Papers/Notes Download - HK Technical PGIMS

Pharmaceutical calculation
Chapter 11
Isotonic solutions
Assistant Prof. Dr. Wedad K. Ali
Introduction
• When a solvent passes through a semipermeable membrane from a dilute solution
into a more concentrated one, the
concentrations become equalized and the
phenomenon is known as osmosis.
• The pressure responsible for this phenomenon
is termed osmotic pressure and varies with
the nature of the solute.
Osmosis
• If the solute is a nonelectrolyte, its solution contains only molecules
and the osmotic pressure varies with the concentration of the
solute.
• If the solute is an electrolyte, its solution contains ions and the
osmotic pressure varies with both the concentration of the solute
and its degree of dissociation.
• Thus, solutes that dissociate present a greater number of particles
in solution and exert a greater osmotic pressure than undissociated
molecules.
• Like osmotic pressure, the other colligative properties of solutions,
vapor pressure, boiling point, and freezing point, depend on the
number of particles in solution. Therefore, these properties are
interrelated and a change in any one of them will result in a
corresponding change in the others.
• Two solutions that have the same osmotic pressure are termed
isosmotic.
• Many solutions intended to be mixed with body fluids are designed
to have the same osmotic pressure for greater patient comfort,
efficacy, and safety.
• A solution having the same osmotic pressure as a specific body fluid
is termed isotonic (meaning of equal tone) with that specific body
fluid.
• Solutions of lower osmotic pressure than that of a body fluid are
termed hypotonic, whereas those having a higher osmotic pressure
are termed hypertonic.
• Pharmaceutical dosage forms intended to be added directly to the
blood or mixed with biological fluids of the eye, nose, and bowel
are of principal concern to the pharmacist in their preparation and
clinical application.

Special Clinical Considerations of
Tonicity
• It is generally accepted that for ophthalmic and
parenteral administration, isotonic solutions are better
tolerated by the patient than those at the extremes of
hypo- and hypertonicity.
• With the administration of an isotonic solution, there
is a homeostasis with the body’s intracellular fluids.
Thus, in most instances, preparations that are isotonic,
or nearly so, are preferred.
• However, there are exceptions, as in instances in which
hypertonic solutions are used to ‘‘draw’’ fluids out of
edematous tissues and into the administered solution.
• Most ophthalmic preparations are formulated to be isotonic, or
approximately isotonic, to duplicate ophthalmic tears for the
comfort of the patient.
• These solutions are also prepared and buffered at an appropriate
pH, both to reduce the likelihood of irritation to the eye’s tissues
and to maintain the stability of the preparations.
• Injections that are not isotonic should be administered slowly and
in small quantities to minimize tissue irritation, pain, and cell fluid
imbalance. The tonicity of small-volume injections is generally
inconsequential when added to large-volume parenteral infusions
because of the presence of tonic substances, such as sodium
chloride or dextrose in the large-volume infusion, which serve to
adjust the tonicity of the smaller added volume.
• Intravenous infusions, which are hypotonic or hypertonic,
can have profound adverse effects because they generally
are administered in large volumes.
• Large volumes of hypertonic infusions containing dextrose,
for example, can result in hyperglycemia, osmotic diuresis,
and excessive loss of electrolytes.
• Excess infusions of hypotonic fluids can result in the
osmotic hemolysis of red blood cells and surpass the upper
limits of the body’s capacity to safely absorb excessive
fluids. Even isotonic fluids, when infused intravenously in
excessive volumes or at excessive rates, can be deleterious
due to an overload of fluids placed into the body’s
circulatory system.

Physical/chemical considerations in
the preparation of isotonic solutions
• The calculations involved in preparing isotonic
solutions may be made in terms of data relating
to the colligative properties of solutions.
• Theoretically, any one of these properties may be
used as a basis for determining tonicity.
Practically and most conveniently, a comparison
of freezing points is used for this purpose. It is
generally accepted that - 0.52°C is the freezing
point of both blood serum and lacrimal fluid.
• When one gram molecular weight of any
nonelectrolyte, that is, a substance with negligible
dissociation, such as boric acid, is dissolved in
1000 g of water, the freezing point of the solution
is about 1.86 °C below the freezing point of pure
water.
• By simple proportion, therefore, we can calculate
the weight of any nonelectrolyte that should be
dissolved in each 1000 g of water if the solution is
to be isotonic with body fluids.
• Boric acid, for example, has a molecular weight of
61.8; thus (in theory), 61.8 g in 1000 g of water
should produce a freezing point of - 1.86°C.
Therefore:
 x = 17.3 g
• In short, 17.3 g of boric acid in 1000 g of water, having a weight-in-volume
strength of approximately 1.73%, should make a solution isotonic with
lacrimal fluid.
• With electrolytes, the problem is not so simple. Because osmotic pressure
depends more on the number than on the kind of particles, substances
that dissociate have a tonic effect that increases with the degree of
dissociation; the greater the dissociation, the smaller the quantity
required to produce any given osmotic pressure.
• If we assume that sodium chloride in weak
solutions is about 80% dissociated, then each 100
molecules yields 180 particles, or 1.8 times as
many particles as are yielded by 100 molecules of
a nonelectrolyte.
• This dissociation factor, commonly symbolized by
the letter i, must be included in the proportion
when we seek to determine the strength of an
isotonic solution of sodium chloride (m.w. 58.5):
 x = 9.09 g
• Hence, 9.09 g of sodium chloride in 1000 g of
water should make a solution isotonic with
blood or lacrimal fluid. In practice, a 0.90%
w/v sodium chloride solution is considered
isotonic with body fluids. Simple isotonic
solutions may then be calculated by using this
formula:
• The value of i for many a medicinal salt has
not been experimentally determined. Some
salts (such as zinc sulfate, with only some 40%
dissociation and an i value therefore of 1.4)
are exceptional, but most medicinal salts
approximate the dissociation of sodium
chloride in weak solutions. If the number of
ions is known, we may use the following
values, lacking better information:
• Nonelectrolytes and substances of slight
dissociation: 1.0
• Substances that dissociate into 2 ions: 1.8
• Substances that dissociate into 3 ions: 2.6
• Substances that dissociate into 4 ions: 3.4
• Substances that dissociate into 5 ions: 4.2
• A special problem arises when a prescription directs us to
make a solution isotonic by adding the proper amount of
some substance other than the active ingredient or
ingredients. Given a 0.5% w/v solution of sodium chloride,
we may easily calculate that
 0.9 g - 0.5 g = 0.4 g of additional sodium chloride that
should be contained in each 100 mL if the solution is to be
made isotonic with a body fluid.
• But how much sodium chloride should be used in preparing
100 mL of a 1% w/v solution of atropine sulfate, which is to
be made isotonic with lacrimal fluid? The answer depends
on how much sodium chloride is in effect represented by
the atropine sulfate.
• The relative tonic effect of two substances—that is, the
quantity of one that is the equivalent in tonic effects to a
given quantity of the other—may be calculated if the
quantity of one having a certain effect in a specified
quantity of solvent is divided by the quantity of the other
having the same effect in the same quantity of solvent.
• For example, we calculated that 17.3 g of boric acid per
1000 g of water and 9.09 g of sodium chloride per 1000 g of
water are both instrumental in making an aqueous solution
isotonic with lacrimal fluid.
• If, however, 17.3 g of boric acid are equivalent in tonicity to
9.09 g of sodium chloride, then 1 g of boric acid must be
the equivalent of 9.09 g ÷ 17.3 g or 0.52 g of sodium
chloride. Similarly, 1 g of sodium chloride must be the
‘‘tonicic equivalent’’ of 17.3 g ÷ 9.09 g or 1.90 g of boric
acid.
• We have seen that one quantity of any substance
should in theory have a constant tonic effect if
dissolved in1000 g of water:1 g molecular weight of the
substance divided by its i or dissociation value. Hence,
the relative quantity of sodium chloride that is the
tonicic equivalent of a quantity of boric acid may be
calculated by these ratios:
 and we can formulate a convenient rule: quantities of
two substances that are tonicic equivalents are
proportional to the molecular weights of each
multiplied by the i value of the other.
• To return to the problem involving 1 g of atropine sulfate
in 100 mL of solution:
• Molecular weight of sodium chloride = 58.5; i = 1.8
• Molecular weight of atropine sulfate = 695; i = 2.6
 x = 0.12 g of sodium chloride
represented by 1 g of atropine sulfate
• Because a solution isotonic with lacrimal fluid should
contain the equivalent of 0.90 g of sodium chloride in
each 100 mL of solution, the difference to be added must
be 0.90 g - 0.12 g = 0.78 g of sodium chloride.

• Table 11.1 gives the sodium chloride equivalents
(E values) of each of the substances listed. These
values were calculated according to the rule
stated previously. If the number of grams of a
substance included in a prescription is
multiplied by its sodium chloride equivalent, the
amount of sodium chloride represented by that
substance is determined.
• The procedure for the calculation of isotonic
solutions with sodium chloride equivalents may
be outlined as follows:
• Step 1. Calculate the amount (in grams) of sodium chloride
represented by the ingredients in the prescription. Multiply the
amount (in grams) of each substance by its sodium chloride
equivalent.
• Step 2. Calculate the amount (in grams) of sodium chloride, alone,
that would be contained in an isotonic solution of the volume
specified in the prescription, namely, the amount of sodium
chloride in a 0.9% solution of the specified volume. (Such a solution
would contain 0.009 g/mL.)
• Step3.Subtract the amount of sodium chloride represented by the
ingredients in the prescription (Step 1) from the amount of sodium
chloride, alone, that would be represented in the specific volume of
an isotonic solution (Step 2). The answer represents the amount (in
grams) of sodium chloride to be added to make the solution
isotonic.
• Step 4. If an agent other than sodium chloride, such as boric acid,
dextrose, or potassium nitrate, is to be used to make a solution
isotonic, divide the amount of sodium chloride (Step 3) by the
sodium chloride equivalent of the other substance.
Example Calculations of the i Factor
• Zinc sulfate is a 2-ion electrolyte, dissociating 40% in a certain
concentration. Calculate its dissociation (i) factor.
• On the basis of 40% dissociation, 100 particles of zinc sulfate
will yield:
 40 zinc ions
 40 sulfate ions
60 undissociated particles
or 140 particles
• Because140 particles represent 1.4 times as many particles as
were present before dissociation, the dissociation (i) factor is
1.4, answer.
• Zinc chloride is a 3-ionelectrolyte,dissociating
80% in a certain concentration. Calculate its
dissociation (i) factor. On the basis of 80%
dissociation, 100 particles of zinc chloride will
yield:
 80 zinc ions 80 chloride ions
 80 chloride ions
 20 undissociated particles
 or 260 particles
 Because 260 particles represents 2.6 times as
many particles as were present before
dissociation, the dissociation (i) factor is 2.6,
answer.
Example Calculations of the Sodium Chloride Equivalent
• The sodium chloride equivalent of a substance
may be calculated as follows:
• Papaverine hydrochloride (m.w. 376) is a 2-ion
electrolyte, dissociating 80% in a given
concentration.
• Calculate its sodium chloride equivalent.
 Because papaverine hydrochloride is a 2-ion
electrolyte, dissociating 80%, its i factor is 1.8.
• Calculate the sodium chloride equivalent for glycerin,
a nonelectrolyte with a molecular weight of 92.2
• Glycerin, i factor = 1.0
• Calculate the sodium chloride equivalent for timolol
maleate, which dissociates into two ions and has a
molecular weight of 432.2
• Timolol maleate, i factor = 1.8
• Calculate the sodium chloride equivalent for
fluorescein sodium, which dissociates into
three ions and has a molecular weight of
376.2
 Fluorescein sodium, i factor = 2.6
Example Calculations of Tonicic Agent Required
How many grams of sodium chloride should be used in compounding the
following prescription?
Rx Pilocarpine Nitrate 0.3 g
 Sodium Chloride q.s.
 Purified Water ad 30 mL
 Make isoton. sol.
 Sig. For the eye.
Step 1.
 0.23 x 0.3 g = 0.069 g of sodium chloride represented by the pilocarpine
nitrate
Step 2.
 30 x 0.009 = 0.270 g of sodium chloride in 30 mL of an isotonic sodium
chloride solution
Step 3.
 0.270 g (from Step 2) - 0.069 g (from Step 1) = 0.201 g of sodium chloride to
be used, answer.
How many grams of boric acid should be used in compounding the following prescription?
Rx Phenacaine Hydrochloride 1%
 Chlorobutanol ½ %
 Boric Acid q.s.
 Purified Water ad 60
 Make isoton. sol.
 Sig. One drop in each eye.
The prescription calls for 0.6 g of phenacaine hydrochloride and 0.3 g of chlorobutanol.
Step 1.
 0.20 x 0.6 g = 0.120 g of sodium chloride represented by phenacaine hydrochloride
 0.24 x 0.3 g = 0.072 g of sodium chloride represented by chlorobutanol
Total: 0.192 g of sodium chloride represented by both ingredients
Step 2.
 60 x 0.009 = 0.540 g of sodium chloride in 60 mL of an isotonic sodium chloride solution
Step 3.
 0.540 g (from Step 2) - 0.192 g (from Step 1) = 0.348 g of sodium chloride required to make
the solution isotonic
But because the prescription calls for boric acid:
Step 4.
0.348 g ÷ 0.52 (sodium chloride equivalent of boric acid) = 0.669 g of boric acid to be used,
answer.
How many grams of potassium nitrate could be used to make the following
prescription isotonic?
Rx Sol. Silver Nitrate 60
 1: 500 w/v
 Make isoton. sol.
 Sig. For eye use.
The prescription contains 0.12 g of silver nitrate.
Step 1.
 0.33 x 0.12 g = 0.04 g of sodium chloride represented by silver nitrate
Step 2.
 60 x 0.009 = 0.54 g of sodium chloride in 60 mL of an isotonic sodium chloride
solution
Step 3.
 0.54 g (from step 2) - 0.04 g (from step 1) 0.50 g of sodium chloride required to
make solution isotonic
Because, in this solution, sodium chloride is incompatible with silver nitrate, the tonic
agent of choice is potassium nitrate. Therefore,
Step 4.
 0.50 g ÷ 0.58 (sodium chloride equivalent of potassium nitrate) = 0.86 g of
potassium nitrate to be used, answer.
How many grams of sodium chloride should be used in compounding the following
prescription?
Rx Ingredient X 0.5
 Sodium Chloride q.s.
 Purified Water ad 50 Make isoton. sol.
 Sig. Eye drops.
Let us assume that ingredient X is a new substance for which no sodium chloride
equivalent is to be found in Table 11.1, and that its molecular weight is 295 and its
i factor is 2.4. The sodium chloride equivalent of ingredient X may be calculated as
follows:
Then, Step 1.
0.26 x 0.5 g= 0.13 g of sodium chloride represented by ingredient X
Step 2.
50 x 0.009 = 0.45 g of sodium chloride in 50 mL of an isotonic sodium chloride
solution
Step 3.
0.45 g (from Step 2) - 0.13 g (from Step 1) = 0.32 g of sodium chloride to be used,
answer.
Using an Isotonic Sodium Chloride Solution to Prepare Other
Isotonic Solutions
A 0.9% w/v sodium chloride solution may be used to compound
isotonic solutions of other drug substances as follows:
Step 1. Calculate the quantity of the drug substance needed to fill the
prescription or medication order.
Step 2. Use the following equation to calculate the volume of water
needed to render a solution of the drug substance isotonic:
Step 3.
Add 0.9% w/v sodium chloride solution to complete the required
volume of the prescription or medication order. Using this method,
determine the volume of purified water and 0.9% w/v sodium
chloride solution needed to prepare 20 mL of a 1% w/v solution of
hydromorphone hydrochloride (E = 0.22).
Step 1.
20 mL x 1% w/v = 0.2 g hydromorphone needed
Step 2.
0.2 g x 0.22 / 0.009 = 4.89 mL purified water required to make an
isotonic solution of hydromorphone hydrochloride, answer.
Step 3.
20 mL- 4.89 mL =15.11 mL 0.9% w/v sodium chloride solution
required, answer.
Proof: 20 mL x 0.9% = 0.18 g sodium chloride or equivalent required
0.2 x 0.22 = 0.044g (sodium chloride represented by 0.2g
hydromorphonehydrochloride)
15.11 mL x 0.9 % = 0.136 g sodium chloride present
0.044 g + 0.136 g = 0.18 g sodium chloride required for isotonicity
Use of Freezing Point Data in Isotonicity Calculations
• Freezing point data ( ΔTf
) can be used in isotonicity
calculations when the agent has a tonicic effect and does
not penetrate the biologic membranes in question (e.g., red
blood cells). As stated previously, the freezing point of both
blood and lacrimal fluid is - 0.52°C. Thus, a pharmaceutical
solution that has a freezing point of -0.52°C is considered
isotonic. Representative data on freezing point depression
by medicinal and pharmaceutical substances are presented
in Table 11.2. Although these data are for solution strengths
of 1% (Δ Tf
1%), data for other solution strengths and for
many additional agents may be found in physical pharmacy
textbooks and in the literature. Freezing point depression
data may be used in isotonicity calculations as shown by
the following.

Example Calculations Using Freezing Point Data
How many milligrams each of sodium chloride and dibucaine hydrochloride are
required to prepare 30 mL of a 1% solution of dibucaine hydrochloride isotonic
with tears?
To make this solution isotonic, the freezing point must be lowered to - 0.52. From
Table 11.2, it is determined that a 1% solution of dibucaine hydrochloride has a
freezing point lowering of 0.08°. Thus,sufficient sodium chloride must be added to
lower the freezing point an additional 0.44° (0.52° - 0.08°).
Also from Table 11.2, it is determined that a 1% solution of sodium chloride lowers the
freezing point by 0.58°.
By proportion:
x = 0.76% (the concentration of sodium chloride needed to lower the freezing point
by 0.44°, required to make the solution isotonic) Thus, to make 30 mL of solution,
30 mL X 1% = 0.3 g = 300 mg dibucaine hydrochloride, and
 30 mL X 0.76% = 0.228 g = 228 mg sodium chloride, answers.
Note: Should a prescription call for more than one medicinal and/or pharmaceutic
ingredient,
thesumofthefreezingpointsissubtractedfromtherequiredvalueindeterminingtheadd
itional lowering required by the agent used to provide isotonicity.