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jenyasd209 [6]
2 years ago
5

our throat is dry, and you want the last cough drop in the box to last a long time in your mouth. What should you do? Keep the c

ough drop whole. This maintains the largest surface-to-volume ratio and slows the dissolution of the cough drop. Break the cough drop into little pieces and put them all in your mouth. Since each little piece must be dissolved separately, the drop will last longer. It doesn't matter if the cough drop is in one piece or many pieces; the total amount of cough drop is all that matters. Break the cough drop into little pieces and put them all in your mouth. This decreases the surface-to-volume ratio and slows the dissolution of the cough drop.
Chemistry
1 answer:
Ann [662]2 years ago
8 0

You should keep the cough drop whole. This maintains the largest surface-to-volume ratio and slows the dissolution of the cough drop.

<h3>Delay of drug action</h3>

The action of the drug can be delayed to either reduce adverse effect if the drugs to the body or to enhance its therapeutic purposes.

Because the throat is dry, the therapeutic purposes of the cough drop would only be achieved if it's dissolution is delayed in the mouth.

To do so, the cough drop should be kept whole to maintain the largest surface-to-volume ratio. This would slow the dissolution of the cough drop.

Learn more about drug here:

brainly.com/question/26254731

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A sample of 0.281 gg of an unknown monoprotic acid was dissolved in 25.0 mLmL of water and titrated with 0.0950 M NaOH NaOH. The
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Answer:

98.6 g/mol.

Explanation:

Equation of the reaction

HX + NaOH--> NaX + H2O

Number of moles = molar concentration × volume

= 0.095 × 0.03

= 0.00285 moles

By stoichiometry, 1 mole of HX reacted with 1 mole of NaOH. Therefore, number of moles of HX = 0.00285 moles.

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5 0
3 years ago
Calculate the volume in liters of a 0.00231M copper(II) fluoride solution that contains 175.g of copper(II) fluoride CuF2. Be su
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Answer:

Volume = 746 L

Explanation:

Given that:- Mass of copper(II) fluoride = 175 g

Molar mass of copper(II) fluoride = 101.543 g/mol

The formula for the calculation of moles is shown below:

moles = \frac{Mass\ taken}{Molar\ mass}

Thus,

Moles= \frac{175\ g}{101.543\ g/mol}

Moles_{copper(II)\ fluoride}= 1.7234\ mol

Also,

Considering:

Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}

So,,

Volume =\frac{Moles\ of\ solute}{Molarity}

Given, Molarity = 0.00231 M

So,

Volume =\frac{1.7234}{0.00231}\ L

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7 0
3 years ago
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