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2 years ago

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Your patient gets a prescription for 51.5 mcg (micrograms, μg) of digoxin in liquid form. The label reads 0.0250 mg/mL. How many

milliliters of digoxin should you give?

1 answer:

Savatey [412]2 years ago

4 0

Taking into account the definition of density, the volume of digoxin should be 2.06 mL.

<h3>Definition of density</h3>

Density is defined as the property that matter, whether solid, liquid or gas, has to compress into a given space and allows us to measure the amount of mass in a certain volume of a substance.

So, the expression for the calculation of density is the quotient between the mass of a body and the volume it occupies:

density= mass÷ volume

You can observe that density is inversely proportional to volume: the smaller the volume occupied by a given mass, the higher the density.

<h3>Volume of digoxin</h3>

In this case, you know that:

Density= 0.0250 mg/mL
Mass= 51.5 micrograms= 0.0515 mg (being 1 micrograms= 0.001 mg)

Replacing in the definition of density:

0.0250 mg/mL= 0.0515 mg÷ volume

Solving:

0.0525 mg= 0.0250 mg/mL ×volume

volume= 0.0515 mg÷ 0.0250 mg/mL

<u><em>volume= 2.06 mL</em></u>

In summary, the volume of digoxin should be 2.06 mL.

Learn more about density:

brainly.com/question/952755

brainly.com/question/1462554

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A chemist measures the amount of iodine solid produced during an experiment. she finds that 1.6 g of iodine solid is produced. c

Yakvenalex [24]

Mass of iodine solid produced = 1.6 g

Iodine solid has a molecular formula : I2

Atomic mass of iodine = 126.904 g/mol

Therefore, molar mass of I2 solid = 2* 126.904 = 253.808 g/mol

Number of moles of a given substance is the ratio of its mass to the molar mass

# moles of I2 solid = mass of I2 solid/molar mass = 1.6 g/253.808 = 0.00630 moles

Hence, the # moles of iodine solid produced is 0.00630 moles

3 0

4 years ago

A sample of argon gas is at a pressure of 1.725x10^4 kPa and a temperature of 24°C in a rigid 20 L tank. How many moles of argon

Paraphin [41]

To find how many moles of the gas you can use ideal gas formula. Remember to change the temperature unit to Kelvin. Since the pressure using kpa, the constant used would be 8.314 kpa*L / mol*K
PV=nRT
n= PV/RT
n= 17,250 kpa * 20 / 8.314 * (24+273.15)K
n=139.64moles

4 0

4 years ago

Calculate the maximum solubility of silver carbonate, Ag2CO3 in g/L when in the presence of 0.057 M AgNO3. The solubility produc

Andreyy89

Answer:

Approximately $4.2 \times 10^{-7}\; \rm g \cdot L^{-1}$ .

Explanation:

Start by finding the concentration of $\rm Ag_2CO_3$ at equilibrium. The solubility equilibrium for

$\rm Ag_2CO_3 \; (s) \rightleftharpoons 2\, Ag^{+}\; (aq) + {CO_3}^{2-}\; (aq)$ .

The ratio between the coefficient of $\rm Ag_2CO_3$ and that of $\rm Ag^{+}$ is $1:2$ . For

Let the increase in $\rm {CO_3}^{2-}$ concentration be $+x\; \rm mol \cdot L^{-1}$ . The increase in $\rm Ag^{+}$ concentration would be $+2\,x\; \rm mol \cdot L^{-1}$ . Note, that because of the $0.057\; \rm mol \cdot L^{-1}$ of $\rm AgNO_3$ , the concentration of

The concentration of $\rm Ag^{+}$ would be $(0.057 + 2\, x) \; \rm mol\cdot L^{-1}$ .
The concentration of $\rm {CO_3}^{2-}$ would be $x\; \rm mol \cdot L^{-1}$ .

Apply the solubility product expression (again, note that in the equilibrium, the coefficient of $\rm Ag^{+}$ is two) to obtain:

$\begin{aligned}&\rm \left[Ag^{+}\right]^2 \cdot \left[{CO_3}^{2-}\right] = K_{\text{sp}} \\ & \implies (0.057 + x)^2\cdot x = 8.1 \times 10^{-12} \end{aligned}$ .

Note, that the solubility product of $\rm Ag_2CO_3$ , $K_{\text{sp}} = 8.1 \times 10^{-12}$ is considerably small. Therefore, at equilibrium, the concentration of

Apply this approximation to simplify $(0.057 + x)^2\cdot x = 8.1 \times 10^{-12}$ :

$0.057^2\, x \approx (0.057 + x)^2 \cdot x = 8.1 \times 10^{-12}$ .

$\begin{aligned} x &\approx \frac{8.1 \times 10^{-12}}{0.057^2}\end{aligned}$ .

Calculate solubility (in grams per liter solution) from the concentration. The concentration of $\rm Ag_2CO_3$ is approximately $\displaystyle \frac{8.1 \times 10^{-12}}{0.057^2}\; \rm mol\cdot L^{-1}$ , meaning that there are approximately $\displaystyle n = \frac{8.1 \times 10^{-12}}{0.057^2}\; \rm mol$ of

$\begin{aligned}m &= n \cdot M \\ &\approx \displaystyle \frac{8.1 \times 10^{-12}}{0.057^2} \; \rm mol\times 167.91\; g \cdot mol^{-1} \\ &\approx 4.2 \times 10^{-7}\; \rm g \end{aligned}$ .

As a result, the maximum solubility of $\rm Ag_2CO_3$ in this solution would be approximately $4.2 \times 10^{-7}\; \rm g \cdot L^{-1}$ .

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3 years ago

A)How many moles of O2 are required for the complete combustion of 2.2 g of C3H8 to form CO2 and H2O?

Oksana_A [137]

<span>A)How many moles of O2 are required for the complete combustion of 2.2 g of C3H8 to form CO2 and H2O?

C3H8 + 5O2 = 3CO2 + 4H2O

2.2 g C3H8 ( 1 mol / 44.11 mol ) ( 5 mol O2 / 1 mol C3H8) = 0.25 mol O2

b)A 65.25 g sample of CuSO4•5H2O (M = 249.7) is dissolved in enough water to make 0.800 L of solution. What volume of this solution must be diluted with water to make 1.00 L of 0.100 M CuSO4?

M1V1 = M2V2
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3 years ago

Which of the following is a characteristic of mixtures? A. Mixtures can only be in solid and liquid form. B. Substances that are

Taya2010 [7]

The correct choice is B.

Mixtures retain their properties because science has proven it. Take a bag of trail mix for example. Those raisins and marshmallows and m&m’s can each be separated. When you take them out, they keep their same texture.

Is not correct because mixtures can be solids (Trail mix is one example)

Correct

Is not correct because sometimes it cannot be seen (Lemonade powder and water is one example)

Is not correct because trail mix is an example.

5 0

3 years ago