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san4es73 [151]
3 years ago
9

A intramuscular medication is given at 5.00mg/kg of body weight. What is the dose in grams for a 180-lb patient?

Chemistry
2 answers:
Alex17521 [72]3 years ago
7 0
0.408 gram for 180-lb patient
Soloha48 [4]3 years ago
4 0

Answer: 0.408 grams is to given for 180 lb patient.

Explanation:

Given : A intramuscular medication is given at 5.00 mg/kg of body weight.

That is for a body with weight of 1 kg , we have to give 5.00 mg of medication

Converting the mass in kg to pounds

1 kg = 2.20462 lb

Thus for a body with weight of 2.20462 lb , we have to give= 5.00 mg of medication

For body weight of 180 lb ,  we have to give =\frac{5.00}{2.20462}\times 180=408.23mg of medication

Also 1 mg = 0.001 grams

Thus 408.23mg=\frac{0.001}{1}\times 408.23=0.408grams

Thus for a body with weight of 2.20462 lb , we have to give 0.408 grams of medication.

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You determine that it takes 26.0 mL of base to neutralize a sample of your unknown acid solution. The pH of the solution when ex
mojhsa [17]

Answer:

a. 1.78x10⁻³ = Ka

2.75 = pKa

b. It is irrelevant.

Explanation:

a. The neutralization of a weak acid, HA, with a base can help to find Ka of the acid.

Equilibrium is:

HA ⇄ H⁺ + A⁻

And Ka is defined as:

Ka = [H⁺] [A⁻] / [HA]

The HA reacts with the base, XOH, thus:

HA + XOH → H₂O + A⁻ + X⁺

As you require 26.0mL of the base to consume all HA, if you add 13mL, the moles of HA will be the half of the initial moles and, the other half, will be A⁻

That means:

[HA] = [A⁻]

It is possible to obtain pKa from H-H equation (Equation used to find pH of a buffer), thus:

pH = pKa + log₁₀ [A⁻] / [HA]

Replacing:

2.75 = pKa + log₁₀ [A⁻] / [HA]

As [HA] = [A⁻]

2.75 = pKa + log₁₀ 1

<h3>2.75 = pKa</h3>

Knowing pKa = -log Ka

2.75 = -log Ka

10^-2.75 = Ka

<h3>1.78x10⁻³ = Ka</h3>

b. As you can see, the initial concentration of the acid was not necessary. The only thing you must know is that in the half of the titration, [HA] = [A⁻]. Thus, the initial concentration of the acid doesn't affect the initial calculation.

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A chemist measures the amount of hydrogen gas produced during an experiment. She finds that 264. g of hydrogen gas is produced.
Lesechka [4]

Answer:

The answer is 130.953 g of hydrogen gas.

Explanation:

Hydrogen gas is formed by two atoms of hydrogen (H), so its molecular formula is H₂. We can calculate is molecular weight as the product of the molar mass of H (1.008 g/mol):

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