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Mademuasel [1]
3 years ago
15

GenAlex Medical, a leading manufacturer of medical laboratory equipment, is designing a new automated system that can detect nor

mal levels of dissolved triiodothyronine ( to ), using a blood sample that is as small as . Calculate the minimum mass in picograms of triiodothyronine that the new system must be able to detect. Be sure your answer has the correct number of significant digits.
Chemistry
1 answer:
Shkiper50 [21]3 years ago
7 0

Answer:

0.87 pg

Explanation:

<em>GenAlex Medical, a leading manufacturer of medical laboratory equipment, is designing a new automated system that can detect normal levels of dissolved triiodothyronine (230. to 660 pg/dL), using a blood sample that is as small as 380 μL. Calculate the minimum mass in picograms of triiodothyronine that the new system must be able to detect. Be sure your answer has the correct number of significant digits.</em>

Step 1: Convert 380 μL to deciliters

We will use the following conversion factors.

  • 1 L = 10⁶ μL
  • 1 L = 10 dL

380 μL × 1 L/10⁶ μL × 10 dL/1 L = 3.8 × 10⁻³ L

Step 2: Calculate the minimum mass of triiodothyronine that can be found in a 3.8 × 10⁻³ L blood sample

Since we are looking for the minimum mass, we will use the lower limit of the concentration interval (230. pg/dL).

3.8 × 10⁻³ L × 230. pg/dL = 0.87 pg

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In this case, given the dissociation reaction of magnesium fluoride:

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We need to compute the yielded moles of magnesium fluoride, but first we need to identify the limiting reactant for which we compute the available moles of magnesium chloride:

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n_{MgCl_2}^{consumed}=0.5L*1.2x10^{-3}molNaF/L*\frac{1molCaCl_2}{2molNaF} =3x10^{-4}molMgCl_2

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n_{MgF_2}=3x10^{-4}molMgCl_2*\frac{1molMgF_2}{1molMgCl_2}=3x10^{-4}molMgF_2

Next, since the magnesium fluoride to magnesium and fluoride ions is in a 1:1 and 1:2 molar ratio, the concentrations of such ions are:

[Mg^{2+}]=\frac{3x10^{-4}molMg^{+2}}{(0.3+0.5)L} =3.75x10^{-4}M

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Q=(3.75x10^{-4})(7.5x10^{-4})^2=2.11x10^{-10}

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