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ivann1987 [24]
3 years ago
14

5. You are investigating an arson scene and you find a corpse in the rubble, but you suspect that the victim did not die as a re

sult of the fire. Instead, you suspect that the victim was murdered earlier, and that the blaze was started to cover up the murder. How would you go about determining whether the victim died before the fire
Chemistry
1 answer:
Marina CMI [18]3 years ago
8 0

Answer:

See the answer below.

Explanation:

Fire has three major components:

  • Heat
  • Smoke
  • Gases ( in form of CO, CO2 etc)

If the victim had died as a result of the fire, he/he would have inhaled smoke and hot gases from the fire. These components would have resulted in traces of burns and soot deposition in the trachea and lungs as well as traces of CO in the blood of the victim.

If the analysis of the victim's corpse does not reflect some of the results above, it can be effectively concluded that the victim has been dead before the fire.

<em>The single most important indicator of death by the fire would be the presence of CO in the blood of the victim's corpse. All others might be to a less significant degrees.</em>

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When the fish-tank water has a pH of 8.0, the hydronium ion concentration is 1.0 × 10-8 mole per liter. What is the hydronium io
Oduvanchick [21]
You must know and use the formula for pH.


pH = - log [H3O+], where [H3O+] is the molar concentration of hydronium ion.


So, when pH is 8.0 => 8.0 = - log [H3O+] and you can use antilogarithm (the inverse function of logarithm) to find [H3O+], in this way:


[H3O+] = 10^-8 = 1 * 10 ^-8 M


When, pH = 7.0 =>

7.0 = - log [H3O+] => [H3O+] = 1 * 10^ -7 M


Answer: 1*10^-7 mole / liter
5 0
3 years ago
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nydimaria [60]

Answer: iss as kfnandn

Explanation:

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3 years ago
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Melting points of molecular solids are lower than melting points of ionic compounds 
5 0
3 years ago
Read 2 more answers
Identify the conjugate acid/base pairs in each of the following equations:
Valentin [98]

Answer:

(a) Pair 1: H₂S and HS⁻

    Pair 2: NH₃ and NH₄⁺

(b) Pair 1: HSO₄⁻ and SO₄⁻

    Pair 2: NH₃ and NH₄⁺

(c) Pair 1: HBr and Br⁻

    Pair 2: CH₃O⁻ and CH₃OH

(d)  Pair 1: HNO₃ and NO₃⁻

     Pair 2: H₃O⁺

Explanation:

When an acid loses its proton (H⁺), a conjugate base is produced.

When a base accepts a proton (H⁺), it forms a conjugate acid.

(a) H₂S is an acid. When it loses a proton, it forms the conjugate base HS⁻.

    NH₃ is a base. When NH₃ gains a proton, it forms the conjugate acid NH₄⁺

(b) The acid HSO₄⁻ loses a H⁺ ion and forms the conjugate base SO₄²⁻.

     The base NH₃ accepts a H⁺ ion to form the conjugate acid NH₄⁺.

(c) HBr is an acid. When loses the H⁺ ion, it forms the conjugate base Br⁻.

   CH₃O⁻ accepts a H⁺ ion to form the conjugate acid CH₃OH.

(d) HNO₃ loses a proton to form the conjugate base NO₃⁻.

    H₂O gains a proton to form the conjugate acid H₃O⁺.

6 0
3 years ago
6. What is the oxidation number for the atom indicated in the following compounds.
Hatshy [7]

Answer:

a. +6;

b. +5;

c. +3.

Explanation:

Start with elements with well-known oxidation states.

The oxidation state on oxygen O in compounds is mostly -2. Common exceptions include:

  • -1 in peroxides and
  • positive when oxygen bonds to fluorine.

The oxidation state on group 1 metals (Li, Na, K, etc.) in compounds is mostly +1.

The oxidation state on group 2 metals (Be, Mg, Ca, etc.) in compounds is mostly +2.

Barium Ba is a group 2 metal. The oxidation state on Ba in the compound BaSO₄ is expected to be +2.

The oxidation state on hydrogen H in compounds is mostly +1. The oxidation state on H might be negative when it is bonded to metals.  

The oxidation state on halogens (F, Cl, Br, etc.) is mostly -1. The oxidation state may vary when the halogen is bonded to oxygen or another halogen element.

Compounds are neutral. The oxidation state on all atoms in a compound shall add up to 0. Both BaSO₄ and HClO₂ are neutral.

<h3>BaSO₄</h3>

Oxidation states:

  • Ba: +2;
  • The oxidation state on sulfur S is to be determined;
  • O: -2.

Let the oxidation state on S be x.

2 + x + 4 × (-2) = 0;

x = 6.

Hence, the oxidation state on S in BaSO₄ is +6.

<h3>HClO₂</h3>

Oxidation states:

  • H: +1;
  • Cl here is bonded to oxygen. The oxidation state on chlorine Cl is to be determined;
  • O: -2.

Let the oxidation state on Cl be x.

<em>Refer to the equation in BaSO₄ as an example. Try setting up the equation on your own. </em>

x = 3.

Hence, the oxidation state on Cl is +3.

<h3>PO₄³⁻</h3>

Ions carry charge. Oxidation states on atoms in an ion shall add up to the charge of the ion. The superscript of an ion shows its charge. The superscript 3- in the phosphate ion shows that the ion carries a charge of -3.

Oxidation states:

  • The oxidation state on P is to be found;
  • O: -2.

Let the oxidation state on P be x.

x + 4 × (-2) = -3;

x = 5.

Hence, the oxidation state on P is +5.

4 0
3 years ago
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