Response:
Tube 2: 8.26 * 10^-3; Tube 4: 6.83 * 10^-5
Explanation:
For the MIC test's serial dilutions, each tube should contain an equal volume of nutrient broth: 5.0 mL, while the agent's volume per dilution must also match: 0.5 mL.
The serial dilution process followed was:
- Tube 1: 0.5/5.5
- Tube 2: 0.5 mL from tube 1 was diluted with 5.0 mL of broth, resulting in a dilution of tube 2 as (1:11) * (1:11) = (0.5/5.5) * (0.5/5.5) = 1:121 = 8.26 * 10^-3
- Tube 3: similar calculations yield 1:1331 = 7.51 * 10^-4
- Tube 4: yields 1:14641 = 6.83 * 10^-5.
Answer:
The correct choice for your inquiry is option A, Argon.
Explanation:
Isotope Atomic mass Percent (%)
1 35.9675 0.337
2 37.9627 0.063
3 39.9624 99.6
To calculate the average atomic mass: (Mass of isotope 1)(percent of 1) + (Mass of isotope 2)(percent of 2) + (Mass of isotope 3)(percent of 3)
Average atomic mass = (35.9675)(0.00337) + (37.9627)(0.00063) + (39.9624)(0.996)
Average atomic mass = 0.1212 + 0.0239 + 39.8025
Average atomic mass = 39.9476
Theoretical Atomic mass
a) Ar 39.95
b) K 39.10
c) Cl 35.45
d) Ca 40.08
Answer:
The categorization of strong, weak, and non-electrolytes is detailed below, based on the examples presented in the question.
Explanation:
A strong electrolyte fully dissociates or nearly so in an aqueous environment; typically, strong acids, bases, and salts fall under this category. Examples of strong electrolytes include:
- Hydrochloric acid, HCl
- Calcium hydroxide, Ca(OH)2
- Potassium chloride, KCl
A weak electrolytepartially ionizes in solution; weak acids and bases are primary instances. Examples consist of:
- Methylamine, CH3NH2
- Hydrofluoric acid, HF
A non-electrolytedoes not dissociate in an aqueous medium. Examples of non-electrolytes are:
- Sucrose, C12H22O11
- Methanol, CH3OH
