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Pani-rosa [81]
2 years ago
15

PLZ HELP, GIVING BRAINLIEST!!

Chemistry
1 answer:
Pani-rosa [81]2 years ago
6 0

Answer:

C. 2.000 M C6H12O6

Explanation:

Let us obtain the molarity of the solution.

Molar Mass of C6H12O6 = (12x6) + (12x1) + (16x6) = 72 + 12 + 96 = 180g/mol

Mass of C6H12O6 = 180g

Number of mole = Mass /Molar Mass

Number of mole of C6H12O6 = 180/180 = 1mole

Volume = 500mL = 500/1000 = 0.5L

Molarity = mole /Volume

Molarity = 1/0.5

Molarity = 2M

So the solution will be best labelled as 2M C6H12O6

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11.19 half lives

Explanation:

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2 years ago
Suppose that a metal oxide of formula m2o3 were soluble in water. what would be the major product or products of dissolving the
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Arrange the following in order of increasing boiling point: RbCl, CH3Cl, CH3OH, CH4. A. CH3OH < CH4 < CH3Cl < RbCl B. R
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Answer:

E. CH₄ < CH₃Cl < CH₃OH < RbCl

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The molecule with the stronger intermolecular forces will have the higher boiling point.

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  • Hydrogen bonding
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If Maria winks exactly 5 times every minute while she is awake and she sleeps exactly 8 hours a day, how many times does Maria w
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5 0
2 years ago
You wish to make a buffer with pH 7.0. You combine 0.060 grams of acetic acid and 14.59 grams of sodium acetate and add water to
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Answer:

The pH of the buffer is 7.0 and this pH is not useful to pH 7.0

Explanation:

The pH of a buffer is obtained by using H-H equation:

pH = pKa + log [A⁻] / [HA]

<em>Where pH is the pH of the buffer</em>

<em>The pKa of acetic acid is 4.74.</em>

<em>[A⁻] could be taken as moles of sodium acetate (14.59g * (1mol / 82g) = 0.1779 moles</em>

<em>[HA] are the moles of acetic acid (0.060g * (1mol / 60g) = 0.001moles</em>

<em />

Replacing:

pH = 4.74 + log [0.1779mol] / [0.001mol]

<em>pH = 6.99 ≈ 7.0</em>

<em />

The pH of the buffer is 7.0

But the buffer is not useful to pH = 7.0 because a buffer works between pKa±1 (For acetic acid: 3.74 - 5.74). As pH 7.0 is out of this interval,

this pH is not useful to pH 7.0

<em />

7 0
2 years ago
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