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eimsori [14]
3 years ago
11

Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium hydroxide to react completely with

3.210 g of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?
Chemistry
1 answer:
Butoxors [25]3 years ago
8 0

Answer:

the molar mass of Acetylsalicylic acid is 180.2 g.

Explanation:

Knowing that Acetylsalicylic acid (AA-H) has one acidic proton, we can write the equation for the reaction with NaOH as follows:

AA-<u>H </u>+ NaOH → AA-Na + H₂O (underlined is the acidic proton)

From the equation, we know that 1 mol NaOH reacts with 1 mol AA-H.

The moles of NaOH that react with AA-H can be calculated using the data provided by the problem since we have the volume and the concentration of the NaOH used:

mol NaOH = V * C  where V = volume and C = concentration.

The molar concentration (M) is the number of moles present in 1 liter solution, then, the NaOH solution used has 0.5065 mol NaOH in 1000 ml.

The moles of NaOH used in the reaction can be calculated this way:

mol NaOH = 35.17 ml * (0.5065 mol / 1000 ml) = 0.01781 mol

Then, because 1 mol NaOH reacts with 1 mol AA-H, there must be 0.01781 mol AA-H that react with 0.01781 mol NaOH.

This number of mol of AA-H has a mass of 3.210 g according to the information provided by the problem. Then the mass of a single mol (the molar mass) must be:

molar mass = 1 mol * 3.210 g / 0.01781 mol = <u>180.2 g</u>

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How many liters of space will 7.80 moles of methane gas (CH4) occupy at STP
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Answer:

V CH4(g) = 190.6 L

Explanation:

assuming ideal gas:

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∴ STP: T =298 K and P = 1 atm

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∴ moles (n) = 7.80 mol CH4(g)

∴ Volume CH4(g) = ?

⇒ V = RTn/P

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⇒ V CH4(g) = 190.6 L

4 0
3 years ago
Opal is a hydrated form of silica. If a laboratory analysis of a sample of opal reveals it to contain29.2% Si, 33.3%O, and 37.5%
ZanzabumX [31]
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Si: (29.2 / 28) = 1.04
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8 0
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You can practice converting between the mass of a solution and mass of solute when the mass percent concentration of a solution
LUCKY_DIMON [66]

<u>Answer:</u> The mass of solution having 768 mg of KCN is 426.66 grams.

<u>Explanation:</u>

We are given:

0.180 mass % of KCN solution.

0.180 %(m/m) KCN solution means that 0.180 grams of KCN is present in 100 gram of solution.

To calculate the mass of solution having 768 mg of KCN or 0.786 g of KCN   (Conversion factor:  1 g = 1000 mg)

Using unitary method:

If 0.180 grams of KCN is present in 100 g of solution.

So, 0.768 grams of KCN will be present in = \frac{100g}{0.180g}\times 0.768=426.66g of solution.

Hence, the mass of solution having 768 mg of KCN is 426.66 grams.

8 0
3 years ago
What are precautions to be taken when doing titrations? A-Make sure to always vigorously shake that flask after every drop if th
-BARSIC- [3]

Answer:

E

Explanation:

This is because all steps from A-D are important to obtain an accurate result

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