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pantera1 [17]
3 years ago
14

Approximately how many moles of chlorine make up 1.79 x 10^23 atoms of chlorine?

Chemistry
1 answer:
laila [671]3 years ago
6 0
<h2>Answer</h2>

The answer of given question is 0.13 mol

<h2>Explanation</h2>

1 mol of chlorine (Cl) contain =6.022^{23} N_{A} atoms atoms (Avogadro Number)

So, we have to determine how many moles of Cl will be contain for 0.79 * 10^{23} N_{A}atoms.

As we know unit method

6.022^{23} N_{A} = 1 mol of chlorine (Cl)

1 N_{A} atom = 1/6.022^{23} N_{A}}

0.79 * 10 ^{23} N_{A} = 1 mol * 0.79^{23} N_{A}/6.022^{23} N_{A}

0.79* 10 ^{23} N_{A} = 0.13 mol

So, the answer is 0.13 mol



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Answer:

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Explanation:

<u>Step 1:</u> The balanced equation

HA(aq) + NaOH(aq) → NaA(aq) + H2O(l)

It takes 1 mole of NaOH to neutralize 1 mole of the triprotic acid. This is called the reaction stoichiometry.

<u>Step 2:</u> Data given

Mass of the acid = 0.093 grams

volume = 250 mL

titrates with 0.16 M NaOH

adds 6.5 mL NaOH

<u>Step 3: </u>Calculate moles of NaOH

We know the concentration and volume of NaOH needed to neutralize the acid.

By determining the moles of NaOH in that volume in liters (95.9mL=0.0959L), the moles of acid in the original sample can be determined from the reaction stoichiometry.

Moles = Molarity * Volume

Moles = 0.16 M * 0.0065 L

Moles = 0.00104 moles NaOH

<u>Step 4: </u>Calculate moles of the unknown acid:

It takes 1 mole of NaOH to neutralize 1 mole of the triprotic acid. This is called the reaction stoichiometry.

For 0.00104 moles NaOH we have 0.00104 moles of HA

<u>Step 5: </u>Calculate the molar mass of the acid

Molar mass Ha = Mass Ha / moles Ha

Molar mass Ha = 0.093 grams / 0.00104 moles

Molar mass Ha = 89.42 g/mol ≈89 g/mol

The molar mass of the unknown acid is 89 g/mol

3 0
3 years ago
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