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3 years ago

11

Balance the following redox equation, identifying the element oxidized and the element reduced. Show all of the work used to sol

ve the problem.
Ag + CN- + O2 yields Ag(CN)2- + H2O

1 answer:

hodyreva [135]3 years ago

3 0

The given equation is,

$Ag(s) + CN^{-}(aq) + O_{2}(aq) --> [Ag(CN)_{2}]^{-} (aq) + H_{2}O(l)$

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In a titration, 4.7 g of an acid (HX) requires 32.6 mL of 0.54 M NaOH(aq) for complete reaction. What is the molar mass of the a

katrin2010 [14]

Answer : The molar mass of an acid is 266.985 g/mole

Explanation : Given,

Mass of an acid (HX) = 4.7 g

Volume of NaOH = 32.6 ml = 0.0326 L

Molarity of NaOH = 0.54 M = 0.54 mole/L

First we have to calculate the moles of NaOH.

$\text{Moles of }NaOH=\text{Molarity of }NaOH\times \text{Volume of solution}=0.54mole/L\times 0.0326L=0.017604mole$

Now we have to calculate the moles of an acid.

In the titration, the moles of an acid will be equal to the moles of NaOH.

Moles of an acid = Moles of NaOH = 0.017604 mole

Now we have to calculate the molar mass of and acid.

$\text{Moles of an acid}=\frac{\text{Mass of an acid}}{\text{Molar mass of an acid}}$

Now put all the given values in this formula, we get:

$0.017604mole=\frac{4.7g}{\text{Molar mass of an acid}}$

$\text{Molar mass of an acid}=266.985g/mole$

Therefore, the molar mass of an acid is 266.985 g/mole

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3 years ago

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Hi there!

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<h3>Further explanation </h3>

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$\tt \sum=1\times 19=19~N$

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3 years ago