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Mekhanik [1.2K]
2 years ago
11

Determine the acid dissociation constant for a 0.0250 M weak acid solution that has a pH of 2.37 . The equilibrium equation of i

nterest is​
Chemistry
1 answer:
Oksanka [162]2 years ago
3 0

Answer:

For part (a): pHsol=2.22

Explanation:

I will show you how to solve part (a), so that you can use this example to solve part (b) on your own.

So, you're dealing with formic acid, HCOOH, a weak acid that does not dissociate completely in aqueous solution. This means that an equilibrium will be established between the unionized and ionized forms of the acid.

You can use an ICE table and the initial concentration ofthe acid to determine the concentrations of the conjugate base and of the hydronium ions tha are produced when the acid ionizes

HCOOH(aq]+H2O(l]⇌ HCOO−(aq] + H3O+(aq]

I 0.20 0 0

C (−x) (+x) (+x)

E (0.20−x) x x

You need to use the acid's pKa to determine its acid dissociation constant, Ka, which is equal to

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<u>Answer:</u> The molarity of Cr^{3+} ions in the solution is 0.299 M

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To calculate the number of moles for given molarity, we use the equation:

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Moles of Cr^{3+}\text{ ions}=(1\times 0.00493)=0.00493moles

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Total moles of chromium cations = [0.00613 + 0.00493] = 0.01106 moles

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\text{Molarity of }Cr^{3+}\text{ cations}=\frac{0.01106\times 1000}{36.9}\\\\\text{Molarity of }Cr^{3+}\text{ cations}=0.299M/tex]Hence, the molarity of [tex]Cr^{3+} ions in the solution is 0.299 M

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