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schepotkina [342]
3 years ago
14

In an aqueous solution of a certain acid the acid is 0.10% dissociated and the pH is 4.06. Calculate the acid dissociation const

ant Ka of the acid. Round your answer to 2 significant digits
Chemistry
1 answer:
Kruka [31]3 years ago
7 0

Answer : The acid dissociation constant Ka of the acid is, 8.7\times 10^{-5}

Explanation :

First we have to calculate the concentration of hydrogen ion.

pH=-\log [H^+]

Given: pH = 4.06

4.06=-\log [H^+]

[H^+]=8.71\times 10^{-5}M

The dissociation of acid reaction is:

                         HA\rightarrow H^++A^-

Initial conc.      c        0         0

At eqm.           c-cα    cα       cα

Given:

Degree of dissociation = α = 0.10 % = 0.001

[H^+]=c\alpha

8.71\times 10^{-5}=c\times 0.001

c=0.0871M

The expression of dissociation constant of acid is:

K_a=\frac{[H^+][A^-]}{[HA]}

K_a=\frac{(c\times \alpha)\times (c\times \alpha)}{(c-c\alpha)}

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

K_a=\frac{(0.0871\times 0.001)\times (0.0871\times 0.001)}{(0.0871-0.0871\times 0.001)}

K_a=8.7\times 10^{-5}

Thus, the acid dissociation constant Ka of the acid is, 8.7\times 10^{-5}

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Answer:

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Explanation:

6 0
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Answer:

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Explanation:

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The central Xe atom in the XeF₄ molecule has <u>two</u> unbonded electron pairs and <u>four</u> bonded electron pairs in its valence shell.

8 0
3 years ago
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77julia77 [94]

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4 0
3 years ago
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egoroff_w [7]

Answer:

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Explanation:

I belive the pro's                                      and cons are

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4 0
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stiv31 [10]

Answer:

Percent yield: 78.2%

Explanation:

Based on the reaction:

4Al + 3O₂ → 2Al₂O₃

<em>4 moles of Al produce 2 moles of Al₂O₃</em>

<em />

To find percent yield we need to find theoretical yield (Assuming a yield of 100%) and using:

(Actual yield (6.8g) / Theoretical yield) × 100

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4.6g Al × (1mol / 26.98g) = 0.1705 moles of Al.

As 4 moles of Al produce 2 moles of Al₂O₃, theoretical moles of Al₂O₃ obtained from 0.1705 moles of Al are:

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0.0852 moles of Al₂O₃ × (101.96g / mol) =

<h3>8.7g of Al₂O₃ can be produced (Theoretical yield)</h3>

Thus, Percent yield is:

(6.8g / 8.7g) × 100 =

<h3>78.2% </h3>
8 0
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