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ioda
2 years ago
7

Calculate the percent ionization of benzoic acid at the following concentrations. (a) 0.32 M WebAssign will check your answer fo

r the correct number of significant figures. 1.4 Correct: Your answer is correct. (b) 0.00014 M WebAssign will check your answer for the correct number of significant figures. 48 Correct: Your answer is correct.
Chemistry
1 answer:
seraphim [82]2 years ago
8 0

Answer: a) 1.4 %

b) 48%

Explanation:

C_7H_6O_2\rightarrow H^+C_7H_5O_2^-

 cM                0             0

c-c\alpha    c\alpha      c\alpha  

So dissociation constant will be:

K_a=\frac{(c\alpha)^{2}}{c-c\alpha}

a) Given c= 0.32M and K_a=6.3\times 10^{-5}

\alpha = ?

Putting in the values we get:

6.3\times 10^{-5}=\frac{(0.32\times \alpha)^2}{(0.32-0.32\times \alpha)}

(\alpha)=0.014

\%(\alpha)=0.014\times 100=1.4\%

b) Given c= 0.00014 M and K_a=6.3\times 10^{-5}

\alpha = ?

Putting in the values we get:

6.3\times 10^{-5}=\frac{(0.00014\times \alpha)^2}{(0.00014-0.00014\times \alpha)}

(\alpha)=0.48

\%(\alpha)=0.48\times 100=48\%

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How would I do this? A beaker contains 50.0 mL of 0.25 M aluminum nitrate solution. What is the minimum volume of 0.2 M sodium s
Serhud [2]

The minimum volume of 0.2M sodium sulfide that will precipitate out aluminum from 50.0 mL, 0.25 M aluminum nitrate would be 0.094 L or 94 mL

<h3>Stoichiometric calculation</h3>

From the equation of the reaction:

2Al(NO_3)_3 + 3Na_2S ---> Al_2S_3 + 6NaNO_3

Mole ratio of Na2S and Al(NO3)3 = 3:2

Mole of 50.0 mL, 0.25 M Al(NO3)3 = 50/1000 x 0.25

                                                         = 0.0125 mole

Equivalent mole of Na2S = 3/2 x 0.0125

                                         = 0.0188 mole

Volume of 0.2M, 0.0188 mole Na2S = 0.0188/0.2

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More on stoichiometric calculations can be found here: brainly.com/question/8062886

6 0
2 years ago
How many grams of antifreeze C2H4(OH)2 would be required per 500 g of water to prevent the water from freezing at a temperature
Wewaii [24]

Answer:

333.7 g.

Explanation:

  • The depression in freezing point of water (ΔTf) due to adding a solute to it is given by: <em>ΔTf = Kf.m.</em>

Where, ΔTf is the depression in water freezing point (ΔTf = 20.0°C).

Kf is the molal freezing point depression constant of the solvent (Kf = 1.86 °C/m).

m is the molality of the solution.

<em>∴ m = ΔTf/Kf</em> = (20.0°C)/(1.86 °C/m) = <em>10.75 m.</em>

molaity (m) is the no. of moles of solute per kg of the solvent.

∵ m = (no. of moles of antifreeze C₂H₄(OH)₂)/(mass of water (kg))

∴ no. of moles of antifreeze C₂H₄(OH)₂ = (m)(mass of water (kg)) = (10.75 m)(0.5 kg) = 5.376 mol.

∵ no. of moles = mass/molar mass.

<em>∴ mass of antifreeze C₂H₄(OH)₂ = no. of moles x molar mass </em>= (5.376 mol)(62.07 g/mol) =<em> 333.7 g.</em>

5 0
3 years ago
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