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3 years ago

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The end point of a titration was reached after 22 ml of 0.050 m disodium edta titrant was dispensed into a solution containing t

he zinc ion. calculate the moles of disodium edta used

2 answers:

ale4655 [162]3 years ago

4 0

The moles of disodium edta used is calculated using the below formula

moles =molarity x volume in liters

molarity=0.050m
volume in liters = 22/1000=0.022 L

moles is therefore= 0.022 x0.050 =1.1 x10^-3 moles of disodium edta

Dimas [21]3 years ago

3 0

Answer:

moles =molarity x volume in liters

molarity=0.050m

volume in liters = 22/1000=0.022 L

moles is therefore= 0.022 x0.050 =1.1 x10^-3 moles of disodium edta

Explanation:

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Answer:

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We have to consider the valencies of the polyatomic ions involved. Recall that it is only a polyatomic ion with a valency of -2 that can form a compound which requires two sodium ions.

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2 years ago

Aclosed system contains an equimolar mixture of n-pentane and isopentane. Suppose the system is initially all liquid at 120°C an

garri49 [273]

Explanation:

The given data is as follows.

T = $120^{o}C$ = (120 + 273.15)K = 393.15 K,

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So, $x_{1}$ = 0.5 and $x_{2}$ = 0.5

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$p^{sat}_{1}$ (393.15 K) = 9.2 bar

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Hence, we will calculate the partial pressure of each component as follows.

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Therefore, the bubble pressure will be as follows.

P = $p_{1} + p_{2}$

= 4.6 bar + 5.25 bar

= 9.85 bar

Now, we will calculate the vapor composition as follows.

$y_{1} = \frac{p_{1}}{p}$

= $\frac{4.6}{9.85}$

= 0.467

and, $y_{2} = \frac{p_{2}}{p}$

= $\frac{5.25}{9.85}$

= 0.527

Calculate the dew point as follows.

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$\frac{1}{P} = \frac{0.5}{9.2} + \frac{0.5}{10.2}$

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P = 9.807

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$x_{i} = \frac{y_{i} \times P}{p^{sat}_{1}}$

= $\frac{0.5 \times 9.807}{9.2}$

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$x_{z} = \frac{y_{i} \times P}{p^{sat}_{1}}$

= $\frac{0.5 \times 9.807}{10.5}$

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Hope this answers the question. Have a nice day.

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3 years ago