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2 years ago

what ppe and engineering controls should be used when working with any dilution of acetic acid? uta lab

Chemistry

1 answer:

Setler79 [48]2 years ago

5 0

Following measures should be taken while working with any dilution of acetic ( $CH_3COOH$ ) acid :

One should wear chemical resistant gloves to protect hand from splash during dilution.

Chemical resistant apron and chemical splash goggles is mandatory to wear to protect one from effects of acetic acid on body.

Go through Safety Guidelines manual whenever diluting concentrated acid.

PPE is mandatory to wear when acetic acid is handled in concentrated state before dilution.

If the area where experiment is performed is not ventilated the wear respiratory equipment.

To know more about Acetic Acid dilution

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3 years ago

Determine whether or not each ion contributes to water hardness.

Virty [35]

Answer: The ion that contribute to water hardness are:

--> a. Ca2+

--> b. (HCO)3^- and

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While K+ DOES NOT contribute to water hardness.

Explanation:

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3 years ago

At 63.5 C the vapor pressure of H2O is 175 torr and that of ethanol is 400 torr. A solution is made by adding equal masses of H2

xxTIMURxx [149]

Answer:

Moel fraction of ethanol in the solution = 0.28

Vapor pressure of the solution = 238 torr

Mole fraction of ethanol in the vapor = 0.47

Explanation:

Let's use 100 g of each substance as a calculus basis. Knowing that the molar mass of water is 18 g/mol and the molar mass of ethanol is 46 g/mol, the number of moles (n = mass/molar mass) of each one is:

nw = 100/18 = 5.56 mol

ne= 100/46 = 2.17 mol

The total number of moles is 7.73 mol, so the mole fraction of ethanol is

2.17/7.73 = 0.28

The mole fraction of water must be 0.72, so if we assume that the solution is ideal, by the Raoult's law, the solution vapor pressure is the sum of the multiplication of the mole fraction by the vapor pressure of each substance, thus:

P = 0.28*400 + 0.72*175

P = 238 torr

The partial pressure of each substance can be found by the multiplication of the molar fraction by the vapor pressure, thus:

Pw = 0.72*175 = 126 torr

Pe = 0.28*400 = 112 torr

To know the number of moles that is vaporized above the solution, we may use the ideal gas law:

PV = nRT

P/n = RT/V

R is the gas constant, T is the temperature and V is the volume, so they are the same for both water and ethanol, thus

Pw/nw = Pe/ne

126/nw = 112/ne

ne = (112/126)*nw

ne = 0.89nw

So, the mole fraction of ethanol is:

ne/(ne + nw) = 0.89nw/(0.89nw + nw) = 0.89/1.89 = 0.47

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3 years ago