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3 years ago

Is waterproof sunscreen polar or non-polar

Chemistry

2 answers:

Tatiana [17]3 years ago

8 0

Answer:

Explanation:

Water proof sunscreen have non - polar molecules.

As water is a polar molecule, the sunscreen is water proof so it is non polar and lack charges.

Due to this property, they do not interact with charged particles hence it do not mix with water.

Waterproof sunscreen do not mix with sweat thus maintaining the color and protective layer on skin.

Stolb23 [73]3 years ago

6 0

Non-polar because hydrophilic means something can be wetted by water

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A solution is created by dissolving 13.0 grams of ammonium chloride in enough water to make 295 mL of solution. How many moles o

Masja [62]

Answer:

(a) Moles of ammonium chloride = 0.243 moles

(b) $Molarity_{ammonium\ chloride}=0.824\ M$

Explanation:

(a) Mass of ammonium chloride = 13.0 g

Molar mass of ammonium chloride = 53.491 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{13.0\ g}{53.491\ g/mol}$

Moles of ammonium chloride = 0.243 moles

(b) Moles of ammonium chloride = 0.243 moles

Volume = 295 mL = 0.295 L ( 1 mL = 0.001 L)

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$Molarity_{ammonium\ chloride}=\frac{0.243}{0.295}$

$Molarity_{ammonium\ chloride}=0.824\ M$

Volume = ?

Molarity = 0.824 M

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

$0.824\ M=\frac{0.0500}{Volume}$

Volume = 0.05 / 0.824 L = 0.06068 L = 60.68 mL

6 0

3 years ago

Help with this question pleasee

kvv77 [185]

Solids. Example: when you hit a drum, it vibrates, then the sound travels through the air, to your ears.

8 0

3 years ago

Read 2 more answers

How much concentrated solution would it take to prepare 2.90 L of 0.420 M HCl upon dilution with water

Zanzabum

Answer:

the quantity required can go from 117 ml (for maximum concentration) up to 2900 ml ( if the concentrated solution has molarity =0.420 M)

Explanation:

the amount of water required to dilute a solution V₁ liters of Molarity M₁ to V₂ liters of M₂

moles of hydrochloric acid = M₁ * V₁= M₂ * V₂

V₁ = V₂ * M₂/M₁

where

M₂ = 0.420 M

V₂ =2.90 L

Since the hydrochloric acid can be concentrated up to 38% p/V ( higher concentrations are possible but the evaporation rate is so high that handling and storage require extra precautions, like cooling and pressurisation)

maximum M₁ =38% p/V = 38 gr/ 0.1 L / 36.5 gr/mol = 10.41 M

then

min V₁ = V₂ * M₂/ max M₁ = 2.90 L* 0.420 M/ 10.41 M= 0.117 L = 117 ml

then the quantity required can go from 117 ml up to 2900 ml ( if M₁ = M₂)

5 0

3 years ago

How many milliliters of this solution are required to prepare 1.00 L of 0.130 M K2Cr2O7 ?

ra1l [238]

Answer:

First you'll need to divide the mass of K2Cr2O7 by its molar mass and volume which should be easy but I'll do some of it to help you out

Explanation:

$K_{2}Cr_{2}O_{7}$

$2K = 39.098 = 2(39.098) = 78.196$

$2Cr = 51.996 = 2(51.996) = 103.992$

and

$7O = 15.999 = 7(15.999) = 111.993$

$78.196 + 103.992 + 111.993 = 294.181$

so that's the mass of K2Cr2O7 and then you divide it by the molar mass and volume.

Hopefully you can do that on your own! Hope I helped a bit atleast and I have a good feeling about 0.438 but I don't want you to just guess

7 0

2 years ago

A cubic meter of air near saturation may contain 28 grams, or about 1.6 moles of water molecules at 30 °C, but

lesantik [10]

For the cubic meter of air near saturation that contains 28 grams (1.6 moles) of water molecules when T = 30°C and 8 grams (0.44 moles) of it when T = 8°C, we have:

1. The pressure of air due to water vapor when the temperature is 30°C and 8°C, is 0.040 atm and 0.010 atm, respectively.

2. Since the water vapor depends on the temperature, it is important to know the temperature of air so we can know how much air pressure is due to water vapor.

1. The pressure of air near saturation can be calculated with the Ideal gas law equation:

$PV = nRT$

Where:

P: is the pressure =?

V: is the volume = 1 m³ = 1000 L

n: is the number of moles

T: is the temperature

R: is the gas constant = 0.082 L*atm/(K*mol)

Pressure when the temperature is 30°C

We have:

T = 30 ° = 303 K

n: number of moles of water = 1.6 moles

Then the pressure is:

$P_{30} = \frac{nRT}{V} = \frac{1.6 \:moles*0.082 L*atm/(K*mol)*303 K}{1000 L} = 0.040 atm$

Hence, the pressure when the temperature is 30°C is 0.040 atm.

Pressure when the temperature is 8°C

T = 8 °C = 281 K

n = 0.44 moles of water

The pressure is:

$P_{8} = \frac{nRT}{V} = \frac{0.44 \:moles*0.082 L*atm/(K*mol)*281 K}{1000 L} = 0.010 atm$

Therefore, the pressure when the temperature is 8°C is 0.010 atm.

2. Since the amount of mass or moles of water in the atmosphere depends on the temperature, having that the higher the temperature, the higher the number of water molecules present in the air, it is important to know the temperature so we can know how much of the air pressure is due to the water vapor and thus the value of humidity in the air.

Find more here:

brainly.com/question/1190311?referrer=searchResults

I hope it helps you!

3 0

3 years ago