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horrorfan [7]
3 years ago
6

A bottle contains 3.100 ml of a liquid. the total mass of the bottle and the liquid together is 6.300 g. the mass of the empty b

ottle is 4.240 g. what is the density of the liquid? a 0.665 g/ml b 2.032 g/ml c 1.505 g/ml d 1.368 g/ml
Chemistry
2 answers:
Mariana [72]3 years ago
8 0

Answer : The density of the liquid is (a) 0.665 g/mL

Explanation : Given,

Volume of a liquid = 3.100 mL

Mass of empty bottle = 4.240 g

Total mass of bottle and the liquid = 6.300 g

First we have to calculate the mass of a liquid.

Mass of liquid + Mass of empty bottle = Total mass of bottle and liquid

Mass of liquid + 4.240 g = 6.300 g

Mass of liquid = 6.300 - 4.240 = 2.06 g

Now we have to calculate the density of a liquid.

Density=\frac{Mass}{Volume}

Density=\frac{2.06g}{3.100mL}=0.665g/mL

Therefore, the density of the liquid is 0.665 g/mL

Olenka [21]3 years ago
7 0
The answer is <span>a. 0.665 g/m</span>
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2 years ago
the equilibrium concentration of hydroxide ion in a saturated iron(ii) hydroxide solution is 1.2 x 10^-5 M at a certain temperat
Anit [1.1K]

From the calculation as shpwn in the procedure below, the equilibrium constant of the substance is 6.9 * 10^-15.

<h3>What is equilibrium constant?</h3>

The equilibrium constant for the solubility of aa solid in solution is called the solubility product Ksp. The Ksp shows the extent to which a solid is dissolved in solution.

Given that;

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We have s as 1.2 x 10^-5 M

So

Ksp = 4s^3

Ksp = 4( 1.2 x 10^-5 )^3

Ksp = 6.9 * 10^-15

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2 years ago
In the context of the 4ps of the marketing mix, high-tech media options like cell phones and the internet have had a huge impact
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8 0
1 year ago
Need to complete the chart
GalinKa [24]

Answer:

Row 1

[H^+]=1.8\times 10^{-6}M

pH=-\log[H^+]=-\log[1.8\times 10^{-6}]=5.7

pOh=14-pH=14-5.7=8.3

pOH=-\log[OH^-]

[OH^-]=0.5\times 10^{-8}M

Hence, acidic

Row 2

[OH^-]=3.6\times 10^{-10}M

pOH=-\log[OH^-]=-\log[3.6\times 10^{-10}]=9.4

pH=14-pOH=14 - 9.4 = 4.6

pH=-\log[H^+]

[H^+]=2.6\times 10^{-5}M

Hence, acidic

Row 3

pH = 8.15

[H^+]=0.7\times 10^{-8}M

pOH=14-pH=14 - 8.15 = 5.8

pOH=-\log[OH^-]

[OH^-]=1.5\times 10^{-6}M

Hence, basic

Row 4

pOH = 5.70

[OH^-]=1.8\times 10^{-6}M

pH=14-pOH=14 - 5.70 = 8.3

pH=-\log[H^+]

[H^+]=0.5\times 10^{-8}M

Hence, basic



3 0
3 years ago
6. Give reasons.
MArishka [77]

Answeryou understand but id ont if your know the answer plz help me

Explanation:

3 0
2 years ago
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