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vovangra [49]
3 years ago
6

If a sample of cork has a mass of 2.88 g and a volume of 12.0 mL, what is the density of the cork? Show your work.

Chemistry
1 answer:
PilotLPTM [1.2K]3 years ago
6 0

Answer:

The answer is

<h2>0.24 g/mL</h2>

Explanation:

The density of a substance can be found by using the formula

<h3>density =  \frac{mass}{volume}</h3>

From the question

mass of cork = 2.88 g

volume = 12 mL

The density is

density = \frac{2.88}{12}

We have the final answer as

0.24 g/mL

Hope this helps you

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Hydrogen is a covalent bond. (A bond where one or more pairs of electrons are shared by two atoms)

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Explain why landscapers might sift soil<br> that they use to construct gardens.
Studentka2010 [4]

Answer:

When one desires to remove debris from the garden then a soil sifter can be used as a beneficial tool. Based on the needs, it can be of different kinds. A landscaper may sift soil that they use at the time of constructing gardens due to many reasons:  

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2 years ago
Identify the base-conjugate acid pair in this balanced equation:
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<h3><u>Answer;</u></h3>

NH3/NH4+

<h3><u>Explanation;</u></h3>

From the equation;

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NH3 is the base; while NH4+ is the conjugate acid  

HNO3 is the acid; while NO3- is the conjugate base  

  • The conjugate base of a Brønsted-Lowry acid is species that is formed after an acid donates a proton while the conjugate acid of a Brønsted-Lowry base is the species formed after a base accepts a proton.
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6 0
1 year ago
A 0.15 m solution of chloroacetic acid has a ph of 1.86. What is the value of ka for this acid?
dem82 [27]

Answer: 1.67\times 10^{-3}

Explanation:

ClCH_2COOH\rightarrow ClCH_2COO^-+H^+

   cM              0             0

c-c\alpha        c\alpha          c\alpha  

So dissociation constant will be:

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

Given:  c = 0.15 M

pH = 1.86

K_a = ?

Putting in the values we get:

Also pH=-log[H^+]

1.86=-log[H^+]

[H^+]=0.01

[H^+]=c\times \alpha

0.01=0.15\times \alpha

\alpha=0.06

As [H^+]=[ClCH_2COO^-]=0.01

K_a=\frac{(0.01)^2}{(0.15-0.15\times 0.06)}

K_a=1.67\times 10^{-3]

Thus the vale of K_a for the acid is 1.67\times 10^{-3}

4 0
3 years ago
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