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otez555 [7]
3 years ago
6

The exact value for the density of aluminum is 2.699 g.cm^3. Working in the science lab at school, Joseph finds the density of a

piece of aluminum to be 2.75 g/cm^3. What is Joseph's percent error? (Round to the nearest hundredth.)
Chemistry
1 answer:
Alex787 [66]3 years ago
4 0

Joseph's percentage error would be 1.89%

<u>Explanation:</u>

Exact value of the density of aluminium = 2.699 g/cm³

Calculated value of the density of aluminium = 2.75 g/cm³

Percentage error = ?

We know:

Percentage error = \frac{experimental - exact}{exact} X 100\\\\

= \frac{2.75 - 2.699}{2.699} X 100\\\\= \frac{0.051}{2.699} X 100\\\\= 1.89\\

Therefore, Joseph's percentage error would be 1.89%

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Answer:

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Explanation:

We'll begin by writing the balanced

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HClO4 —> H+ + ClO4-

A. Determination of the concentration of H+ in 0.0025 M HClO4. This is illustrated below:

From the balanced equation above,

1 mole of HClO4 produced 1 mole of H+.

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The concentration of H+ is 0.0025 M

B. Determination of the pH.

The pH of the solution can be obtained as follow:

The concentration of H+, [H+]

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pH = - log [H+]

pH = - log 0.0025

pH = 2.6

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To obtain the concentration of OH-, we must first calculate the pOH of the solution. This is illustrated below:

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2.6 + pOH = 14

Collect like terms

pOH = 14 - 2.6

pOH = 11.4

Now, we can calculate the concentration of the OH- as follow:

pOH = - Log [OH-]

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8 0
3 years ago
How many liters of nitrogen gas are needed to make 25 mol of nitrogen trifluoride
ikadub [295]
The reaction between N₂ and F₂ gives Nitrogen trifluoride as the product. The balanced equation is;

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