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jeka94
2 years ago
5

What is the concentration of a solution made by dissolving 0.99mol of acetic acid in enough water to make 0.58L of solution?

Chemistry
1 answer:
marissa [1.9K]2 years ago
4 0

Answer:

[CH₃COOH] = 1.70 M

Explanation:

When we talk about concentration we can determine Molarity

Molarity determines the moles of solute that are contained in 1L of solution.

In this case our solute is the acetic acid.

M = mol/L

M = 0.99 mol /0.58L → 1.70 M

We can also make a rule of three

In 0.58 L of solution we have 0.99 moles of solute

In 1 L of solution we may have (1 . 0.99) / 0.58 = 1.70 moles

Acetic acid is a weak acid, partially dissociated in water.

CH₃COOH  +  H₂O  ⇄  CH₃COO⁻  +  H₃O⁺     Ka

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A household cleaner has a pH around 10. It would be considered
anyanavicka [17]

Answer:

an acid

Explanation:

A household cleaner has a pH around 10. It would be considered. a base. an acid. neutral. a liquid.

4 0
3 years ago
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How many grams of sulfuric acid is needed to neutralize 380 ml of solution with pH = 8.94
erma4kov [3.2K]

Answer : The mass of sulfuric acid needed is 16.23\times 10^{-5}g.

Solution : Given,

pH = 8.94

Volume of solution = 380 ml = 380\times 10^{-3}      (1ml=10^{-3}L)

Molar mass of sulfuric acid = 98.079 g/mole

As we know,

pH+pOH=14\\pOH=14-8.94=5.06

pOH=-log[OH^-]

5.06=-log[OH^-]

[OH^-]=0.00000871=8.71\times 10^{-6}mole/L

Now we have to calculate the moles of OH^-.

Formula used : Moles=Concentration\times Volume

\text{ Moles of }[OH^-]=\text{ Concentration of }[OH^-]\times Volume\\\text{ Moles of }[OH^-]=(8.71\times 10^{-6}mole/L)\times (380\times 10^{-3}L)=3309.8\times 10^{-9}moles

For neutralization, equal number of moles of H^+ ions will neutralize same number of OH^- ions.

\text{ Moles of }[OH^-]=\text{ Moles of }[H^+]=3309.8\times 10^{-9}moles

As, H_2SO_4\rightarrow 2H^++SO^{2-}_4

From this reaction, we conclude that

2 moles of H^+ ion is given by the 1 mole of H_2SO_4

3309.8\times 10^{-9} moles of H^+ ion is given by \frac{3309.8\times 10^{-9}}{2}=1654.9\times 10^{-9} moles of H_2SO_4

Now we have to calculate the mass of sulfuric acid.

Mass of sulfuric acid = Moles of H_2SO_4 × Molar mass of sulfuric acid

Mass of sulfuric acid = (1654.9\times 10^{-9}moles)\times (98.079g/mole)=162310.94\times 10^{-9}=16.23\times 10^{-5}g

Therefore, the mass of sulfuric acid needed is 16.23\times 10^{-5}g.

3 0
3 years ago
Elements in the same group have _____.
Xelga [282]

Similar chemical properties

(OPTION C)

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3 years ago
Elements in a given period of the periodic table contain the same number of
leva [86]
Its C, Outermost Electrons.
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3 years ago
Explain the energy transformation that occurs when food is digested.
Lunna [17]

<em>Answer:</em>

<em>C. Mechanical energy transforms into chemical energy.</em>

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<em>Hope this helped. Have a nice day.</em>

4 0
2 years ago
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