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1 year ago

Which pair of aqueous solutions can create a buffer solution if present in the appropriate concentrations?.

Chemistry

1 answer:

Julli [10]1 year ago

8 0

HF and NaF - If the right concentrations of aqueous solutions are present, they can produce a buffer solution.

<h3>What are buffer solutions and how do they differ?</h3>

The two main categories of buffers are acidic buffer solutions and alkaline buffer solutions.
Acidic buffers are solutions that contain a weak acid and one of its salts and have a pH below 7.
For instance, a buffer solution with a pH of roughly 4.75 is made of acetic acid and sodium acetate.

<h3>Describe buffer solution via an example.</h3>

When a weak acid or a weak base is applied in modest amounts, buffer solutions withstand the pH shift.
A buffer made of a weak acid and its salt is an example.
It is a solution of acetic acid and sodium acetate CH3COOH + CH3COONa.

learn more about buffer solutions here

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Pentaborane-9,

frozen [14]

Given question is incomplete. The complete question is as follows.

Pentaborane ( $B_{5}H_{9}$ ) is a colorless highly reactive liquid that will burst into flames when exposed to oxygen.the reaction is:

$2B_{5}H_{9}(l) + 12O_{2} \rightarrow 5B_{2}O_{2}(s) + 9H_{2}O(l)$

Calculate the kilojoules of heat released per gram of the compound reacted with oxygen.the standard enthalpy of formation $B_{5}H_{9}(l)$ , $B_{2}O_{3}(s)$ , and $H_{2}O(l)$ are 73.2, -1271.94, and -285.83 kJ/mol, respectively.

Explanation:

As the given reaction is as follows.

$2B_{5}H_{9}(l) + 12O_{2} \rightarrow 5B_{2}O_{2}(s) + 9H_{2}O(l)$

Therefore, formula to calculate the heat energy released is as follows.

$\Delta H = \sum H_{products} - \Delta H_{reactants}$

Hence, putting the given values into the above formula is as follows.

$\Delta H = \sum H_{products} - \Delta H_{reactants}$

= $5 \times (-1271.94 kJ/mol) + 9 \times (-285.83 kJ/mol) - 2 \times (73.2 kJ/mol) - 12(0)$

= -9078.59 kJ/mol

Since, 2 moles of Pentaborane reacts with oxygen. Therefore, heat of reaction for 2 moles of Pentaborane is calculated as follows.

$\frac{\Delta H}{2 \times \text{molar mass of pentaborane}}$

$\frac{-9078.59 kJ/mol}{2 \times 63.12 g/mol}$

= -71.915 kJ/g

Thus, we can conclude that heat released per gram of the compound reacted with oxygen is 71.915 kJ/g.

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Answer:

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Explanation:

From the question,

Mass of Al used = 0.660g

The percentage yield = 63.5%

Mass of Alum used = y

To find the mass of Alum used, do the following:

%yield = Mass of Al /Mass and Alum

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65/100 = 0.660/y

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65 x y = 0.660x100

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