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andreev551 [17]
1 year ago
8

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

<u>brainly.com/question/8676275</u>

#SPJ4

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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,

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