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sveticcg [70]
3 years ago
9

Calculate the ph of a solution that is 0.26 m in hf and 0.12 m in naf.

Chemistry
1 answer:
DochEvi [55]3 years ago
5 0
When a mixture consists of a weak acid, such as HF, and its corresponding salt, NaF, this is an acid buffer. So, we can use the equation as written below:

pH = pKa + log(salt/acid)

For HF, the pKa = 3.17

Thus,
pH = 3.17 + log(0.12/0.26)
<em>pH = 2.83</em>
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Answer : The volume of solution will be 2.96 liters.

Explanation :

Molarity : It is defined as the number of moles of solute present in one liter of volume of solution.

Formula used :

\text{Molarity}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}

In this question, the solute is NaF.

Now put all the given values in this formula, we get:

0.0550M=\frac{0.163mole}{\text{Volume of solution (in L)}}

\text{Volume of solution (in L)}=\frac{0.163mole}{0.0550M}

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Considering the law of conservation of mass, if 56 g samples of solid iron (Fe) reacts with 24 g of oxygen (O2), how many grams
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