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stepladder [879]
3 years ago
12

Find the [H+] in an acetic acid solution that has a pH of 5.12

Chemistry
1 answer:
Eva8 [605]3 years ago
3 0
<span>Data:
pH = 5.2
[H+] = ?

Knowing that: (</span><span>Equation to find the pH of a solution)</span>
pH = -log[H+]
<span>
Solving:
</span>pH = -log[H+]
5.2 = - log [H+]
Knowing that the exponential is the opposite operation of the logarithm, then we have:
[H+] = 10^{-5.2}
\boxed{\boxed{[H+] = 6.30*10^{-6}}}\end{array}}\qquad\quad\checkmark
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How many grams of dry nh4cl need to be added to 2.50 l of a 0.800 m solution of ammonia, nh3, to prepare a buffer solution that
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Explanation:

Based on the given information, the number of moles of NH₃ will be,  

= 2.50 L × 0.800 mol/L

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pH + pOH = 14.00

pOH = 14.00 - pH

pOH = 14.00 - 8.53

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= -log (1.8 ×10⁻⁵)

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Based on Henderson equation:  

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5.47 = 4.74 + log ([NH₄⁺]/[NH₃])

log([NH₄⁺]/[NH₃]) = 5.47-4.74 = 0.73

[NH₄⁺]/[NH₃] = 10^0.73= 5.37

[NH₄⁺ = 5.37 × 2 mol = 10.74 mol

Now the mass of dry ammonium chloride required is,  

mass of NH₄Cl = 10.74 mol × 53.5 g/mol

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Answer:

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