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Art [367]
3 years ago
11

I need help filling out this table, please help ASAP

Chemistry
2 answers:
aleksandr82 [10.1K]3 years ago
6 0

Answer:

A-20 B-40 C-Ca D-10 E-9 F-F

Dovator [93]3 years ago
3 0

Explanation:

<h2>----------------------------------------------</h2><h2>atomic number= no.of protons</h2><h2>and </h2>

<h2>mass no.= no. of protons+no. of neutrons</h2><h2>__________________________</h2><h2><em>A</em><em>=</em><em> </em><em>2</em><em>0</em></h2><h2><em>B</em><em>=</em><em> </em><em>4</em><em>0</em></h2><h2><em>C=</em><em> </em><em>ca</em></h2><h2><em>D</em><em>=</em><em> </em><em>1</em><em>0</em></h2><h2><em>E</em><em>=</em><em> </em><em>9</em></h2><h2><em>F</em><em>=</em><em>F</em></h2>

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An analytical chemist is titrating of a solution of nitrous acid with a solution of . The of nitrous acid is . Calculate the pH
Burka [1]

Answer:

pH = 2.69

Explanation:

The complete question is:<em> An analytical chemist is titrating 182.2 mL of a 1.200 M solution of nitrous acid (HNO2) with a solution of 0.8400 M KOH. The pKa of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 46.44 mL of the KOH solution to it.</em>

<em />

The reaction of HNO₂ with KOH is:

HNO₂ + KOH → NO₂⁻ + H₂O + K⁺

Moles of HNO₂ and KOH that react are:

HNO₂ = 0.1822L × (1.200mol / L) = <em>0.21864 moles HNO₂</em>

KOH = 0.04644L × (0.8400mol / L) = <em>0.0390 moles KOH</em>

That means after the reaction, moles of HNO₂ and NO₂⁻ after the reaction are:

NO₂⁻ = 0.03900 moles KOH = moles NO₂⁻

HNO₂ = 0.21864 moles HNO₂ - 0.03900 moles = 0.17964 moles HNO₂

It is possible to find the pH of this buffer (<em>Mixture of a weak acid, HNO₂ with the conjugate base, NO₂⁻), </em>using H-H equation for this system:

pH = pKa + log₁₀ [NO₂⁻] / [HNO₂]

pH = 3.35 + log₁₀ [0.03900mol] / [0.17964mol]

<h3>pH = 2.69</h3>
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