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AnnyKZ [126]
2 years ago
8

How many moles are in 17.0 grams of H2O2?

Chemistry
2 answers:
Dvinal [7]2 years ago
8 0

Answer:

C) 0.500 mol H2O2 is correct

Explanation:

I just took the test and got it right ;)

vekshin12 years ago
3 0

Answer: Option (c) is the correct answer.

Explanation:

Number of moles is defined as given mass of substance divided by molar mass.

Mathematically,    No. of moles = \frac{mass of given substance}{molar mass}

Molar mass of H_{2}O_{2} is 34.015 g/mol.

Therefore, calculate number of moles of H_{2}O_{2} as follows.

       No. of moles = \frac{mass of given substance}{molar mass}

                             = \frac{17.0 g}{34.015 g/mol}

                             = 0.4997 mol

or,                          = 0.500 mol (approx)

Thus, we can conclude that 0.500 mol is present in 17.0 grams of H_{2}O_{2}.

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A chemistry graduate student is given 500. mL of a 0.20 M chloroacetic acid (HCH2ClCO2) solution. Chloroacetic acid is a weak ac
zhenek [66]

Answer:

12 g of choloracetic acid

Explanation:

The buffer equilibrium is:

HCH₂ClCO₂ ⇄ CH₂ClCO₂⁻ + H⁺

pka= -log ka =

Ka: 1,3x10⁻³ = [CH₂ClCO₂⁻] [H⁺] / [HCH₂ClCO₂]

By Henderson-Hasselbalch equation:

pH = pka + log₁₀ [A⁻] / [HA]

3,01 = 2,89 + log₁₀ [A⁻] / [HA]

1,318 = [A⁻] / [HA]

As molar concentration of chloroacetic acid (HA) is 0,20M

[A⁻] = 0,26 mol/L

The volume is 500 mL ≡ 0,5 L

0,26mol/L × 0,5 L = 0,13 moles of chloroacetic acid. In grams:

0,13 mol × (94,5g / 1mol) = <em>12 g of choloracetic acid</em>

<em></em>

I hope it helps!

3 0
3 years ago
A 1.00 liter solution contains 0.43 M hydrofluoric acid and 0.56 M potassium fluoride. If 0.280 moles of potassium hydroxide are
kolbaska11 [484]

Answer:

Answers are in the explanation

Explanation:

Equlibrium of HF in H₂O is:

HF + H₂O ⇄ F⁻ + H₃O⁺

Now, the KOH reacts with HF, thus:

KOH + HF →  F⁻ + H₂O

<em>That means after reaction, concentration of HF decrease increasing F⁻ concentration.</em>

Now, seeing the equilibrium, as moles of HF decrease and F⁻ moles increase, the equilibrium will shift to the left decreasing H₃O⁺ concentration.

For the statements:

A. The number of moles of HF will increase. <em>FALSE</em>. HF react with KOH, thus, moles of HF decrease

B. The number of moles of F- will decrease. <em>FALSE</em>. The reaction produce  F⁻ increasing its moles.

C. The equilibrium concentration of H₃O⁺ will increase. <em>FALSE. </em>The equilibrium shift to the left decreasing concentration of H₃O⁺

D. The pH will decrease. <em>FALSE</em>. As the H₃O⁺ concentration decrease, pH will increase

E. The ratio of [HF] / [F-] will remain the same. <em>FALSE</em>. Because moles of HF are decreasing whereas F- moles are increasing changing, thus, ratio.

6 0
3 years ago
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