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zaharov [31]
3 years ago
6

What volume of a 0.155 M potassium hydroxide solution is required to neutralize 25.7 mL of a 0.388 M hydrobromic acid solution

Chemistry
1 answer:
vekshin13 years ago
8 0

Answer: Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

According to the neutralization law,

n_1M_1V_1=n_2M_2V_2

where,

M_1 = molarity of HBr solution = 0.338 M

V_1 = volume of HBr solution = 25.7 ml

M_2 = molarity of KOH solution = 0.155 M

V_2 = volume of KOH solution = ?

n_1 = valency of HBr = 1

n_2 = valency of KOH = 1

1\times 0.338\times 25.7=1\times 0.155\times V_2

V_2=56.0ml

Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml

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What is the pH of a 0.1 M phosphate buffer (pKa = 6.86) that contains equal amounts of acid and conjugate base?
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Answer : The pH of a 0.1 M phosphate buffer is, 6.86

Explanation : Given,

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Using Henderson Hesselbach equation :

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pH=6.86+\log (\frac{0.1}{0.1})

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Answer:

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2C2H2(g)+5O2(g)=4CO2(g)+2H2O(g)
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The volume of ethyne, C₂H₂ required to produce 12 moles of CO₂ assuming the reaction is at STP is 134.4 L

<h3>Balanced equation</h3>

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From the balanced equation above,

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<h3>How to determine the mole of C₂H₂ needed to produce 12 moles of CO₂</h3>

From the balanced equation above,

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Therefore,

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<h3>How to determine the volume (in L) of C₂H₂ needed at STP</h3>

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