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marta [7]
3 years ago
15

825 mL sample of an unknown HClO4 Solution requires titration with 22.62 mL of 0.2000 M NaOH to reach the equivalence point. Wha

t is the concentration of the unknown HClO4 solution? The neutralization reaction is HClO4 (Aq) + NaOH (aq) -> H2O (l) + NaClO4 (aq)
Chemistry
1 answer:
vichka [17]3 years ago
5 0

Answer:

M_{acid}=5.484x10^{-3}M

Explanation:

Hello,

By using the following formula, which comes from the assurance of the equivalence point:

M_{acid}*V_{acid}=M_{base}*V_{base}\\M_{acid}=\frac{M_{base}*V_{base}}{V_{acid}}

We just simply compute the acid's concentration (molarity), turning out into:

M_{acid}=\frac{0.2000M*22.62mL}{825mL} \\\\M_{acid}=5.484x10^{-3}M

Best regards.

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Explanation:

First, let's review the ideal gas law, PV = nRT. In this equation, 'P' is the pressure in atmospheres, 'V' is the volume in liters, 'n' is the number of particles in moles, 'T' is the temperature in Kelvin and 'R' is the ideal gas constant (0.0821 liter atmospheres per moles Kelvin)

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Which chemical equation is unbalanced? c o2 right arrow. co2 sr o2 right arrow. 2sro 6h2 3o2 right arrow. 6h2o h2 h2 o2 right ar
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The unbalanced equation is one in which the moles of atoms are not equal on both sides of the reaction.

<h3>What is a balanced chemical equation?</h3>

A balanced chemical equation is one in wgich the moles of atoms in the reactants side is equal to the moles of atoms on the product side.

The given equations of reaction is not clearly stated.

Therefore, the unbalanced equation is one in which the moles of atoms are not equal on both sides of the reaction.

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3 years ago
A 1.0 mole sample of fluorine gas at 25 °C has an average molecular velocity of 415 m/s. What is the total KE of the gas sample?
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The total kinetic energy of the gas sample is 3.3 KJ

<h3>What is kinetic energy? </h3>

This is the energy possessed by an object in motion. Mathematically, it can be expressed as:

KE = ½mv²

Where

  • KE is the kinetic energy
  • m is the mass
  • v is the velocity

<h3>How to determine the mass of the fluorine gas</h3>
  • Molar mass of fluorine gas = 38 g/mol
  • Mole of fluorine gas = 1 mole
  • Mass of fluorine gas = ?

Mass = mole × molar mass

Mass of fluorine gas = 1 × 38

Mass of fluorine gas = 38 g

<h3>How to determine the KE of the gas sample</h3>
  • Mass (m) = 38 g = 38 / 1000 = 0.038 Kg
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KE = ½mv²

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Divide by 1000 to express in kilojoule

KE = 3272.275 / 1000

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