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Chemical properties of insecticides

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Answer from: Quest

Hello!

How many mL of a 12.5% (by volume) solution of ethanol are required to produce 175 mL of 0.664 M acetic acid? (density of pure ethanol = 0.789 g/mL)

$C_2H_5OH(aq) + O_2(g) \Longrightarrow HC_2H_3O_2(aq) + H_2O$

We have the following data:

% m1/m (percent by solute mass/solution mass) = 12.5

Molar Mass (MM) of ethanol (C2H5OH) ≈ 46.07 g/mol

M1 (molarity) = 0.664 M (or 0.664 mol/L)

V1 (initial volume) = 175 ml = 0.175 L

n (number of mol) = ?

m1 (solute mass - ethanol) = ?

m (solution mass) = ?

d (density of pure ethanol) = 0.789 g/ml

v (volume of pure ethanol) = ? (in ml)

Solving:

[First Step] Let's find the number of moles or matter number, let's see:

If:

n_1 = n_2

M_1*V_1 = M_2*V_2

M_1*V_1 = n_2

n_2 = M_1*V_1

$n_2 = 0.664\:\dfrac{mol}{\diagup\!\!\!\!L} * 0.175\:\diagup\!\!\!\!L$

$\boxed{n_2 = 0.1162\:mol}$

[Second Step] We apply the data to the Molarity or Molar Concentration formula and find the mass of the solute (m1), let's see:

$M_1 = \dfrac{m_1}{MM*V_1}$

m_1 = M_1*V_1*MM

m_1 = n_2*MM

$m_1 = 0.1162\:mol\!\!\!\!\!\!\!\!\!\!\!\dfrac{\hspace{0.6cm}}{~}*46.07\:\dfrac{g}{mol\!\!\!\!\!\!\!\!\!\!\!\dfrac{\hspace{0.6cm}}{~}}$

$m_1 = 5.353334\:g\to \boxed{m_1 \approx 5.36\:g}$

[Third Step] We apply the data to the formula of percent solute mass per solution mass and let's find the solution mass, let's see:

$\%\:m_1/m = \dfrac{m_1}{m}*100$

$12.5 = \dfrac{5.36}{m}*100$

12.5*m = 5.36*100

$12.5\:m = 536$

$m = \dfrac{536}{12.5}$

$\boxed{m = 42.88\:g}$

[Fourth Step] We apply the data to the density formula and let's find the volume of ethanol, let's see:

$d = \dfrac{m}{v}$

$v = \dfrac{m}{d}$

$v = \dfrac{42.88\:\diagup\!\!\!\!\!g}{0.789\:\dfrac{\diagup\!\!\!\!\!g}{ml} }$

$\boxed{\boxed{v \approx 54.3\:ml}}\:\:\:\:\:\:\bf\blue{\checkmark}$

The volume is approximately 54.3 ml

________________________

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Answer from: Quest

Atomic Symbol of Oxygen is "O"
Atomic Number is "8"

Answer from: Quest

Molarity of solution: 1.1884 M

Further explanation

The concentration of a substance can be expressed in several quantities such as moles, percent (%) weight / volume,), molarity, molality, parts per million (ppm) or mole fraction. The concentration shows the amount of solute in a unit of the amount of solvent.

Molarity shows the number of moles of solute in every 1 liter of solution or mmol in each ml of solution

$\rm M=\dfrac{n}{V}$

Where

M = Molarity

n = Number of moles of solute

V = Volume of solution

Mole itself is the number of particles contained in a substance

1 mole = 6.02.10²³ particles

Mole can be obtained if the amount of substance mass and its molar mass is known

$\rm mole=\dfrac{mass}{molar\:mass}$

Given

KOH (Potassium hydroxide)

Molar mass: Ar K + Ar O + Ar H

molar mass: 39,0983 + 15,999 + 1,008

molar mass: 56.1053 g / mol

15 g of KOH

225 ml of solution = 0.225 L

Asked

The molar concentration of a solution

Solution

$\rm mole=\dfrac{15}{56.1053}\\\\mole=0.2674$

Molarity (M) of a solution

$\rm M=\dfrac{mole}{V}\\\\M=\dfrac{0.2674}{0.225}\\\\M=\boxed{\bold{1.1884}}$

Learn more

atoms in 5.1 moles of Sulfur

the mole fractions of the solute and the solvent

moles of CaCO3

the mole ratio of Al to Cl2

#LetsStudy

Answer from: Quest

I think the answer is the first one, physical

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