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3 years ago

What is the final concentration if 50.0 ml of a 2.00 m solution are diluted to 500.0 ml??

1 answer:

4 0

In order to calculate the final concentration of a dilution, it is important to memorise and remember the following equation:

C1V1/C2V2
Where:
C1 = Initial concentration
V1 = Initial volume
C2 = Final concentration
V2 = Final volume

We are given three of the four, and we are asked to calculate the final concentration in moles, so we may substitute these given values into our equation as follows:

C1V1 = C2V2
(2.00m)(50.0 mL) = (C2)(500mL)
100 = C2(500mL)
C2 = 0.2 m

In the final step, we simply divide 100 by 500 to get our final concentration value.

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Suppose 0.245 g of sodium chloride is dissolved in 50. mL of a 18.0 m M aqueous solution of silver nitrate.

Bezzdna [24]

Answer:

$\large \boxed{\text{ 0.066 mol/L}}$

Explanation:

We are given the amounts of two reactants, so this is a limiting reactant problem.

1. Assemble all the data in one place, with molar masses above the formulas and other information below them.

Mᵣ: 58.44

NaCl + AgNO₃ ⟶ NaNO₃ + AgCl

m/g: 0.245

V/mL: 50.

c/mmol·mL⁻¹: 0.0180

2. Calculate the moles of each reactant

$\text{Moles of NaCl} = \text{245 mg NaCl} \times \dfrac{\text{1 mmol NaCl}}{\text{58.44 mg NaCl}} = \text{4.192 mmol NaCl}\\\\\text{ Moles of AgNO}_{3}= \text{50. mL AgNO}_{3} \times \dfrac{\text{0.0180 mmol AgNO}_{3}}{\text{1 mL AgNO}_{3}} = \text{0.900 mmol AgNO}_{3}$

3. Identify the limiting reactant

Calculate the moles of AgCl we can obtain from each reactant.

From NaCl:

The molar ratio of NaCl to AgCl is 1:1.

$\text{Moles of AgCl} = \text{4.192 mmol NaCl} \times \dfrac{\text{1 mmol AgCl}}{\text{1 mmol NaCl}} = \text{4.192 mmol AgCl}$

From AgNO₃:

The molar ratio of AgNO₃ to AgCl is 1:1.

$\text{Moles of AgCl} = \text{0.900 mmol AgNO}_{3} \times \dfrac{\text{1 mmol AgCl}}{\text{1 mmol AgNO}_{3}} = \text{0.900 mmol AgCl}$

AgNO₃ is the limiting reactant because it gives the smaller amount of AgCl.

4. Calculate the moles of excess reactant

Ag⁺(aq) + Cl⁻(aq) ⟶ AgCl(s)

I/mmol: 0.900 4.192 0

C/mmol: -0.900 -0.900 +0.900

E/mmol: 0 3.292 0.900

So, we end up with 50. mL of a solution containing 3.292 mmol of Cl⁻.

5. Calculate the concentration of Cl⁻

$\text{[Cl$^{-}$] } = \dfrac{\text{3.292 mmol}}{\text{50. mL}} = \textbf{0.066 mol/L}\\\text{The concentration of chloride ion is $\large \boxed{\textbf{0.066 mol/L}}$}$

8 0

3 years ago

Identify and label the Brønsted-Lowry acid, its conjugate base, the Brønsted-Lowry base, and its conjugate acid in each of the f

julia-pushkina [17]

Explanation:

As per Brønsted-Lowry concept of acids and bases, chemical species which donate proton are called Brønsted-Lowry acids.

The chemical species which accept proton are called Brønsted-Lowry base.

(a) $HNO_3 + H_2O \rightarrow H_3O^+ + NO_3^-$

$HNO_3$ is Bronsted lowry acid and $NO_3^-$ is its conjugate base.

$H_2O$ is Bronsted lowry base and $H_3O^+$ is its conjugate acid.

(b)

$CN^- + H_2O \rightarrow HCN + OH^-$

$CN^-$ is Bronsted lowry base and HCN is its conjugate acid.

$H_2O$ is Bronsted lowry acid and $OH^-$ is its conjugate base.

(c)

$H_2SO_4 + Cl^- \rightarrow HCl + HSO_4^-$

$H_2SO_4$ is Bronsted lowry acid and $HSO_4^-$ is its conjugate base.

Cl^- is Bronsted lowry base and HCl is its conjugate acid.

(d)

$HSO_4^-+OH^- \rightarrow SO_4^{2-}+H_2O$

$HSO_4^-$ is Bronsted lowry acid and $SO_4^{2-}$ is its conjugate base.

OH^- is Bronsted lowry base and $H_2O$ is its conjugate acid.

(e)

$O_{2-}+H_2O \rightarrow 2OH^-$

$O_{2-}$ is Bronsted lowry base and OH- is its conjugate acid.

$H_2O$ is Bronsted lowry acid and OH- is its conjugate base.

6 0

4 years ago

Sulfur hexafluoride is represented by

katrin2010 [14]

Elagas

Esaflon
Sulfur(VI) fluoride

Sulfuric fluoride

4 0

4 years ago

Read 2 more answers

A scientist is measuring the pressure that is exerted by each of the following gases in the atmosphere: carbon dioxide,

Pani-rosa [81]

Answer:

D. Partial pressure

Explanation:

Partial pressure is the individual pressure exerted by each gas present in a gaseous mixture. As he is measuring the pressure of each gas in the atmosphere separately, so PARTIAL PRESSURE is the exact term for his measurement.

8 0

3 years ago

What is the poH of a 3.67 x 10-5 M OH solution and is it acidic, basic, or neutral?

Anni [7]

Answer:

The pOH is 4, 44 and the solution is basic.

Explanation:

The pOH is a measure of the concentration of OH (hydroxyl) ions in the solution.

The pOH is calculated as :

pOH = -log (OH-)= -log (3.67 x 10-5 )= 4, 44. In this case, the solution is basic.

The p0H scale ranges from values of 0 to 14 (less than 7.0 is basic and greater than 7.0 is acidic, a pH = 7.0 is neutral)

3 0

3 years ago