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Ilia_Sergeevich [38]
3 years ago
5

What is the final concentration if water is added to 0.50 L of a 12 M NaOH solution to make 3.0 L of a diluted NaOH solution?

Chemistry
2 answers:
Kisachek [45]3 years ago
6 0

Answer:

2 M NaOH solution

Explanation:

Initial concentration of NaOH = 12 M

Initial volume of solution = 0.5

Initial number of moles = Molarity×Volume = 12×0.5 = 6 moles

Note: On dilution the number of moles does not change.

Initial number of moles = final number of moles.

Final number of moles = 6 moles

Final volume of solution = 3 L

Final concentration (in Molarity) = \frac{Final\ no\ of\ moles}{final\ volume\ in\ L}=\frac{6}{3}= 2\ M

SVETLANKA909090 [29]3 years ago
3 0

Answer:

The answer to your question is the second option: 2M NaOH solution

Explanation:

Data

Volume 1 = 0.5 l

Concentration 1 = 12 M NaOH

Volume 2 = 3 l

Concentration 2 = ?

Formula

                     V₁C₁  =  V₂C₂

Solve for C₂

                     C₂ = V₁C₁ / V₂

Substitution

                    C₂ = (0.5)(12) / 3

Simplification and result

                    C₂ = 6 / 3

                    C₂ = 2 M  

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Consider the reaction below for which K = 78.2 atm-1. A(g) + B(g) ↔ C(g) Assume that 0.386 mol C(g) is placed in the cylinder re
borishaifa [10]

Answer:

1.65 L

Explanation:

The equation for the reaction is given as:

                        A            +            B           ⇄        C

where;

numbers of moles = 0.386 mol C  (g)

Volume =  7.29 L

Molar concentration of C = \frac{0.386}{7.29}

= 0.053 M

                        A            +            B           ⇄        C

Initial               0                           0                      0.530    

Change          +x                          +x                       - x

Equilibrium      x                           x                      (0.0530 - x)

K = \frac{[C]}{[A][B]}

where

K is given as ; 78.2 atm-1.

So, we have:

78.2=\frac{[0.0530-x]}{[x][x]}

78.2= \frac{(0.0530-x)}{(x^2)}

78.2x^2= 0.0530-x

78.2x^2+x-0.0530=0  

Using quadratic formula;

\frac{-b+/-\sqrt{b^2-4ac} }{2a}

where; a = 78.2 ; b = 1 ; c= - 0.0530

= \frac{-b+\sqrt{b^2-4ac} }{2a}   or \frac{-b-\sqrt{b^2-4ac} }{2a}

= \frac{-(1)+\sqrt{(1)^2-4(78.2)(-0.0530)} }{2(78.2)}  or \frac{-(1)-\sqrt{(1)^2-4(78.2)(-0.0530)} }{2(78.2)}

= 0.0204  or -0.0332

Going by the positive value; we have:

x = 0.0204

[A] = 0.0204

[B] = 0.0204

[C] = 0.0530 - x

     = 0.0530 - 0.0204

     = 0.0326

Total number of moles at equilibrium = 0.0204 +  0.0204 + 0.0326

= 0.0734

Finally, we can calculate the volume of the cylinder at equilibrium using the ideal gas; PV =nRT

if we make V the subject of the formula; we have:

V = \frac{nRT}{P}

where;

P (pressure) = 1 atm

n (number of moles) = 0.0734 mole

R (rate constant) = 0.0821 L-atm/mol-K

T = 273.15 K  (fixed constant temperature )

V (volume) = ???

V=\frac{(0.0734*0.0821*273.15)}{(1.00)}

V = 1.64604

V ≅ 1.65 L

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Explanation:

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