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Alex777 [14]
3 years ago
12

What mass of Sodium Chloride is required to make 100.0 mL of 3.0 M solution?

Chemistry
1 answer:
Julli [10]3 years ago
5 0

Answer:

17.55 g of NaCl

Explanation:

The following data were obtained from the question:

Molarity = 3 M

Volume = 100.0 mL

Mass of NaCl =..?

Next, we shall convert 100.0 mL to L. This can be obtained as follow:

1000 mL = 1 L

Therefore,

100 mL = 100/1000

100 mL = 0.1 L

Therefore, 100 mL is equivalent to 0.1 L.

Next, we shall determine the number of mole NaCl in the solution. This can be obtained as follow:

Molarity = 3 M

Volume = 0.1 L

Mole of NaCl =?

Molarity = mole /Volume

3 = mole of NaCl /0.1

Cross multiply

Mole of NaCl = 3 × 0.1

Mole of NaCl = 0.3 mole

Finally, we determine the mass of NaCl required to prepare the solution as follow:

Mole of NaCl = 0.3 mole

Molar mass of NaCl = 23 + 35.5 = 58.5 g/mol

Mass of NaCl =?

Mole = mass /Molar mass

0.3 = mass of NaCl /58.5

Cross multiply

Mass of NaCl = 0.3 × 58.5

Mass of NaCl = 17.55 g

Therefore, 17.55 g of NaCl is needed to prepare the solution.

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What is the molarity when water is added to 4 moles of sodium chloride to make 0.5 liter of solution?
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       If    0.5 L of solution contains 4 mol
then let     1 L of solution contain  x  mol
      
       ⇒    (0.5 L) x  = (4 mol) (1 L)

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Calculate the density of a solid that has a volume of 2cm3 and a mass of 3g
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At equilibrium, the concentrations in this system were found to be [N21 O20.200 M and [NO]0.500 M. N2(8) 02e) 2NO(g) If more NO
erastovalidia [21]

Answer : The concentration of NO at equilibrium is 0.9332 M

Solution :  Given,

Concentration of N_2 and O_2 at equilibrium = 0.200 M

Concentration of N_2 and O_2 at equilibrium = 0.500 M

First we have to calculate the value of equilibrium constant.

The given equilibrium reaction is,

N_2(g)+O_2(g)\rightleftharpoons 2NO(g)

The expression of K_c will be,

K_c=\frac{[NO]^2}{[N_2][O_2]}

K_c=\frac{(0.500)^2}{(0.200)\times (0.200)}

K_c=6.25

Now we have to calculate the final concentration of NO.

The given equilibrium reaction is,

                         N_2(g)+O_2(g)\rightleftharpoons 2NO(g)

Initially             0.200   0.200         0

.800

At equilibrium  (0.200-x) (0.200-x)  (0.800+2x)

The expression of K_c will be,

K_c=\frac{[NO]^2}{[N_2][O_2]}

K_c=\frac{(0.800+2x)^2}{(0.200-x)\times (0.200-x)}

By solving the term x, we get

x=2.6\text{ and }-0.0666

From the values of 'x' we conclude that, x = 2.6 can not more than initial concentration. So, the value of 'x' which is equal to 2.6 is not consider.

And the negative value of 'x' shows that the equilibrium shifts towards the left side (reactants side).

Thus, the concentration of NO at equilibrium = (0.800+2x) = 0.800 + 2(0.0666) = 0.9332 M

Therefore, the concentration of NO at equilibrium is 0.9332 M

5 0
3 years ago
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