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2 years ago

What mass of nacl is in 0.600 l of 0.250 m solution?

Chemistry

1 answer:

kipiarov [429]2 years ago

4 0

Answer:

8.77 grams NaC

Explanation:

To find the mass of NaCl, you need to (1) use the molarity equation to find moles, then (2) calculate the molar mass of NaCl (via the periodic table), and then (3) convert moles NaCl to grams (via molar mass). The final answer should have 3 sig figs because the given values also have 3 sig figs.

(Step 1)

Molarity (M) = moles / volume (L)

0.250 M = moles / 0.600 L

(0.250 M) x (0.600 L) = moles

0.150 = moles

(Step 2)

Molar Mass (NaCl): 22.99 g/mol + 35.45 g/mol

Molar Mass (NaCl): 58.44 g/mol

(Step 3)

0.150 moles NaCl 58.44 g
--------------------------- x ------------------- = 8.77 grams NaCl
1 mole

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3 years ago

Calculate the freezing point (in degrees C) of a solution made by dissolving 7.99 g of anthracene{C14H10} in 79 g of benzene. Th

mario62 [17]

<u>Answer:</u> The freezing point of solution is 2.6°C

<u>Explanation:</u>

To calculate the depression in freezing point, we use the equation:

$\Delta T_f=iK_fm$

Or,

$\Delta T_f=i\times K_f\times \frac{m_{solute}\times 1000}{M_{solute}\times W_{solvent}\text{ in grams}}$

where,

$\Delta T_f$ = $\text{Freezing point of pure solution}-\text{Freezing point of solution}$

Freezing point of pure solution = 5.5°C

i = Vant hoff factor = 1 (For non-electrolytes)

$K_f$ = molal freezing point depression constant = 5.12 K/m = 5.12 °C/m

$m_{solute}$ = Given mass of solute (anthracene) = 7.99 g

$M_{solute}$ = Molar mass of solute (anthracene) = 178.23 g/mol

$W_{solvent}$ = Mass of solvent (benzene) = 79 g

Putting values in above equation, we get:

$5.5-\text{Freezing point of solution}=1\times 5.12^oC/m\times \frac{7.99\times 1000}{178.23g/mol\times 79}\\\\\text{Freezing point of solution}=2.6^oC$