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2 years ago

at standard pressure, what is the temperature at which a saturated solution of NH4Cl has a concentration of 60g NH4CL/100 g H2O

Chemistry

1 answer:

Nataliya [291]2 years ago

5 0

Answer: Temperature = T, unknown

Saturated Solution, NH4Cl concentration = 60g/100g H2O = 0.6g NH4Cl/g H2O

Assume density of H2O = 1 g/ml

m = 0.6g NH4Cl/g H2O / 1 g/ml

m = 0.6g NH4Cl/ml

See the table of saturated solutions and identify the temperature at which the concentration of NH4Cl is 60g/100g H2O.

Explanation: The line on the graph on reference table G indicates a saturated solution of NH4CL as a concentration of 60. g NH4 Cl/100. g H2O

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3 years ago

If the solubility of sodium chloride is 36 grams per 100 grams of water, which of the following solutions would be considered un

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Answer: If the solubility of sodium chloride is 36 grams per 100 grams of water then 5.8 moles of NaCl dissolved in 1 L of water solution would be considered unsaturated.

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A solution which contains the maximum amount of solute is called a saturated solution. Whereas a solution in which more amount of solute is able to dissolve is called an unsaturated solution.

Now, the number of moles present in 36 g of NaCl (molar mass = 58.4 g/mol) is as follows.

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So, a solution in which number of moles of NaCl are less than 0.616 mol per 100 mL then the solution formed will be an unsaturated solution.

As 5.8 moles of NaCl dissolved in 1 L (or 1000 mL) of water. So, moles present in 100 mL are calculated as follows.

$Moles = \frac{5.8 mol}{1000 mL} \times 100 mL\\= 0.58 mol$

Moles present in 100 mL of water for 3.25 moles of NaCl dissolved in 500 ml in water are as follows.

$Moles = \frac{3.25 mol}{500 mL} \times 100 mL\\0.65 mol$

Moles present in 100 mL of water for 1.85 moles of NaCl dissolved in 300 ml of water are as follows.

$Moles = \frac{1.85 mol}{300 mL} \times 100 mL\\= 0.616 mol$

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