4.) Calculate the molality of the following aqueous solutions: a) 250 mL of 2.90 M NaCl solution (density of solution = 1.12 g/mL). b) 335 mL 0.87 M NaOH solution (density of solution = 1.04 g/mL). c) 525 mL 6.25 M NaHCO3 solution (density of solution = 1.19 g/mL).
4.) Calculate the molality of the following aqueous solutions: a) 250 mL of 2.90 M NaCl solution (density of solution = 1.12 g/mL). b) 335 mL 0.87 M NaOH solution (density of solution = 1.04 g/mL). c) 525 mL 6.25 M NaHCO3 solution (density of solution = 1.19 g/mL).
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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I’m stuck with part 4 please can you explain for me
![4.) Calculate the molality of the following aqueous solutions:
a) 250 mL of 2.90 M NaCl solution (density of solution = 1.12 g/mL).
b) 335 mL 0.87 M NaOH solution (density of solution = 1.04 g/mL).
c) 525 mL 6.25 M NaHCO3 solution (density of solution = 1.19 g/mL).
5.) A solution of 0.250 g of naphthalene in 35.00 g of camphor (pure solvent) lowers the
freezing point by 2.10 degrees Celsius. What is the molar mass of naphthalene? The
freezing point depression constant for camphor is 37.7 (°C kg/mol).
6.) A solution is prepared by dissolving 35.0 g of hemoglobin (Hb) in enough water to
make up 1 L in volume. If the osmotic pressure of the solution is found to be 10.0 mmHg
at 25 °C, calculate the molar mass of hemoglobin.
7.) Consider the reaction: A + B --→ products.
From the following data obtained at a certain temperature, determine the order of the
reaction (rate law) and calculate the rate constant:
[A] (M)
[B] (M)
1.50
1.50
#
1.50
2.50
$
Rate (M/s)
3.15 X 10-1.
2.98 X 10-1
MacBook Pro
&
7
8](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd3840565-ac9f-4952-a30d-6589a9cae738%2Fb6687194-c017-4634-9a2d-926f2b244c9f%2Fp1n21xo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:4.) Calculate the molality of the following aqueous solutions:
a) 250 mL of 2.90 M NaCl solution (density of solution = 1.12 g/mL).
b) 335 mL 0.87 M NaOH solution (density of solution = 1.04 g/mL).
c) 525 mL 6.25 M NaHCO3 solution (density of solution = 1.19 g/mL).
5.) A solution of 0.250 g of naphthalene in 35.00 g of camphor (pure solvent) lowers the
freezing point by 2.10 degrees Celsius. What is the molar mass of naphthalene? The
freezing point depression constant for camphor is 37.7 (°C kg/mol).
6.) A solution is prepared by dissolving 35.0 g of hemoglobin (Hb) in enough water to
make up 1 L in volume. If the osmotic pressure of the solution is found to be 10.0 mmHg
at 25 °C, calculate the molar mass of hemoglobin.
7.) Consider the reaction: A + B --→ products.
From the following data obtained at a certain temperature, determine the order of the
reaction (rate law) and calculate the rate constant:
[A] (M)
[B] (M)
1.50
1.50
#
1.50
2.50
$
Rate (M/s)
3.15 X 10-1.
2.98 X 10-1
MacBook Pro
&
7
8
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