A solution was made by dissolving 5.50 mg of hemoglobin in water
to give a final...
A solution was made by dissolving 5.50 mg of hemoglobin in water
to give a final volume of 1.00 mL. The osmotic pressure of this
solution was 2.10×10-3 atm at 25.0°C.
A solution is prepared by dissolving 50.4g sucrose
(C12H22O11) in 0.332kg of water.
The final volume of thesolution is 355 mL. Calculate the
concentration of the solution in each unit?
Molarity
Molality
Percent by mass
Mole fraction
mole percent.
A solution is made by dissolving 0.0100 mol of HF in 1.00 kg of
water. The solution was found to freeze at –0.0236 °C. Calculate
the value of i and estimate the percent ionization of HF in this
solution.
i =____ so HF is ______
A solution is made by dissolving 0.0100 mol of HF in 1.00 kg of
water. The solution was found to freeze at –0.0236 °C. Calculate
the value of i and estimate the percent ionization of HF in this
solution.
i =____ so HF is ______
A solution is made by dissolving 18.29g of glucose
C6H12O2 in 50mL of water at 25C
Calculate the molality,molarity, percent mass, Assume density of
water is 1.00g/ml
a
solution if phosphoric acid was made by dissolving 10g of H3PO4 in
100mL of water. the resulting volume was 104mL. calculate the
density, mole fraction, molarity, and molality of the solution.
assume water has a density of 1g/cm3
Would the pH of a solution made by dissolving the following solids
in water be less than 7, be equal to 7, or greater than 7? Explain.
A) NaCl
B) NaF
C) AlCl3
A solution is prepared by dissolving 50.8 g sucrose(C12H22O11)
in 0.387 kg of water. The final volume of the solution is 355
mL.
For this solution, calculate molarity.
For this solution, calculate molality.
For this solution, calculate percent by mass.
For this solution, calculate mole fraction.
You prepare a solution by dissolving 50.4g sucrose (C12H22O11) in
0.332 kg of water. The final volume of the solution is 355 mL.
Calculate the concentration of the solution in each unit.
1 mole C12H22O11 = 342.296 g sucrose
(a) Molarity
(b) Molality
(c) Percent by mass
(d) Mole fraction
A solution
is made by dissolving 0.4352g of nickel through water to make a
500.0 mL solution. A dilution is made by pipeting 2.00 mL into a
250.0 mL volumetric flask and bring it to volume with distilled
water. What is the parts per million, ppm, concentration of nickel
in the dilution?
A solution is made by dissolving 10.0 g of sodium chloride in
110.5 g of water at 25oC. The density of the solution is 1.021
g/mL
1.What is the osmotic pressure of this solution?
2.What is the boiling point of this solution?
3.What is the freezing point of this solution?