this is a really long question. i don't understand how to answer it. help please.

A 10.0% aquueous solution of sulfuric acid has a density of 1.0661 g/mL at 20 degrees celsius.
A. how many grams of H2SO4 are found in 50.0 g of this solution?
B. how many grams of water are found in 50.0 g of this solution?
C. What mass of H2SO4 must be mixed with 50.0 g of water to make this solution?
D. how many grams of H2SO4 are required to make 50.0 mL of this solution?
E. what volume of this solution contains 50.0 g of H2SO4?
F. what is the molarity of this solution?
G. assuming a complete dissociation of H2SO4 in water (H2SO4 ---> 2H^- + SO4^-2) what is the normality of the solution?
H. what is the gram-equivalent mass of H2SO4 given in the dissociation in (g)?
I. how many equivalents of H2SO4 are in 50.0 g of this solution?
J. what is the molality of this solution?
K. what is the particle molality of of this solution?
L. what is the boiling point of this solution?
M. what is the freezing point of this solution?
N. what is the osmotic pressure of this solution? hint: use information from (f)
PLEASE HELP

You need to be aware of the definitions. I can get you started. For A, remember the definition of % by mass is

(mass solute/mass soln)*100 = % w/w.
Therefore, you have 10 g H2SO4/100 g solution. You want to know how many g H2SO4 are in 50 g of this solution. Of course that's just half or 5 g H2SO4 but you work that out by
10 g H2SO4 x (50/100) = ?

B.
If you have a 10% w/w solution it means 10 g solute + 90 g water. So 90 g H2O in the original means 5 g solute in 45 g H2O (to make a total of 50 g).
Using these two examples you need to try your hand at these.

To answer these questions, we need to apply various concepts and calculations related to solution chemistry. Let's go through each question and explain how to find the answer step by step.

A. How many grams of H2SO4 are found in 50.0 g of this solution?
To answer this question, we need to determine the mass of H2SO4 in 50.0 g of the solution. Since the solution is 10% sulfuric acid, we can use the mass percentage formula:
Mass of H2SO4 = (10/100) * mass of solution
Substituting the given values:
Mass of H2SO4 = (10/100) * 50.0 g

B. How many grams of water are found in 50.0 g of this solution?
Similarly, to find the mass of water in the solution, we can subtract the mass of H2SO4 from the total mass of the solution:
Mass of water = mass of solution - mass of H2SO4

C. What mass of H2SO4 must be mixed with 50.0 g of water to make this solution?
To answer this question, we need to determine the mass of H2SO4 needed to make the solution. Since the mass of water is given, we can subtract it from the total mass of the solution:
Mass of H2SO4 = mass of solution - mass of water

D. How many grams of H2SO4 are required to make 50.0 mL of this solution?
Here, we need to determine the mass of H2SO4 required to make a specific volume of the solution. Since the density of the solution is given, we can use the formula:
Mass of H2SO4 = Volume of solution * Density of solution

E. What volume of this solution contains 50.0 g of H2SO4?
To find the volume of the solution containing a certain mass of H2SO4, we can rearrange the formula from the previous question:
Volume of solution = Mass of H2SO4 / Density of solution

F. What is the molarity of this solution?
Molarity is defined as the number of moles of solute (H2SO4) per liter of the solution. To find the molarity, we need to first calculate the number of moles of H2SO4. The formula for moles is:
Moles of H2SO4 = Mass of H2SO4 / Molar mass of H2SO4
Then, we divide the moles by the volume of the solution in liters to calculate the molarity:
Molarity = Moles of H2SO4 / Volume of solution (in liters)

G. Assuming complete dissociation of H2SO4 in water, what is the normality of the solution?
Normality is the number of equivalents of a solute (H2SO4) per liter of the solution. Since sulfuric acid dissociates into two H+ ions and one SO4^-2 ion, the equivalent weight of H2SO4 is half its molar mass. The formula for normality is:
Normality = Molarity * N, where N is the number of H+ ions contributed per molecule of H2SO4

H. What is the gram-equivalent mass of H2SO4 given in the dissociation (in g)?
Gram-equivalent mass is the molar mass divided by the number of equivalents. In this case, since H2SO4 is monoprotic (donates one H+ ion), the gram-equivalent mass is equal to the molar mass.

I. How many equivalents of H2SO4 are in 50.0 g of this solution?
To calculate the number of equivalents, we divide the given mass of H2SO4 by its gram-equivalent mass.

J. What is the molality of this solution?
Molality is defined as moles of solute (H2SO4) per kilogram of solvent (water). To calculate the molality, we need to first calculate the number of moles of H2SO4, and then divide it by the mass of water (in kg).

K. What is the particle molality of this solution?
Particle molality refers to the number of particles of solute (H2SO4) per kilogram of solvent (water). Since sulfuric acid dissociates into three particles (two H+ ions and one SO4^-2 ion), the particle molality would be three times the molality.

L. What is the boiling point of this solution?
To determine the boiling point elevation, we need to know the molality of the solution and the boiling point elevation constant of water (which is a colligative property). The formula to calculate the change in boiling point is:
Change in boiling point = molality * boiling point elevation constant
The boiling point of the solution is then calculated by adding the change in boiling point to the boiling point of pure water.

M. What is the freezing point of this solution?
Similar to the previous question, to determine the freezing point depression, we need the molality of the solution and the freezing point depression constant of water. The formula is:
Change in freezing point = molality * freezing point depression constant
The freezing point of the solution is then calculated by subtracting the change in freezing point from the freezing point of pure water.

N. What is the osmotic pressure of this solution?
The osmotic pressure of a solution can be calculated using the formula:
Osmotic pressure = (Molarity * R * Temperature), where R is the ideal gas constant and Temperature is in Kelvin.

Please note that to obtain the exact answers to these questions, specific values for molar mass, boiling point elevation constant, freezing point depression constant, and the ideal gas constant should be used.