Now sure how to do this!
1. DESCRIBE & CALCULATE how to make 750. mL of a 1.25 M sucrose solution
2. Concentrated HCl has a molarity of 12 M. DESCRIBE & CALCULATE how to make 1.50 L of a 3.00 M HCl.
a. 1.25M=molesSucrose/.75
moles Sucrose=1.25*.75
grams sucrose= molesSucrose*342.3
put sucrose in a beaker, add water to 750ml mark, stir, and label.
2. You want 1.50L, so in that you have 1.50*3 moles HCL, or 4.5moles
determine the volume of 12 molar in which you get 4.5moles
4.5/volume=12
volume=4.5/12 liters=375ml
so, always adding acid to water, put about 900mlof water in a beaker, add 375ml 12 molar acid slowly, stiring. When mixed, add water up to the 1.5Liter mark. label, and safely store.
Is 1 or part A's answer then 321
and question 2's answer is 375...??
1. To prepare 750 mL of a 1.25 M sucrose solution, you will need to follow these steps:
Step 1: Determine the amount of sucrose needed.
The formula to calculate the amount of solute needed is:
moles = concentration (M) × volume (L)
In this case, the concentration is 1.25 M and the volume is 0.75 L (since 750 mL is equivalent to 0.75 L).
moles of sucrose = 1.25 M × 0.75 L = 0.9375 moles
Step 2: Convert moles of sucrose to grams.
The molar mass of sucrose (C12H22O11) is 342.3 g/mol.
mass of sucrose = moles of sucrose × molar mass of sucrose
mass of sucrose = 0.9375 moles × 342.3 g/mol = 320.44 g (round to the nearest hundredth)
Step 3: Dissolve the calculated mass of sucrose in enough solvent to make a total volume of 750 mL.
To do this, you can follow these sub-steps:
- Weigh out 320.44 g of sucrose using a balance.
- Transfer the sucrose into a beaker or container.
- Add a small amount of water to dissolve the solid.
- Once dissolved, add water to bring the total volume up to 750 mL.
Now you have prepared 750 mL of a 1.25 M sucrose solution.
2. To prepare 1.50 L of a 3.00 M HCl solution using concentrated HCl with a molarity of 12 M, you will need to perform a dilution using the following steps:
Step 1: Determine the volume of concentrated HCl needed.
The dilution formula is:
C1V1 = C2V2
Where:
C1 = initial concentration (12 M)
V1 = initial volume (unknown)
C2 = final concentration (3 M)
V2 = final volume (1.50 L)
Substituting the values into the formula, we get:
(12 M) × V1 = (3 M) × (1.50 L)
V1 = (3 M × 1.50 L) / 12 M
V1 = 0.375 L (or 375 mL)
Step 2: Measure 375 mL of concentrated HCl using a graduated cylinder or pipette.
Step 3: Add the measured 375 mL of concentrated HCl into a 1.50 L volumetric flask.
Step 4: Fill the remaining volume of the flask with distilled water to reach the 1.50 L mark.
Now you have prepared 1.50 L of a 3.00 M HCl solution through dilution.
To describe and calculate how to prepare a certain volume and concentration of a solution, you will need to use the concepts of molarity and dilution. Molarity is defined as the number of moles of solute per liter of solution, while dilution involves adding solvent to a concentrated solution to decrease its concentration.
1. To make a 750 mL of a 1.25 M sucrose solution:
a. Determine the number of moles of sucrose needed. This is calculated using the equation:
Moles of solute = Molarity × Volume (in liters)
In this case, the volume is in milliliters, so convert it to liters by dividing by 1000:
Moles of sucrose = 1.25 M × 0.750 L
b. Calculate the mass of sucrose needed. This requires the molar mass of sucrose, which is approximately 342.3 g/mol:
Mass of sucrose = Moles of sucrose × Molar mass of sucrose
Substitute the value of moles from step (a) into the equation:
Mass of sucrose = (1.25 M × 0.750 L) × 342.3 g/mol
c. Add the calculated mass of sucrose to a container. Then, add enough solvent (usually water) to bring the total volume to 750 mL. Stir until the sucrose completely dissolves.
2. To make 1.50 L of a 3.00 M HCl:
a. Determine the number of moles of HCl needed. This is calculated using the same equation as in step (1a):
Moles of solute = Molarity × Volume
Convert the volume to liters:
Moles of HCl = 3.00 M × 1.50 L
b. Calculate the volume of concentrated HCl required. This can be obtained by applying the equation:
Moles = Molarity × Volume
Rearrange the equation to solve for volume:
Volume = Moles ÷ Molarity
Substitute the values calculated earlier:
Volume = (3.00 M × 1.50 L) ÷ 12 M
This will give you the volume of the concentrated HCl in liters.
c. Add the calculated volume of concentrated HCl to a container, then add water (solvent) to reach the target volume of 1.50 L. Be cautious when handling and diluting concentrated acids, as they can be hazardous. It is recommended to follow appropriate safety measures and dilute acids slowly, while stirring gently.