I know everyone guessed i had a few more i couldn't do. Sorry but assistance please:
1.Sucralfate (molecular weight: 2087g/mol) is a major component of Carafate® which is prescribed for the treatment of gastrointestinal ulcers. The recommended dose for a duodenal ulcer is 1g taken orally in 10 mL (2 teaspoons) of a solution four times a day. Calculate the molarity of the solution.
a 0.010 M
b 0.02087 M
c 0.0005 M
d 0.048 M
2.A bottle of 6.00 M NaOH is on the lab bench. You are instructed to use 75.0 mL of 0.500 M NaOH. How much 6.00 M NaOH do you have to dilute to 75.0 mL to meet the requirement?
a The solution cannot be produced from 6 M NaOH.
b 37.5 mL
c 9.0 mL
d 6.25 mL
3.If 25.0 mL of 3.0 M HCl are diluted to give a final volume of 150 mL, what is the new concentration?
a 75 M
b 2.0 M
c 4.5 M
d 0.50 M
1.
It appears the problem states the single dose is 1g per 10 mL.
mols of the stuff = grams/molar mass = ?
Then M = mols/0.010 L = ?
2. Sure is a funny way of stating the problem but it is
mL1 x M1 = mL2 x M2
mL1 x 6 = 75 mL x 0.5
Solve for mL 1.
3.
mL1 x M1 = mL2 x M2
i tried 37.5 for 2 it was wrong.
1 is D!
1. To calculate the molarity of the solution, we need to use the formula:
Molarity (M) = moles of solute / volume of solution in liters
First, let's calculate the moles of sucralfate. The molecular weight of sucralfate is given as 2087 g/mol. The recommended dose is 1g taken orally in 10 mL of solution four times a day.
So, for one dose of 10 mL, the mass of sucralfate is 1g. To convert this to moles, we divide by the molar mass:
moles of sucralfate = 1g / 2087 g/mol = 0.0004792 mol
Since this dose is taken four times a day, the total moles of sucralfate in 40 mL (4 x 10 mL) of solution would be:
total moles of sucralfate = 0.0004792 mol x 4 = 0.001917 mol
Now, we can calculate the volume of the solution in liters. 40 mL is equivalent to 0.040 L.
Now, we can substitute these values into the molarity formula:
Molarity = 0.001917 mol / 0.040 L = 0.0479 M
Rounded to three decimal places, the molarity of the solution is 0.048 M. Therefore, the answer is (d) 0.048 M.
2. To dilute a concentrated solution to a desired concentration, we can use the dilution formula:
C1V1 = C2V2
Where C1 and C2 are the initial and final concentrations, and V1 and V2 are the initial and final volumes respectively.
In this case, we have a 6.00 M NaOH solution and want to dilute it to 0.500 M NaOH with a final volume of 75.0 mL.
Substituting the given values into the dilution formula:
6.00 M x V1 = 0.500 M x 75.0 mL
Now, we can solve for V1:
V1 = (0.500 M x 75.0 mL) / 6.00 M = 6.25 mL
So, to meet the requirement, you need to dilute 6.25 mL of the 6.00 M NaOH solution. The answer is (d) 6.25 mL.
3. To calculate the new concentration after dilution, we can use the dilution formula again:
C1V1 = C2V2
In this case, we have an initial concentration of 3.0 M HCl with a volume of 25.0 mL. After dilution, the final volume is 150 mL.
Substituting the given values into the dilution formula:
3.0 M x 25.0 mL = C2 x 150 mL
Now, we can solve for C2:
C2 = (3.0 M x 25.0 mL) / 150 mL = 0.50 M
The new concentration after dilution is 0.50 M. Therefore, the answer is (d) 0.50 M.