Muriatic acid is the common name of industrial-grade hydrochloric acid (HCl). One of its uses is to clean or etch concrete in preparation for sealing or painting. It is typically sold in 5.00 gallon buckets, with a concentration of 11.7 M.

a.What volume of concentrated muriatic acid is needed to prepare 10.00 L of a 2.5 M solution?
b.If the entire 5.00 gallon bucket were diluted with enough water to make 100.00 gallons of solution, what would be the concentration of the diluted solution? NOTE: 1 gal = 3.7854 L

A compound Contains 14.5g of magnesium and 3.5 g of oxygen. what the mass of oxygen in the compound ?

a. How many mols do you need? That's M x L = mols

Then M = mols/L. You have M and mols, solve for L. You may want to convert L to mL.

b. 5.00 gallons x 3.7854 L/gallon = 18.93 L.
100 gallons x 3.7854 L/gallon = 378.54 L.
Then c1v1 = c2v2
11.7 x 18.93 = c2*378.54
Solve for c2.
I should point out to you that there is no need to convert gallons to L.
If you use
11.7 x 5 gallons = c2*100 gallons you will get the same answer.

I may be missing something but the problem tells you there are 3.5 g oxygen in the compound.

How much energy is required to change the temperature of 210g of h2o from -40oC to 155oC?

You should not post piggy back on another post. Most of the times it doesn't get answered. Go to the top of the page and make a new post.

To answer the first question, we need to calculate the volume of concentrated muriatic acid required to prepare a 2.5 M solution.

To do this, we can use the dilution formula:

M1V1 = M2V2

Where:

M1 = initial concentration of the acid (11.7 M)
V1 = volume of concentrated acid to be used (unknown)
M2 = final concentration of the solution (2.5 M)
V2 = final volume of the solution (10.00 L)

Rearranging the formula to solve for V1, we have:

V1 = (M2 * V2) / M1

Substituting the given values, we get:

V1 = (2.5 M * 10.00 L) / 11.7 M
V1 = 21.37 L

Therefore, you would need to use approximately 21.37 L of concentrated muriatic acid to prepare 10.00 L of a 2.5 M solution.

To answer the second question, we need to calculate the concentration of the diluted solution when the entire 5.00-gallon bucket is diluted with enough water to make 100.00 gallons of solution.

First, we need to convert the volume from gallons to liters using the conversion factor given (1 gal = 3.7854 L):

Volume of the concentrated acid in liters = 5.00 gal * 3.7854 L/gal = 18.927 L

Volume of the diluted solution in liters = 100.00 gal * 3.7854 L/gal = 378.54 L

Using the dilution formula again, we can find the concentration of the diluted solution:

M1V1 = M2V2

Where:

M1 = initial concentration of the acid (11.7 M)
V1 = volume of concentrated acid used (18.927 L)
M2 = final concentration of the solution (unknown)
V2 = final volume of the solution (378.54 L)

Rearranging the formula to solve for M2, we have:

M2 = (M1 * V1) / V2

Substituting the values, we get:

M2 = (11.7 M * 18.927 L) / 378.54 L
M2 = 0.585 M

Therefore, the concentration of the diluted solution would be approximately 0.585 M when the entire 5.00-gallon bucket is diluted with enough water to make 100.00 gallons of solution.