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Question 150851: Sulfuric acid (H2SO4) can be used to remove water from organic materials leaving behind a residue of black carbon. If beaker A contains a 15% solution of sulfuric acid and beaker B contains a 20% solution of sulfuric acid, how much from each beaker should be used to make 6 liters of a 18% solution of sulfuric acid?
: Sulfuric acid (H2SO4) can be used to remove water from organic materials leaving behind a residue of black carbon. If beaker A contains a 15% solution of sulfuric acid and beaker B contains a 20% solution of sulfuric acid, how much from each beaker should be used to make 6 liters of a 18% solution of sulfuric acid?

Answer by Fombitz(1270) About Me  (Show Source):
You can put this solution on YOUR website!
Let's call the amount from beaker A, A.
Let's call the amount from beaker B, B.
The total final volume is 6 liters.
1.A+B=6
The final concentration is 18%.
2.A(0.15)+B(0.20)=(A+B)(0.18)
Let's multiply equation 2 by 100 to get rid of decimals.
2.15A+20B=18(A+B)
2.15A+20B=18A+18B)
2.3A-2B=0
We can use eq. 2 to solve for B in terms of A.
2.3A-2B=0
2B=3A
B=(3/2)A
Now substitute this into eq. 1 and solve for A.
1.A+B=6
A+(3/2)A=6
(5/2)A=6
A=12/5
Now back substitute to find B,
B=(3/2)A
B=(3/2)(12/5)
B=18/5
2.4 liters of solution A and 3.6 liters of solution B.
Question 150851: Sulfuric acid (H2SO4) can be used to remove water from organic materials leaving behind a residue of black carbon. If beaker A contains a 15% solution of sulfuric acid and beaker B contains a 20% solution of sulfuric acid, how much from each beaker should be used to make 6 liters of a 18% solution of sulfuric acid?
: Sulfuric acid (H2SO4) can be used to remove water from organic materials leaving behind a residue of black carbon. If beaker A contains a 15% solution of sulfuric acid and beaker B contains a 20% solution of sulfuric acid, how much from each beaker should be used to make 6 liters of a 18% solution of sulfuric acid?

Answer by josmiceli(1851) About Me  (Show Source):
You can put this solution on YOUR website!
In words:
(liters of acid in beaker A) + (liters of acid in beaker B) / (total liters of solution in A and B) = % solution of acid
Let A = liters of solution needed from beaker A
Let B = liters of solution needed from beaker B
(.15A + .2B) / (A + B) = .18
Note that we are told A + B = 6liters
(.15A + .2B) / 6 = .18
Multiply both sides by 6
.15A + .2B = 1.08
And since A + B = 6
B = 6 - A
.15A + .2*(6 - A) = 1.08
.15A + 1.2 - .2A = 1.08
-.05A = -.12
A = 2.4liters
Given is A + B = 6
B = 6 - 2.4
B = 3.6
2.4 liters of solution are needed from beaker A
and 3.6 liters of solution are needed from beaker B
check answer:
(.15A + .2B) / 6 = .18
(.15*2.4 + .2*3.6) / 6 = .18
(.36 + .72) / 6 = .18
1.08 / 6 = .18
1.08 = .18*6
1.08 = 1.08
OK
Question 150851: Sulfuric acid (H2SO4) can be used to remove water from organic materials leaving behind a residue of black carbon. If beaker A contains a 15% solution of sulfuric acid and beaker B contains a 20% solution of sulfuric acid, how much from each beaker should be used to make 6 liters of a 18% solution of sulfuric acid?
: Sulfuric acid (H2SO4) can be used to remove water from organic materials leaving behind a residue of black carbon. If beaker A contains a 15% solution of sulfuric acid and beaker B contains a 20% solution of sulfuric acid, how much from each beaker should be used to make 6 liters of a 18% solution of sulfuric acid?

Answer by stanbon(18017) About Me  (Show Source):
You can put this solution on YOUR website!
If beaker A contains a 15% solution of sulfuric acid and beaker B contains a 20% solution of sulfuric acid, how much from each beaker should be used to make 6 liters of a 18% solution of sulfuric acid?
----------------------
EQUATIONS:
Quantity Equation: a + b = 6 L
Active Ingrediant: 0.15a + 0.20b = 0.18(6) = 1.08
----------------
Rearrange for elimination:
15a + 15b = 90
15a + 20b = 108
------------------
Subtract 1st from 2nd to get:
5b = 18
b = 3.6 L (amt. of 15% solution in the mix)
Since a+b=6, a = 6-3.6 = 2.4 L (amt. of 20% solution in the mix)
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Cheers,
Stan H.