Explain how to prepare a 2.0L solution of each of the following solutions:
a. 0.25 M NaOH from 1.0 M stock NaOH solution
b. 0.100 M K2CrO4 from 1.75 M K2CrO4
a) M1V1 = M2V2 (M = moles of solute / liters of solution; V = volume) M1 = 1.0 M V1 = x M2 = .25 M V2 = 2.0 L
(1.0 M)(x) = (.25 M)(2.0 L) x = .50 L
Fill a graduated cylinder with .50 liters of NaOH stock solution, then pour this into a volumetric flask. Then, fill the volumetric flask with water until the 2.0 L mark.
b) M1V1 = M2V2 (M = moles of solute / liters of solution; V = volume) M1 = 1.75 M V1 = x M2 = .100 M V2 = 2.0 L
(1.75 M)(x) = (.100 M)(2.0 L) x = .114 L
Fill a graduated cylinder with .114 liters of 1.75 M K2CrO4 solution, then pour this into a volumetric flask. Then, fill the volumetric flask with water until the 2.0 L mark.
Molarity= moles of solute/liters of solution Molarity(1)*Volume(1)=Molarity(2)*Volume(2)
a. (1.0 M)*(x)=(.25 M)*(2.0 L) x=.50 Liters NAOH Solution
Pour .50 liters of NAOH solution from your original stock into a graduated cylinder. Then pour that into a volumetric flask (for most accurate measurement), and fill the rest of the flask with H2O (1.5 L) until it reaches 2.0 L.
b. (1.75 M)*(x)=(.100 M)*(2.0 L)*(0.100 M) x=.114 L K2CrO4
Pour .114 liters of K2CrO4 solution from your original stock into a graduated cylinder. Then pour that into a volumetric flask, and fill the rest of the flask with H2O (1.886 L) until it reaches 2.0 L.
a) M1V1=M2V2 (M meaning molarity or moles of solute/liters of solution; and V meaning Volume). This is the general formula used for dilutions from that of a stock solution.) M1=1.0 M (M1 is 1.0, because this is the molarity of the stock solution and the stock solution will be used to dilute the final solution to a lower molarity; in other words this is the initial concentration to be used in order to make the final concentration.) M2=0.25 M (This is the molarity we want to get to as a result of M1) V1=x (This is the volume of the initial solution, or stock solution, which we need to find in order to know how much stock solution we need for the final or diluted solution.) V2=2.0 L (This is the volume of the final or diluted solution.) (1.0 M)(x L)=(0.25 M)(2.0 L) X=0.50 L Therefore 0.50 L of the stock (NaOH) solution must be filled into a graduated cylinder as a reference point, and then must be poured inside a volumetric flask, since it’s the most accurate lab equipment available. Finally, the volumetric flask must be filled with water up to the 2.0 L mark and we have successfully made a 0.25 M NaOH solution with a volume of 2.0 L.
b) M1V1=M2V2 (M meaning molarity or moles of solute/liters of solution; and V meaning Volume). This is the general formula used for dilutions from that of a stock solution.) M1=1.75 M (M1 is 1.75, because this is the molarity of the stock solution and the stock solution will be used to dilute the final solution to a lower molarity; in other words this is the initial concentration to be used in order to make the final concentration.) M2=0.100 M (This is the molarity we want to get to as a result of M1) V1=x (This is the volume of the initial solution, or stock solution, which we need to find in order to know how much stock solution we need for the final or diluted solution.) V2=2.0 L (This is the volume of the final or diluted solution.) (1.75 M)(x L)=(0.100 M)(2.0 L) X=0.114 L Therefore 0.114 L of the stock (K2CrO4) solution must be filled into a graduated cylinder as a reference point, and then must be poured inside a volumetric flask, since it’s the most accurate lab equipment available. Finally, the volumetric flask must be filled with water up to the 2.0 L mark and we have successfully made a 0.100 M K2CrO4 solution with a volume of 2.0 L.
Molarity=moles of solute/liters of solution M1V1=M2V2 a-(1.0M)(V1)=(.25M)(2.0L) V1=0.5L First you fill 0.5L of the stock solution(1.0M NaOH) into a 2L volumetric flask because they are the most accurate glassware. Then add water until you reach the 2.0L mark while mixing the solution. b- (1.75M)(V1)=(.100M)(2.0L) V1=.114L Fill .114L of the stock solution (1.75M K2CrO4) into a 2L volumetric flask. Then add water until it reaches the 2.0L mark.
molarity=moles of solute over the liters of solution. so if M1V1=M2V2 then.. QUESTION A:(1.0M)(V1)=(.25M)(2.0L) and therefore V1=.5L QUESTION B:(1.75M)(V1)=(.100M)(2.0L) therefore V1=.114
Since M1V1=M2V2 and M= moles of solute/ liters of solvent
a) M1= 1.0 M2= 0.25 V1=x V2= 2.0 (1)(x)=(.25)(2) x= .50 L
So, put .50 L of the NaOH stock solution into a volumetric flask (since it is the most accurate) and then add water into the flask until it reaches the 2.0 L mark
b) M1= 1.75 M2= 1.00 V1= x V2= 2
x= .114 L
Now, add .114 L of the K2CrO4 stock solution into a volumetric flask and add water until it reaches the 2.0 L mark
Molarity is moles of solute over the liters of solution.M1V1=M2V2
a-(1.0 M)(V) = (.25 M)(2.0 L) V = .50 L Take the .50 L of NaOH stock solution and pour it into a graduated cylinder. After pour the .50 L NaOH into a 2 L volumetric flask. Next fill the volumetric flask with water.
b-(1.75 M)(V) = (.100 M)(2.0 L) V = .114 L Take the .114L of K2CrO4 stock solution and pour it into a graduated cylinder. After pour the .114 L K2CrO4 into a 2 L volumetric flask. Next fill the volumetric flask with water.
A)Need: 2.0L of .25M NaOH Given: 1.0M solution NaOH (MI)(VI)= (M2)(V2) M1: 1.0M V1: ? M2:.25M V2: 2.0L (1.0M)(V1)=(.25M)(2.0L) V1= .5L V1 is equal to .5L of 1.0M NaOH solution So.. you get a 2L volumetric flask, pour .5L of 1.0M NaOH solution (again, premeasured in graduated cylinder). Stir, then add 1.5L of water and stir. B)Need: 2.0L w/ .100M K2CrO4 Given: 1.75M K2CrO4 M1V1=M2V2 (1.75M)(V1)=(.100M)(2.0L) V1= .11L of 1.75M K2CrO4 First, measure 110 mL of 1.75M K2CrO4 with a graduated cylinder, then pour it into a 2.0L volumetric flask, then add water till the bottom of the miniscus is on the mark.
M1V1=M2V2 (1.0M)(x)=(0.25M)(2.0L) V1=0.5L Take a 2L volumetric flask pour in the solution, add some water and stir but do not fill the flask, since some solutions increase in volume after dissolving, after fully dissolving the solute in water fill the remaining amount with water until the flask holds 2L of solution.
M1V1=M2V2 (1.75M)(x)=(0.100M)(2.00L) x=0.114L=V1 (0.114L)(100)=114mL fill a graduated cylinder with exactly 114 mL of K2CrO4, pour into a 2L volumetric flask then fill with water until about halfway, stir the solution to make sure the K2CrO4 fully dissolves before filling the rest of the flask with water until it measures exactly 2L
Molarity is a concentration measured by the number of moles of solute per liters of solution. To show this we use M=mol/L. To find the molarity of a second solution given a stock you use the equation M1V1=M2V2.
a) M1= 1.0 M V1=? M2=.25 V2=2.0 L M1V1=M2V2 (1.0 M)(V1)=(.25 M)(2.0 L) V1= .50 L so you would put the NaOH solute inside a 2 L volumetric flask, then add a little water, shake it, add a little water, shake it, until the solution reaches the 2 L line. You have to shake the solution and add water little by little because the solute does end up taking some of the volume of the solution and you have to take that into consideration before pouring the whole .50 L of solution
b) M1= 1.75 M V1= ? M2= .100 M V2= 2.0 L (1.75 M)(V1)=(.100 M)(.2 L) V1=.114 you have to do the same process for this solution as well.
M1V1 = M2V2 Molarity is the moles of solute divided by the liters of solution
A) (1.0 M)(x L) = (0.25 M)(2.0 L) x = 0.50 L Fill a graduated cylinder with 0.50 L of the stock solution. Then transfer the solution to a more accurate measuring glass like a volumetric flask, and then fill the flask with some H20, mix, and then fill the rest until it reaches 2.0 L.
B) (1.75 M)(x) = (.100 M)(2.0 L) x = .114 L Fill a graduated cylinder with .114 Liters of 1.75 M K2CrO4 solution, then pour this into a volumetric flask, then fill the flask with water until you reach the 2.0 L mark.
(1.0M)(X)=(0.25M)(2.0L) X= 0.50 L First, obtain a 2.0 L volumetric flask and fill it up with 0.50 L NaOH (stock solution) and add water until the 2.0 L mark of the flask.
B)M1V1=M2V2 M1= 1.75 M V1= X M2= 0.100 M V2= 2.0 L
(1.75M)(X)=(0.100M)(2.0L) X=0.114 L First, obtain a 2.0 L volumetric flask and fill it up with 0.114 L K2CrO4 (stock solution) and add water until the 2.0 L mark of the flask.
a) M1= 1.0 M NaOH Solution M2= 0.25 M NaOH Solution V1= ? V2= 2.0 L (1.0 mol/L NaOH solution)(V1 L)= (0.25 mol/L NaOH Solution)(2.0 L) so V1= 0.5 L Poor 0.5 L of your stock (1.0 M NaOH Solution) in a 2.0 L volumetric flask and then add 1.5 L of H2O to it.
b) M1= 1.75 M K2CrO4 solution M2= 0.100 M K2CrO4 solution V1= ? V2= 2.0 L (1.75 mol/L K2CrO4 solution)(V1 L)= (0.100 mol/L K2CrO4 solution)(2.0 L) V1 ≈ 0.114 L K2CrO4 solution Poor 0.114 L of your stock (1.75 M K2CrO4 solution) into a 2.0 L volumetric flask. Then add about 1.886 L of H2O to it.
A) (1.0 M)(x L) = (0.25 M)(2.0 L) x = 0.50 L B) (1.75 M)(x) = (.100 M)(2.0 L) x = .114 L Just add water to equal 2.0 L(a) and for part b add water to equal again 2.0.
a) M1V1 = M2V2 (M = moles of solute / liters of solution; V = volume)
ReplyDeleteM1 = 1.0 M
V1 = x
M2 = .25 M
V2 = 2.0 L
(1.0 M)(x) = (.25 M)(2.0 L)
x = .50 L
Fill a graduated cylinder with .50 liters of NaOH stock solution, then pour this into a volumetric flask. Then, fill the volumetric flask with water until the 2.0 L mark.
b) M1V1 = M2V2 (M = moles of solute / liters of solution; V = volume)
M1 = 1.75 M
V1 = x
M2 = .100 M
V2 = 2.0 L
(1.75 M)(x) = (.100 M)(2.0 L)
x = .114 L
Fill a graduated cylinder with .114 liters of 1.75 M K2CrO4 solution, then pour this into a volumetric flask. Then, fill the volumetric flask with water until the 2.0 L mark.
Molarity= moles of solute/liters of solution
ReplyDeleteMolarity(1)*Volume(1)=Molarity(2)*Volume(2)
a. (1.0 M)*(x)=(.25 M)*(2.0 L)
x=.50 Liters NAOH Solution
Pour .50 liters of NAOH solution from your original stock into a graduated cylinder. Then pour that into a volumetric flask (for most accurate measurement), and fill the rest of the flask with H2O (1.5 L) until it reaches 2.0 L.
b. (1.75 M)*(x)=(.100 M)*(2.0 L)*(0.100 M)
x=.114 L K2CrO4
Pour .114 liters of K2CrO4 solution from your original stock into a graduated cylinder. Then pour that into a volumetric flask, and fill the rest of the flask with H2O (1.886 L) until it reaches 2.0 L.
a) M1V1=M2V2 (M meaning molarity or moles of solute/liters of solution; and V meaning Volume). This is the general formula used for dilutions from that of a stock solution.)
ReplyDeleteM1=1.0 M (M1 is 1.0, because this is the molarity of the stock solution and the stock solution will be used to dilute the final solution to a lower molarity; in other words this is the initial concentration to be used in order to make the final concentration.)
M2=0.25 M (This is the molarity we want to get to as a result of M1)
V1=x (This is the volume of the initial solution, or stock solution, which we need to find in order to know how much stock solution we need for the final or diluted solution.)
V2=2.0 L (This is the volume of the final or diluted solution.)
(1.0 M)(x L)=(0.25 M)(2.0 L)
X=0.50 L
Therefore 0.50 L of the stock (NaOH) solution must be filled into a graduated cylinder as a reference point, and then must be poured inside a volumetric flask, since it’s the most accurate lab equipment available. Finally, the volumetric flask must be filled with water up to the 2.0 L mark and we have successfully made a 0.25 M NaOH solution with a volume of 2.0 L.
b) M1V1=M2V2 (M meaning molarity or moles of solute/liters of solution; and V meaning Volume). This is the general formula used for dilutions from that of a stock solution.)
M1=1.75 M (M1 is 1.75, because this is the molarity of the stock solution and the stock solution will be used to dilute the final solution to a lower molarity; in other words this is the initial concentration to be used in order to make the final concentration.)
M2=0.100 M (This is the molarity we want to get to as a result of M1)
V1=x (This is the volume of the initial solution, or stock solution, which we need to find in order to know how much stock solution we need for the final or diluted solution.)
V2=2.0 L (This is the volume of the final or diluted solution.)
(1.75 M)(x L)=(0.100 M)(2.0 L)
X=0.114 L
Therefore 0.114 L of the stock (K2CrO4) solution must be filled into a graduated cylinder as a reference point, and then must be poured inside a volumetric flask, since it’s the most accurate lab equipment available. Finally, the volumetric flask must be filled with water up to the 2.0 L mark and we have successfully made a 0.100 M K2CrO4 solution with a volume of 2.0 L.
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ReplyDeleteMolarity=moles of solute/liters of solution
ReplyDeleteM1V1=M2V2
a-(1.0M)(V1)=(.25M)(2.0L)
V1=0.5L
First you fill 0.5L of the stock solution(1.0M NaOH) into a 2L volumetric flask because they are the most accurate glassware. Then add water until you reach the 2.0L mark while mixing the solution.
b- (1.75M)(V1)=(.100M)(2.0L)
V1=.114L
Fill .114L of the stock solution (1.75M K2CrO4) into a 2L volumetric flask. Then add water until it reaches the 2.0L mark.
molarity=moles of solute over the liters of solution.
ReplyDeleteso if M1V1=M2V2 then..
QUESTION A:(1.0M)(V1)=(.25M)(2.0L)
and therefore V1=.5L
QUESTION B:(1.75M)(V1)=(.100M)(2.0L)
therefore V1=.114
Nice job! You found the trick! M1V1=M2V2. Very easy that way. Then you just add water to the specified level.
ReplyDeleteSince M1V1=M2V2 and M= moles of solute/ liters of solvent
ReplyDeletea) M1= 1.0 M2= 0.25
V1=x V2= 2.0
(1)(x)=(.25)(2)
x= .50 L
So, put .50 L of the NaOH stock solution into a volumetric flask (since it is the most accurate) and then add water into the flask until it reaches the 2.0 L mark
b) M1= 1.75 M2= 1.00
V1= x V2= 2
x= .114 L
Now, add .114 L of the K2CrO4 stock solution into a volumetric flask and add water until it reaches the 2.0 L mark
Molarity is moles of solute over the liters of solution.M1V1=M2V2
ReplyDeletea-(1.0 M)(V) = (.25 M)(2.0 L)
V = .50 L
Take the .50 L of NaOH stock solution and pour it into a graduated cylinder. After pour the .50 L NaOH into a 2 L volumetric flask. Next fill the volumetric flask with water.
b-(1.75 M)(V) = (.100 M)(2.0 L)
V = .114 L
Take the .114L of K2CrO4 stock solution and pour it into a graduated cylinder. After pour the .114 L K2CrO4 into a 2 L volumetric flask. Next fill the volumetric flask with water.
A)Need: 2.0L of .25M NaOH
ReplyDeleteGiven: 1.0M solution NaOH
(MI)(VI)= (M2)(V2)
M1: 1.0M
V1: ?
M2:.25M
V2: 2.0L
(1.0M)(V1)=(.25M)(2.0L)
V1= .5L
V1 is equal to .5L of 1.0M NaOH solution
So.. you get a 2L volumetric flask, pour .5L of 1.0M NaOH solution (again, premeasured in graduated cylinder). Stir, then add 1.5L of water and stir.
B)Need: 2.0L w/ .100M K2CrO4
Given: 1.75M K2CrO4
M1V1=M2V2
(1.75M)(V1)=(.100M)(2.0L)
V1= .11L of 1.75M K2CrO4
First, measure 110 mL of 1.75M K2CrO4 with a graduated cylinder, then pour it into a 2.0L volumetric flask, then add water till the bottom of the miniscus is on the mark.
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ReplyDeleteThis comment has been removed by the author.
ReplyDeleteM1V1=M2V2
ReplyDelete(1.0M)(x)=(0.25M)(2.0L)
V1=0.5L
Take a 2L volumetric flask pour in the solution, add some water and stir but do not fill the flask, since some solutions increase in volume after dissolving, after fully dissolving the solute in water fill the remaining amount with water until the flask holds 2L of solution.
M1V1=M2V2
(1.75M)(x)=(0.100M)(2.00L)
x=0.114L=V1
(0.114L)(100)=114mL
fill a graduated cylinder with exactly 114 mL of K2CrO4, pour into a 2L volumetric flask then fill with water until about halfway, stir the solution to make sure the K2CrO4 fully dissolves before filling the rest of the flask with water until it measures exactly 2L
Molarity is a concentration measured by the number of moles of solute per liters of solution. To show this we use M=mol/L. To find the molarity of a second solution given a stock you use the equation M1V1=M2V2.
ReplyDeletea) M1= 1.0 M V1=? M2=.25 V2=2.0 L
M1V1=M2V2
(1.0 M)(V1)=(.25 M)(2.0 L)
V1= .50 L
so you would put the NaOH solute inside a 2 L volumetric flask, then add a little water, shake it, add a little water, shake it, until the solution reaches the 2 L line. You have to shake the solution and add water little by little because the solute does end up taking some of the volume of the solution and you have to take that into consideration before pouring the whole .50 L of solution
b) M1= 1.75 M V1= ? M2= .100 M V2= 2.0 L
(1.75 M)(V1)=(.100 M)(.2 L)
V1=.114
you have to do the same process for this solution as well.
M1V1 = M2V2
ReplyDeleteMolarity is the moles of solute divided by the liters of solution
A) (1.0 M)(x L) = (0.25 M)(2.0 L)
x = 0.50 L
Fill a graduated cylinder with 0.50 L of the stock solution. Then transfer the solution to a more accurate measuring glass like a volumetric flask, and then fill the flask with some H20, mix, and then fill the rest until it reaches 2.0 L.
B) (1.75 M)(x) = (.100 M)(2.0 L)
x = .114 L
Fill a graduated cylinder with .114 Liters of 1.75 M K2CrO4 solution, then pour this into a volumetric flask, then fill the flask with water until you reach the 2.0 L mark.
A)M1V1=M2V2
ReplyDeleteM1= 1.0 M
V1= X
M2= 0.25 M
V2= 2.0 L
(1.0M)(X)=(0.25M)(2.0L)
X= 0.50 L
First, obtain a 2.0 L volumetric flask and fill it up with 0.50 L NaOH (stock solution) and add water until the 2.0 L mark of the flask.
B)M1V1=M2V2
M1= 1.75 M
V1= X
M2= 0.100 M
V2= 2.0 L
(1.75M)(X)=(0.100M)(2.0L)
X=0.114 L
First, obtain a 2.0 L volumetric flask and fill it up with 0.114 L K2CrO4 (stock solution) and add water until the 2.0 L mark of the flask.
a) M1= 1.0 M NaOH Solution
ReplyDeleteM2= 0.25 M NaOH Solution
V1= ?
V2= 2.0 L
(1.0 mol/L NaOH solution)(V1 L)= (0.25 mol/L NaOH Solution)(2.0 L)
so V1= 0.5 L
Poor 0.5 L of your stock (1.0 M NaOH Solution) in a 2.0 L volumetric flask and then add 1.5 L of H2O to it.
b) M1= 1.75 M K2CrO4 solution
M2= 0.100 M K2CrO4 solution
V1= ?
V2= 2.0 L
(1.75 mol/L K2CrO4 solution)(V1 L)= (0.100 mol/L K2CrO4 solution)(2.0 L)
V1 ≈ 0.114 L K2CrO4 solution
Poor 0.114 L of your stock (1.75 M K2CrO4 solution) into a 2.0 L volumetric flask. Then add about 1.886 L of H2O to it.
A) (1.0 M)(x L) = (0.25 M)(2.0 L) x = 0.50 L
ReplyDeleteB) (1.75 M)(x) = (.100 M)(2.0 L) x = .114 L
Just add water to equal 2.0 L(a) and for part b add water to equal again 2.0.