if 25.00 mL of 1.04 M Na2CO3 is diluted to .500 L, what is the molarity of Na2CO3 in the diluted solution?
(M1)(V1)=(M2)(V2)
convert all moles to grams and mL to L
25mL=0.025L
1.04M (0.025L)=M2 (0.500L)
0.026=M2 (0.5L)
(0.026)/(.5L)=M2
M2=0.052M NaCO3
1.04 M x (25.00 mL/500 mL) = ? M.
To find the molarity of Na2CO3 in the diluted solution, we can use the equation:
M1V1 = M2V2
Where:
M1 = initial molarity of solute
V1 = initial volume of solute
M2 = final molarity of solute
V2 = final volume of solute
Given:
M1 = 1.04 M Na2CO3
V1 = 25.00 mL = 0.025 L (convert mL to L)
M2 = ?
V2 = 0.500 L
Plugging the values into the equation, we have:
(1.04 M)(0.025 L) = M2(0.500 L)
Simplifying, we get:
0.02504 = 0.500 M2
To solve for M2, divide both sides by 0.500:
M2 = 0.02504 / 0.500
M2 = 0.0501 M
Therefore, the molarity of Na2CO3 in the diluted solution is 0.0501 M.
To find the molarity of the Na2CO3 in the diluted solution, you need to use the equation for dilution:
M1V1 = M2V2
Where:
M1 is the initial molarity of the solution (1.04 M Na2CO3 in this case)
V1 is the initial volume of the solution (25.00 mL or 0.025 L in this case)
M2 is the final molarity of the solution (what we want to find)
V2 is the final volume of the solution (0.500 L in this case)
Now, let's plug in the values into the equation:
(1.04 M) x (0.025 L) = M2 x (0.500 L)
0.026 = M2 x 0.500
Next, solve for M2 by dividing both sides of the equation by 0.500:
M2 = 0.026 / 0.500
M2 = 0.052 M
Therefore, the molarity of Na2CO3 in the diluted solution is 0.052 M.