Answer :
Answer: [tex]6.4\times 10^{-7}M[/tex].
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.
[tex]Molarity=\frac{n\times 1000}{V_s}[/tex]
where,
n= moles of solute
[tex]Moles=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{0.6597g}{158g/mol}=0.004mole[/tex]
[tex]V_s[/tex] = volume of solution in ml = 500 ml
[tex]Molarity=\frac{0.004\times 1000}{500}=0.008M[/tex]
According to the dilution law:
[tex]M_1V_1=M_2V_2[/tex]
where,
[tex]M_1[/tex] = molarity of stock solution = 0.008 M
[tex]V_1[/tex] = volume of stock solution = 2 ml
[tex]M_2[/tex] = molarity of resulting solution = ?
[tex]V_2[/tex] = volume of resulting solution = 1000 ml
[tex]0.008\times 2 ml=M_2\times 1000ml[/tex]
[tex]M_2=0.000016M[/tex]
According to the dilution law:
[tex]M_1V_1=M_2V_2[/tex]
where,
[tex]M_1[/tex] = molarity of stock solution = 0.000016 M
[tex]V_1[/tex] = volume of stock solution = 10 ml
[tex]M_2[/tex] = molarity of resulting solution = ?
[tex]V_2[/tex] = volume of resulting solution = 250 ml
[tex]0.000016\times 10 ml=M_2\times 250ml[/tex]
[tex]M_2=0.00000064M=6.4\times 10^{-7}M[/tex]
Scientific notation is defined as the representation of expressing the numbers that are too big or too small and are represented in the decimal form with one digit before the decimal point times 10 raise to the power.
Therefore, the concentration of of the final solution is [tex]6.4\times 10^{-7}M[/tex].
A solution is prepared by dissolving 0.6597 g of KMnO₄ in a 500.0 mL volumetric flask and then is subjected to 2 successive dilutions. The final molarity of the solution is 6.680 × 10⁻⁷ M.
A solution is prepared by dissolving 0.6597 g of KMnO₄ in a 500.0 mL volumetric flask and then is subjected to 2 successive dilutions.
The initial molarity of the solution is:
[tex]M = \frac{mass\ solute }{molar\ mass\ solute \times liters\ solution} = \frac{0.6597g}{158.03g/mol \times 0.5000L } = 8.349 \times 10^{-3} M[/tex]
First dilution
A 2.000−mL (V₁) sample of this solution was transferred to a 1000−mL (V₂) volumetric flask and diluted to the mark with water. We can calculate the final concentration using the dilution rule.
[tex]C_2 = \frac{C_1 \times V_1 }{V_2} = \frac{(8.349 \times 10^{-3}M )\times 2.000mL }{1000mL} = 1.670 \times 10^{-5}M[/tex]
Second dilution
10.00 mL (V₁) of the diluted solution was transferred to a 250.0−mL (V₂) flask and diluted to the mark with water. We can calculate the final concentration using the dilution rule.
[tex]C_2 = \frac{C_1 \times V_1 }{V_2} = \frac{(1.670 \times 10^{-5}M )\times 10.00mL }{250.0mL} = 6.680 \times 10^{-7}M[/tex]
A solution is prepared by dissolving 0.6597 g of KMnO₄ in a 500.0 mL volumetric flask and then is subjected to 2 successive dilutions. The final molarity of the solution is 6.680 × 10⁻⁷ M.
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