(A) Using the dilution formula $C_1V_1 = C_2V_2$: Given $C_1 = 40 \, mg/mL$,$C_2 = 16 \, mg/mL$,and $V_1 = 1 \, mL$. $40 \, mg/mL \times 1 \, mL = 16

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Each $mL$ must be diluted to $2.5 \, mL$

(A) Using the dilution formula $C_1V_1 = C_2V_2$: Given $C_1 = 40 \, mg/mL$,$C_2 = 16 \, mg/mL$,and $V_1 = 1 \, mL$. $40 \, mg/mL \times 1 \, mL = 16 \, mg/mL \times V_2$ $V_2 = \frac{40}{16} = 2.5 \, mL$. Therefore,each $1 \, mL$ of the original solution must be diluted to a total volume of $2.5 \, mL$.

Class 12 Chemistry Solutions Method of expressing concentration of solution

Medium

To what extent must a given solution of concentration of $40 \, mg$ silver nitrate per $mL$ be diluted to yield a solution of concentration of $16 \, mg$ $AgNO_3$ per $mL$?

A
Each $mL$ must be diluted to $2.5 \, mL$
B
To each $mL$ of solution $2.5 \, mL$ of water should be added
C
To $2.5 \, mL$ of solution $2 \, mL$ of water should be added
D
To $1.5 \, mL$ of solution $1.5 \, mL$ of water should be added

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Method of expressing concentration of solution

Which concentrations can be calculated if the mole fraction and density of an aqueous solution of $HCl$ are known? $1.$ Molality $2.$ Molarity $3.$ Percentage by mass

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Calculate the molarity of $NaOH$ in the solution prepared by dissolving $4 \,g$ of it in enough water to form $250 \,mL$ of the solution. (in $,M$)

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The mole fraction of a solute in a solution is $0.1$. At $298 \ K$,molarity of the solution is the same as its molality. The density of this solution at $298 \ K$ is $2.0 \ g \ cm^{-3}$. The ratio of the molecular weights of the solute and solvent,$\left(\frac{MW_{solute}}{MW_{solvent}}\right)$,is

MediumIIT 2016

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The molality of a solution,when $18 \ g$ of glucose is added to $18 \ g$ of $H_2O$,is: (in $m$)

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The molality of $648 \ g$ of pure water is ........... $m$.

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To what extent must a given solution of concentration of $40 \, mg$ silver nitrate per $mL$ be diluted to yield a solution of concentration of $16 \, mg$ $AgNO_3$ per $mL$?

Similar Questions

Which concentrations can be calculated if the mole fraction and density of an aqueous solution of $HCl$ are known? $1.$ Molality $2.$ Molarity $3.$ Percentage by mass

Calculate the molarity of $NaOH$ in the solution prepared by dissolving $4 \,g$ of it in enough water to form $250 \,mL$ of the solution. (in $,M$)

The mole fraction of a solute in a solution is $0.1$. At $298 \ K$,molarity of the solution is the same as its molality. The density of this solution at $298 \ K$ is $2.0 \ g \ cm^{-3}$. The ratio of the molecular weights of the solute and solvent,$\left(\frac{MW_{solute}}{MW_{solvent}}\right)$,is

The molality of a solution,when $18 \ g$ of glucose is added to $18 \ g$ of $H_2O$,is: (in $m$)

The molality of $648 \ g$ of pure water is ........... $m$.

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