(C) The molarity of the final mixture is calculated using the formula: $M_1V_1 + M_2V_2 = M_3V_3$Given:$M_1 = 1.5 \ M, V_1 = 480 \ mL$$M_2 = 1.2 \ M,

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(C) The molarity of the final mixture is calculated using the formula: $M_1V_1 + M_2V_2 = M_3V_3$Given:$M_1 = 1.5 \ M, V_1 = 480 \ mL$$M_2 = 1.2 \ M, V_2 = 520 \ mL$$V_3 = V_1 + V_2 = 480 \ mL + 520 \ mL = 1000 \ mL$Substituting the values:$M_3 = \frac{M_1V_1 + M_2V_2}{V_3}$$M_3 = \frac{(1.5 \times 480) + (1.2 \times 520)}{1000}$$M_3 = \frac{720 + 624}{1000} = \frac{1344}{1000} = 1.344 \ M$Rounding to two decimal places,the molarity is $1.34 \ M$.

Class 12 Chemistry Solutions Method of expressing concentration of solution

Medium

Two solutions of a substance (non-electrolyte) are mixed in the following manner: $480 \ mL$ of $1.5 \ M$ first solution $+ 520 \ mL$ of $1.2 \ M$ second solution. What is the molarity of the final mixture $.......... \ M$.

AIEEE 2005 All AIEEE

A
$1.20$
B
$1.50$
C
$1.34$
D
$2.70$

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Two solutions of a substance (non-electrolyte) are mixed in the following manner: $480 \ mL$ of $1.5 \ M$ first solution $+ 520 \ mL$ of $1.2 \ M$ second solution. What is the molarity of the final mixture $.......... \ M$.

Similar Questions

The molarity of a solution of $Na_2CO_3$ having $10.6 \ g$ in $500 \ mL$ of solution is ......... $M$.

When $7.1 \ g$ of $Na_2SO_4$ (molecular mass $142$) dissolves in $100 \ mL$ of $H_2O$,the molarity of the solution is $.........$ $M$.

If $23 \ g$ of ethanol ($C_2H_5OH$,molar mass $= 46 \ g \ mol^{-1}$) is dissolved in $500 \ mL$ of solution,find the molarity of the solution in $M$.

If $1 \ M$ and $2.5 \ L$ $NaOH$ solution is mixed with another $0.5 \ M$ and $3 \ L$ $NaOH$ solution,then the molarity of the resultant solution will be $........ \ M$.

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