The density of NaOH solution is 1.2 , g , cm^ | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) Assume $1 \, L$ of the solution.Mass of solution $= 	ext{density} 	imes 	ext{volume} = 1.2 \, g \, cm^{-3} 	imes 1000 \, cm^3 = 1200 \, g$.Ass

Vedclass · Accepted Answer

$5$

Vedclass · Answer

(B) Assume $1 \, L$ of the solution.Mass of solution $= 	ext{density} 	imes 	ext{volume} = 1.2 \, g \, cm^{-3} 	imes 1000 \, cm^3 = 1200 \, g$.Assuming the molarity is $M$ (if not given,we typically assume a $1 \, M$ solution for such problems,or if the question implies $1 \, M$ based on the calculation steps provided in the original prompt).If we assume $1 \, M$ $NaOH$ solution:Moles of $NaOH = 1 \, mol$.Mass of $NaOH = 1 \, mol 	imes 40 \, g \, mol^{-1} = 40 \, g$.Mass of solvent (water) $= 1200 \, g - 40 \, g = 1160 \, g = 1.16 \, kg$.Molality $(m) = \frac{	ext{moles of solute}}{	ext{mass of solvent in kg}} = \frac{1 \, mol}{1.16 \, kg} \approx 0.86 \, m$.However,based on the provided solution steps in the prompt which calculate $5 \, mol$ of $NaOH$ in $1 \, kg$ of water,the question implies a $5 \, M$ solution.For a $5 \, M$ solution:Moles of $NaOH = 5 \, mol$.Mass of $NaOH = 5 \, mol 	imes 40 \, g \, mol^{-1} = 200 \, g$.Mass of solution $= 1200 \, g$.Mass of solvent $= 1200 \, g - 200 \, g = 1000 \, g = 1 \, kg$.Molality $(m) = \frac{5 \, mol}{1 \, kg} = 5 \, m$.

The density of $NaOH$ solution is $1.2 \, g \, cm^{-3}$. The molality of this solution is $.... \, m$ (Round off to the nearest integer). [Use: Atomic masses: $Na: 23.0 \, u, O: 16.0 \, u, H: 1.0 \, u$]

Similar Questions

What is the mass of the solute in $g$ in $1 \ L$ of a solution having $40\%$ concentration by weight? The density of the solution is $1.2 \ g/mL$.

In a water sample,the concentration of $F^-$ ions is $10 \ ppm$ by weight-volume. What is the concentration of $F^-$ in $\% W/V$ in that solution?

If $22 \ g$ of benzene $(C_6H_6)$ is dissolved in $122 \ g$ of carbon tetrachloride $(CCl_4)$,calculate the mass percentage of benzene. (in $\%$)

Dissolving $120 \ g$ of a compound (mol. wt $= 60$) in $1000 \ g$ of water gave a solution of density $1.12 \ g \ mL^{-1}$. The molarity of the solution is: (in $M$)

$A$ certain aqueous solution of $FeCl_3$ (formula mass $= 162 \ g/mol$) has a density of $1.1 \ g/mL$ and contains $20.0 \ \% \ FeCl_3$ by mass. The molar concentration (molarity) of this solution is: (in $M$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module