Browse by Stream
QnA
Home
QnA
Go To Your Study Dashboard

Get Answers to all your Questions

header-bg qa
  • Home
  • Medical
  • A solution is prepared by dissolving 2 g of   in 100 g of water. What is the molarity of the solution? (Given:<img

A solution is prepared by dissolving 2 g of NaOH  in 100 g of water. What is the molarity of the solution? (Given:\text { Molar mass of } \mathrm{NaOH}=40 \mathrm{~g} / \mathrm{mol} \text {. })

Option: 1

0.5 M


Option: 2

1 M


Option: 3

2 M


Option: 4

4 M


Answers (1)

best_answer

To calculate the molarity of the solution, we need to first calculate the number of moles of NaOH present in the solution.

\begin{aligned} & \text { Number of moles of } \mathrm{NaOH}=\text { Mass of } \mathrm{NaOH} / \text { Molar mass of } \mathrm{NaOH} \\ & =2 \mathrm{~g} / 40 \mathrm{~g} / \mathrm{mol} \\ & =0.05 \mathrm{~mol} \end{aligned}

Now, we need to calculate the volume of the solution in liters.

\begin{aligned} & \text { Volume of the solution }=\text { Mass of solvent } / \text { Density of solvent } \\ & =100 \mathrm{~g} / 1 \mathrm{~g} / \mathrm{mL} \\ & =100 \mathrm{~mL} \\ & =0.1 \mathrm{~L} \end{aligned}

Therefore, the molarity of the solution can be calculated as:

\begin{aligned} & \text { Molarity }=\text { Number of moles of solute/Volume of solution in liter } \\ & =0.05 \mathrm{~mol} / 0.1 \mathrm{~L} \\ & =0.5 \mathrm{M} \end{aligned}

Hence, the correct answer is option a) 0.5 M.

Posted by

Anam Khan

View full answer

NEET 2024 Most scoring concepts

    Just Study 32% of the NEET syllabus and Score up to 100% marks

Similar Questions

Trending Articles/News

anam-khan

NEET UG 2025: NTA's 5 new rules, changes for medical entrance exam
anam-khan

NEET UG 2025: New tie-breaking rule, independent expert panel to resolve through ‘random process’
anam-khan

NEET Registration 2025 Live: NTA NEET UG application form out at neet.nta.nic.in; exam schedule

Latest Question