Ask Questions, Get Answers

Want to ask us a question? Click here
Browse Questions
Home  >>  JEEMAIN and AIPMT  >>  Chemistry  >>  Solutions
0 votes

Calculate the amount of ammonium sulphate required to prepare 500ml of 1 molar solution of ammonium sulphate? (m.wt of $(NH_4)_2SO_4$ is 132.14gm/mol)

$\begin{array}{1 1}(a)\;66gm\\(b)\;132gm\\(c)\;198gm\\(d)\;212gm\end{array}$

Can you answer this question?

1 Answer

0 votes
Answer: 66 g
Given Molarity of Ammonium Sulphate solution $ = 1$, Volume of solution is $500\;mL$ and the Molecular Weight $ = 132.14 \; g\;mol^{-1}$
Molarity (M) is defined as number of moles of solute dissolved in one litre (or one cubic decimetre) of solution, $M = \large\frac{\text{ Moles of solute }}{\text{Molarity Volume of solution in litre}}$
$\Rightarrow $ Molues of solute $= 1M \times 0.5\;L = 0.5\; mol$
$\Rightarrow 0.5\; mol = \large\frac{\text{Amount of Ammonium Sulphate}}{\text{Molar Mass of Ammonium Sulphate}}$
$\Rightarrow$ Amount of Ammonium Sulphate $= 0.5\;mol \times 131.14\; g\;mol^{-1} = 66\;g$
answered Feb 12, 2014 by sreemathi.v
edited Jul 16, 2014 by balaji.thirumalai

Related questions

Ask Question
student study plans
JEE MAIN, CBSE, NEET Mobile and Tablet App
The ultimate mobile app to help you crack your examinations
Get the Android App