In the standardization of using by iodometry, the equivalent weight of is :
$\begin{array}{*{20}{l}}
{\left( {molecular{\rm{ }}weight} \right)/2}
\end{array}$
$\begin{array}{*{20}{l}}
{\left( {molecular{\rm{ }}weight} \right)/6}
\end{array}$
$\begin{array}{*{20}{l}}
{\left( {molecular{\rm{ }}weight} \right)/3}
\end{array}$
Same as molecular weight
Related Questions
A 1 molal aqueous solution contains 0.5 moles of solute. What is the mass of the solvent (water) in kilograms?
0.5 kg
1 kg
2 kg
1.5 kg
100 mL of 0.1 M solution of a reductant is diluted to 1 litre, which of the following changes?
Molarity
Millimole
Milliequivalent
None of these
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0.25 moles
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1 mole
2 moles
If 1 kg of solvent contains 2 moles of solute, what is the molality of the solution?
1 molal
2 molal
0.5 molal
4 molal
A solution is prepared by dissolving 0.25 moles of glucose in 500g of water. What is the molality of the glucose solution?
0.25 molal
0.5 molal
1 molal
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Which of the following describes a 0.5 molal solution?
0.5 moles of solute in 1 kg of solvent
1 mole of solute in 0.5 kg of solvent
0.5 moles of solute in 0.5 kg of solvent
1 mole of solute in 1 kg of solvent
100 mL of 0.1 M solution of a reductant is diluted to 1 litre, which of the following changes?
Molarity
Millimole
Milliequivalent
None of these
