Respuesta :
Answer: The molarity of KOH solution is 0.093 M
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.
[tex]Molarity=\frac{n\times 1000}{V_s}[/tex]
where,
n = moles of solute
[tex]V_s[/tex] = volume of solution in ml
moles of [tex]HSO_3NH_2[/tex] = [tex]\frac{\text {given mass}}{\text {Molar mass}}=\frac{0.179g}{97.1g/mol}=0.0018mol[/tex]
Now the balanced chemical equation will be :
[tex]HSO_3NH_2+KOH\rightarrow KSO_3NH_2+H_2O[/tex]
As 1 mole of [tex]HSO_3NH_2[/tex] requires 1 mole of KOH
Thus 0.0018 moles of [tex]HSO_3NH_2[/tex] requires =[tex]\frac{1}{1}\times 0.0018=0.0018[/tex] moles of KOH
Now put all the given values in the formula of molality, we get
[tex]Molarity=\frac{0.0018\times 1000}{19.4ml}[/tex]
[tex]Molarity=0.093M[/tex]
Therefore, the molarity of KOH solution is 0.093 M
The molarity of the KOH solution is 0.093 M
We'll begin by calculating the number of mole of HSO₃NH₂.
- Mass of HSO₃NH₂ = 0.179 g
- Molar mass of HSO₃NH₂ = 97.1 g/mol
- Mole of HSO₃NH₂ =?
Mole = mass / molar mass
Mole of HSO₃NH₂ = 0.179 / 97.1
Mole of HSO₃NH₂ = 0.0018 mole
Next, we shall determine the number of mole of KOH required to react with 0.0018 mole of HSO₃NH₂.
HSO₃NH₂ + KOH —> KSO₃NH₂ + H₂O
From the balanced equation,
1 mole of HSO₃NH₂ reacted with 1 mole of KOH.
Therefore,
0.0018 mole of HSO₃NH₂ will also react with 0.0018 mole of KOH.
Finally, we shall determine the molarity of the KOH solution.
- Mole of KOH = 0.0018 mole
- Volume = 19.4 mL = 19.4 / 1000 = 0.0194 L
- Molarity of KOH =?
Molarity = mole / Volume
Molarity of KOH = 0.0018 / 0.0194
Molarity of KOH = 0.093 M
Thus, the molarity of the KOH solution is 0.093 M.
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