Answer: 0.123 M
Explanation:
According to the neutralization law:
where,
= molarity of
solution = ?
= volume of
solution = 15.00 ml
= molarity of
solution = 0.100 M
= volume of
solution = 18.44 ml
= valency of
= 1
= valency of
= 1
Therefore, the concentration of the unknown HBr solution is 0.123 M
Answer :
The mass of excess mass of ,
are, 1.908 g, 0 g, 12.144 g and 3.74 g respectively.
Explanation : Given,
Mass of = 4.25 g
Mass of = 7.50 g
Molar mass of = 106 g/mole
Molar mass of = 170 g/mole
Molar mass of = 276 g/mole
Molar mass of = 85 g/mole
First we have to calculate the moles of and
.
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 2 moles of react with 1 mole of
So, 0.044 moles of react with
moles of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
The excess mole of = 0.040 - 0.022 = 0.018 mole
Now we have to calculate the mass of excess mole of .
Now we have to calculate the moles of .
As, 1 moles of react to give 1 moles of
So, 0.044 moles of react to give 0.044 moles of
Now we have to calculate the mass of .
Now we have to calculate the moles of .
As, 2 moles of react to give 2 moles of
So, 0.044 moles of react to give 0.044 moles of
Now we have to calculate the mass of .