the volume of nh3 at stp needed to pass into 30 ml of in h2so4 solution to bring down its strength to m/10
To find the volume of NH3 needed to bring the H2SO4 solution to a specific strength, we need to determine the stoichiometry of the reaction between NH3 and H2SO4.
The balanced chemical equation for the reaction between ammonia (NH3) and sulfuric acid (H2SO4) is as follows:
2 NH3 + H2SO4 -> (NH4)2SO4
From the equation, we can see that 2 moles of NH3 react with 1 mole of H2SO4 to produce 1 mole of (NH4)2SO4.
To calculate the volume of NH3 required, we need to know the molarity (M) or concentration of the H2SO4 solution and the desired final concentration.
Let's assume the initial concentration of the H2SO4 solution is C1 M (molarity) and we want to dilute it to C2 M (molarity).
First, we need to determine the number of moles of H2SO4 in the initial solution:
Moles of H2SO4 (initial) = C1 x Volume (in liters)
Next, we can calculate the number of moles of (NH4)2SO4 needed to achieve the desired concentration:
Moles of (NH4)2SO4 = Moles of H2SO4 (initial)
Since 2 moles of NH3 react with 1 mole of H2SO4, the number of moles of NH3 required will be half the number of moles of (NH4)2SO4:
Moles of NH3 = 0.5 x Moles of (NH4)2SO4
Finally, we can calculate the required volume of NH3 using its molarity:
Volume of NH3 (in liters) = Moles of NH3 / Molarity (NH3)
Now, let's plug in the given values:
Initial volume of H2SO4 solution = 30 ml = 0.03 L (converted to liters)
Desired final concentration of H2SO4 = m/10
(Multiply the desired final concentration by 0.001 to convert from molar (M) to molarity (mol/L))
Using the provided information, substitute the values into the equations to calculate the volume of NH3:
Moles of H2SO4 (initial) = C1 x Volume (in liters)
Moles of (NH4)2SO4 = Moles of H2SO4 (initial)
Moles of NH3 = 0.5 x Moles of (NH4)2SO4
Volume of NH3 (in liters) = Moles of NH3 / Molarity (NH3)
By following these steps, you should be able to calculate the volume of NH3 required to bring down the strength of the H2SO4 solution to m/10.