A solution consisting of 25.00 g Nh4Cl in 178 ml of water is titrated with 0.114M KOH.
How many mL of KOH are required to reach the equivalence pt?
you need 4100 ml
use M1V1=M2V2
To determine how many mL of KOH are required to reach the equivalence point, we need to first calculate the number of moles of NH4Cl in the solution. Then, we will use stoichiometry to determine the number of moles of KOH needed to react with all the moles of NH4Cl. Finally, we will convert the moles of KOH to mL using the given concentration.
Step 1: Calculate moles of NH4Cl
Moles of NH4Cl = (mass of NH4Cl) / (molar mass of NH4Cl)
Given:
mass of NH4Cl = 25.00 g
molar mass of NH4Cl = 53.49 g/mol
Moles of NH4Cl = 25.00 g / 53.49 g/mol
≈ 0.4676 mol NH4Cl
Step 2: Determine moles of KOH needed
The balanced chemical equation for the reaction between NH4Cl and KOH is:
NH4Cl + KOH -> NH3 + H2O + KCl
From the equation, we can see that 1 mole of NH4Cl reacts with 1 mole of KOH. Therefore, the number of moles of KOH needed is also ≈ 0.4676 mol.
Step 3: Convert moles of KOH to mL
Using the given concentration of KOH, we can determine the volume of KOH needed in mL:
Volume of KOH (in L) = moles of KOH / concentration of KOH
Given:
concentration of KOH = 0.114 M
Volume of KOH (in L) = 0.4676 mol / 0.114 mol/L
≈ 4.095 L
To convert L to mL, multiply by 1000:
Volume of KOH (in mL) = 4.095 L * 1000
≈ 4095 mL
Therefore, approximately 4095 mL of KOH are required to reach the equivalence point.
To determine the number of mL of KOH required to reach the equivalence point, we need to calculate the number of moles of NH4Cl present in the solution and then use stoichiometry to determine the amount of KOH required. Here's how you can do it:
1. Calculate the number of moles of NH4Cl:
- First, convert the mass of NH4Cl to moles. The molar mass of NH4Cl is 53.49 g/mol, so:
Moles of NH4Cl = mass of NH4Cl / molar mass of NH4Cl
Moles of NH4Cl = 25.00 g / 53.49 g/mol
2. Determine the amount of KOH required using stoichiometry:
- The balanced chemical equation for the reaction between NH4Cl and KOH is:
NH4Cl + KOH -> NH3 + H2O + KCl
- According to the equation, 1 mole of NH4Cl reacts with 1 mole of KOH. Therefore, the moles of KOH required are equal to the moles of NH4Cl calculated in step 1.
3. Convert moles of KOH to volume (mL) of KOH:
- The molarity of KOH is given as 0.114M, which represents 0.114 moles of KOH per liter of solution. Therefore, we can use the following equation to calculate the volume of KOH required in mL:
Volume (mL) of KOH = (moles of KOH / molarity of KOH) * 1000
Volume (mL) of KOH = (moles of KOH / 0.114 mol/L) * 1000
Now, you can plug in the value of moles of NH4Cl calculated in step 1 into the equation from step 3 to find the volume of KOH required in mL.