What volume (in mL) OF 0.0215M HBr solution is be required to titrate 0.235L of a 0.0150M Ca(OH)2 solution? Ca(OH)2+2HBr= CaBr2+2H2O
the base is diprotic,
Na*Va=Nb*Vb
.0215Va=2*.0150*.235L
solve for Volume of the acid, Va
nM1V1=nM2V2
n= the moles from the balance equation
HBr Ca(oH)2
2(0.0215)V1=1(0.015)(0.235L)
V1= 0.08192L
To calculate the required volume of 0.0215M HBr solution to titrate 0.235L of 0.0150M Ca(OH)2 solution, we need to determine the stoichiometric ratio between HBr and Ca(OH)2.
From the balanced chemical equation:
Ca(OH)2 + 2HBr → CaBr2 + 2H2O
We can see that the stoichiometric ratio is 1:2, meaning that 1 mole of Ca(OH)2 reacts with 2 moles of HBr.
First, let's calculate the number of moles of Ca(OH)2 in 0.235L of the solution:
Moles of Ca(OH)2 = Molarity × Volume
= 0.0150 mol/L × 0.235 L
= 0.003525 mol
According to the stoichiometry, the number of moles of HBr required will be twice the amount of Ca(OH)2.
Moles of HBr required = 2 × Moles of Ca(OH)2
= 2 × 0.003525 mol
= 0.00705 mol
Now, we can calculate the required volume of the 0.0215M HBr solution using the formula:
Volume = Moles / Molarity
Volume = 0.00705 mol / 0.0215 mol/L
= 0.328 mL
Therefore, approximately 0.328 mL of the 0.0215M HBr solution is required to titrate 0.235L of the 0.0150M Ca(OH)2 solution.
To determine the volume of the 0.0215M HBr solution required to titrate the 0.235L of 0.0150M Ca(OH)2 solution, we need to use the balanced equation:
Ca(OH)2 + 2HBr = CaBr2 + 2H2O
From the equation, we can see that the stoichiometric ratio between Ca(OH)2 and HBr is 1:2. This means that for every 1 mole of Ca(OH)2, we need 2 moles of HBr.
First, let's find the number of moles of Ca(OH)2 in the given 0.235L solution:
Moles of Ca(OH)2 = volume (in liters) × molarity
= 0.235L × 0.0150M
= 0.003525 moles of Ca(OH)2
Since the stoichiometric ratio is 1:2, we require twice the number of moles of HBr to react with Ca(OH)2:
Moles of HBr required = 2 × moles of Ca(OH)2
= 2 × 0.003525 moles of Ca(OH)2
= 0.00705 moles of HBr
Now, we can use the molarity of the HBr solution to find the volume of the solution needed:
Moles of HBr = volume (in liters) × molarity
0.00705 = volume (in liters) × 0.0215M
Solving for the volume, we get:
Volume (in liters) = 0.00705 moles ÷ 0.0215M
Volume (in liters) = 0.3279 L
Finally, we convert the volume from liters to milliliters:
Volume (in mL) = 0.3279 L × 1000 mL/L
Volume (in mL) ≈ 327.9 mL
Therefore, approximately 327.9 mL of the 0.0215M HBr solution is required to titrate 0.235L of the 0.0150M Ca(OH)2 solution.