A flask containing 5.00mL of 3 M HCl solution requires 14.45mL of 1.00 M NaOH for titration. How many moles of HCl are present in the solution? The density of 3 M HCl is 1.05g/mL
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To find the number of moles of HCl present in the solution, we need to use the molarity and volume of the NaOH solution used for titration.
The balanced chemical equation for the reaction between HCl and NaOH is:
HCl + NaOH -> NaCl + H2O
From the balanced equation, we can see that HCl and NaOH react in a 1:1 ratio. This means that for every 1 mole of NaOH, we have 1 mole of HCl.
First, let's find the number of moles of NaOH used for titration:
Moles of NaOH = Molarity of NaOH x Volume of NaOH (in liters)
= 1.00 M x 0.01445 L
= 0.01445 moles
Since the reaction is 1:1, the number of moles of NaOH used is equal to the number of moles of HCl present in the solution.
Now, let's find the mass of HCl present in the solution:
Mass of HCl = Volume of HCl x Density of HCl
= 5.00 mL x 1.05 g/mL
= 5.25 g
Next, we can calculate the number of moles of HCl:
Moles of HCl = Mass of HCl / Molar Mass of HCl
The molar mass of HCl is calculated using the atomic masses of hydrogen (H) and chlorine (Cl), which are 1.008 g/mol and 35.453 g/mol, respectively.
Molar mass of HCl = 1.008 g/mol + 35.453 g/mol
= 36.461 g/mol
Moles of HCl = 5.25 g / 36.461 g/mol
= 0.144 moles
Therefore, the flask contains 0.144 moles of HCl.