Answer:
0.0588
Explanation:
HBr + NaOH ==> NaBr + H2O
(35.6 ml)(x M) = (18.2 ml)(0.115 M)
x = 0.0588 M
The Molarity of the HBr solution is 0.058 M
Molarity of a given solution is defined as the total number of moles of solute per litre of solution.
HBr reacts with NaOH and forms NaBr and H₂O as the products.
The balanced equation is as follows :
NaOH + HBr --> NaBr + H₂O
Molarity (M) = moles of solute (mol) / volume of the solution (L)
Molarity of NaOH = 0.115 M
Volume of NaOH = 18.2 mL = 18.2 x 10⁻³ L
So, moles of NaOH = molarity x volume of the solution
= 0.115 M x 18.2 x 10⁻³ L
= 2.093 x 10⁻³ mol
From the equation,
we can see that the ratio between NaOH and HBr is 1 : 1.
Therefore,
Moles of HBr in 35.6 mL = Moles of NaOH added = 2.093 x 10⁻³ mol
Hence,
Molarity of HBr = 2.093 x 10⁻³ mol / 35.6 x 10⁻³ L = 0.058 M
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