Question

35.6Ml of an HBr solution were tirated with 18.2 ml of a 0.115M naoh solution to reach equivance point. what is the molarity of the hbr solution

Answer 1

Answer:

0.058 M

Explanation:

HBr reacts with NaOH and forms NaBr and H₂O as the products. The balanced equation is as follows:

$NaOH + HBr \implies NaBr + H_2O$

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

Answer 2

0.0588

This is what I got, and my online school curriculum said it was correct.