What is the concentration of an HBr solution if 29.0 mL of a 0.200 M NaOH solution are needed to titrate 54.0 mL of the acid?

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31-03-2018
Chemistry

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What is the concentration of an HBr solution if 29.0 mL of a 0.200 M NaOH solution are needed to titrate 54.0 mL of the acid?

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mixter17 mixter17 · Answer 1 · 2018-04-09T05:10:33+02:00

Hello!

The concentration of the HBr solution is 0,107M

The chemical reaction between HBr and NaOH is the following:

HBr + NaOH → NaBr + H₂O

To calculate the concentration of the HBr solution, we'll need to apply the following equation (molar equivalence) and clear for the concentration of HBr:

[tex][HBr]*V_{HBr}=[NaOH]*V_{NaOH}[/tex]

[tex][HBr]= \frac{[NaOH]*V_{NaOH}}{V HBr}= \frac{0,2 M*29,0 mL}{54,0 mL}=0,107 M [/tex]

Have a nice day!

mahima6824soni mahima6824soni · Answer 2 · 2022-03-10T13:43:29+01:00

The concentration (molarity) of an HBr solution is 0.0107 m.

What is molarity?

Molarity is the measure of the concentration of any solute in per unit volume of the solution.

The chemical reaction is

[tex]\rm HBr + NaOH = NaBr + H_2O[/tex]

We will calculate the concentration by formula of molar equivalence

[tex][HBr] \times V_H_B_r = NaOH \times V_N_a_O_H\\\\\\HBr = \dfrac{NaOH \times V_N_a_O_H}{V_H_B_r} \\\\\\HBr = \dfrac{0.2\;m\times 29.0\;ml}{54.0\;ml} = 0.0107\;m[/tex]

Thus, the concentration is 0.0107 m

Learn more about molarity, here:

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