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Q8. The titration of 15.00 mL of HBr solution of unknown concentration requires 18.44 mL of a 0.100 M KOH solution to reach the equivalence point. What is the concentration of the unknown HBr solution in M? Tro, Nivaldo J.. Chemistry (p. 201). Pearson Education. Kindle Edition.

Respuesta :

Answer: 0.123 M

Explanation:

According to the neutralization law:

[tex]n_1M_1V_1=n_2M_2V_2[/tex]

where,

[tex]M_1[/tex] = molarity of [tex]HBr[/tex] solution = ?

[tex]V_1[/tex] = volume of [tex]HBr[/tex] solution = 15.00 ml

[tex]M_2[/tex] = molarity of [tex]KOH[/tex] solution = 0.100 M

[tex]V_2[/tex] = volume of [tex]KOH[/tex] solution = 18.44 ml

[tex]n_1[/tex] = valency of [tex]HBr[/tex] = 1

[tex]n_2[/tex] = valency of [tex]KOH[/tex] = 1

[tex]1\times M_1\times 15.00=1\times 0.100\times 18.44[/tex]

[tex]M_1=0.123[/tex]

Therefore, the concentration of the unknown HBr solution is 0.123 M