Answer: 28 ml
Explanation: [tex]HBr+NaOH\rightarrow NaBr+H_2O[/tex]
At equivalence point the number of [tex]H^+[/tex] ions is equal the number of [tex]OH^-[/tex] ions and thus the acid has been completely neutralized by the base.
[tex]M_1V_1=M_2V_2[/tex]
[tex]M_1[/tex] = molarity of acid
[tex]V_1[/tex] = volume of acid
[tex]M_2[/tex] = molarity of base
[tex]V_2[/tex] = volume of base
[tex]0.140\times 40ml=0.200\times V_2[/tex]
[tex]V_2=28ml[/tex]
Thus 28 ml of 0.200 M NaOH are needed to titrate 40.00 mL of 0.140 M HBr to the equivalence point.
28 ml of 0.200 M [tex]\rm NaOH[/tex] is needed to titrate [tex]\rm HBr[/tex] to the equivalence point.
Titration is the chemical analysis method by which the quantity or the volume of a constituent of substance is estimated by adding it to the sample of known quantity and concentration.
Given,
The volume of the base [tex]\rm NaOH[/tex] can be determined by the formula:
[tex]\rm M_{1}V_{1} = M_{2}V_{2}[/tex]
Substituting values we get:
[tex]\begin{aligned}0.140 \times 40 &= 0.200 \times \rm V_{2}\\\\\rm V_{2} &= \dfrac{0.140 \times 40}{0.200}\\\\\rm V_{2} &= 28\;\rm mL\end{aligned}[/tex]
Therefore, 28 mL of [tex]\rm NaOH[/tex] is required for titrating [tex]\rm HBr[/tex] .
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