How many milliliters of 0.231 M HBr are needed to titrate each of thefollowing s

Question

How many milliliters of 0.231 MHBr are needed to titrate each of thefollowing solutions to the equivalence point?




(a) 45.6 mL of 0.347 M LiOH

1 mL



(b) 54.7 mL of 0.139 M NaOH

2 mL



(c) 732.0 mL of a solution thatcontains 9.47 g of RbOH per liter

3 mL

Explanation / Answer

(a) LiOH + HBr -> LiBr + H2O n(LiOH) = cv = 0.347 x 0.0456 = 0.01582mol n(HBr) = n(LiOH) = 0.01582mol c(HBr) = n/v 0.231 = 0.01582/v v(HBr) = 0.0685L = 68.5mL (b) NaOH + HBr -> NaBr + H2O n(NaOH) = cv = 0.139 x 0.0547 = 0.0076mol n(HBr) = n(LiOH) = 0.0076mol c(HBr) = n/v 0.231 = 0.0076/v v(HBr) = 0.0329L = 32.9mL (c) RbOH + HBr -> RbBr + H2O n(RbOH) = m/M = 9.47/102.478 = 0.09241mol n(HBr) = n(RbOH) = 0.09241mol c(HBr) = n/v 0.231 = 0.09241/v v(HBr) = 0.4L = 400mL Hope this helps!

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.