How many millilitres of 0.550 mol L^-1 hydriodic acid are needed to react with 15.00 mL of 0.217 mol L^-1 CsOH?
HI(aq) + CsOH(aq) → CsI(aq) + H₂O(l)

Question

How many millilitres of 0.550 mol L^-1 hydriodic acid are needed to react with 15.00 mL of 0.217 mol L^-1 CsOH? HI(aq)+ CsOH(aq)→ CsI(aq)+ H₂O(l) A)0.0263 mL B)0.169 mL C)5.92 mL D)38.0 mL

Quizplus · Accepted Answer

First, balance the equation: HI(aq) + CsOH(aq) → CsI(aq) + H2O(l) Next, use the mole ratio from the balanced equation to find the moles of L^-1 HI that will react with the given amount of L^-1 CsOH: 0.217 mol CsOH x (1 mol HI / 1 mol CsOH) = 0.217 mol HI Finally, use the concentration and volume of the L^-1 HI solution to find the amount of L^-1 HI that contains 0.217 mol: 0.550 mol/L x V = 0.217 mol V = 0.217 mol / 0.550 mol/L = 0.395 L = 395 mL Therefore, the required amount of L^-1 HI is 5.92 mL.

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