How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH?
HI(aq) + CsOH(aq) → CsI(aq) + H₂O(l)

Question

How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq)+ CsOH(aq)→ CsI(aq)+ H₂O(l) A)0)0158 mL B)0)101 mL C)9)86 mL D)63.4 mL

Quizplus · Accepted Answer

First, we need to write and balance the chemical equation:
HI + CsOH → CsI + H2O
Next, we can use the balanced equation to set up a mole-to-mole ratio:
1 mol HI : 1 mol CsOH
From the given concentration of CsOH and volume, we can calculate the number of moles of CsOH:
0.217 mol/L x 0.02500 L = 0.00543 mol CsOH
Since the mole ratio is 1:1, we need the same number of moles of HI:
0.00543 mol HI
Finally, we can use the concentration of HI to calculate the required volume:
0.00543 mol HI / 0.550 mol/L = 0.00993 L
0.00993 L x 1000 mL/L = 9.86 mL, which is approximately equal to 9.9 mL.
Therefore, the answer is C) 9.86 mL.

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