How many milliliters of 0.550 M hydriodic acid are needed to react with 5.00 mL of 0.217 M CsOH? HI(aq)+ CsOH(aq)→ CsI(aq)+ H₂O(l) A)0.0789 mL B)0.507 mL C)1.97 mL D)12.6 mL

Question

Quizplus · Accepted Answer

Step 1: Write a balanced chemical equation for the reaction.

HI(aq) + CsOH(aq) → CsI(aq) + H2O(l)

Step 2: Determine the limiting reagent.

Use stoichiometry to determine the amount of HI needed to react with the CsOH.

0.217 M CsOH × 5.00 mL = 0.00109 moles CsOH

0.00109 moles CsOH × 1 mole HI ÷ 1 mole CsOH = 0.00109 moles HI needed

Use the molarity of the HI solution to determine the volume needed.

0.00109 moles HI ÷ 0.550 M HI = 0.00199 L HI

Convert the volume to milliliters.

0.00199 L × (1000 mL/1 L) = 1.97 mL HI

Therefore, the best choice is C (1.97 mL).

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