Asked by johnel
Determine how many milliliters of 0.255 M HClO4 will be required to neutralize 48.56 g Ca(OH)2 according to the reaction:
2HClO4(aq)+Ca(OH)2(s)=CA(ClO4)2(aq)+2H2O(l)
2HClO4(aq)+Ca(OH)2(s)=CA(ClO4)2(aq)+2H2O(l)
Answers
Answered by
DrBob222
Here is the corrected equation.
2HClO4(aq)+Ca(OH)2(s)=Ca(ClO4)2(aq)+2H2O(l)
mols Ca(OH)2 = grams/molar mass
Using the coefficients in the balanced equation, convert mols Ca(OH)2 to mols HClO4.
Then M HClO4 = mols HClO4/L HClO4. You know Mols and M, solver for L HClO4 and convert to mL.
2HClO4(aq)+Ca(OH)2(s)=Ca(ClO4)2(aq)+2H2O(l)
mols Ca(OH)2 = grams/molar mass
Using the coefficients in the balanced equation, convert mols Ca(OH)2 to mols HClO4.
Then M HClO4 = mols HClO4/L HClO4. You know Mols and M, solver for L HClO4 and convert to mL.
Answered by
Jeffrey Lee
I love chemistry sm 🧪👨🔬🥼
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