Question

I need help with Chemistry

Answer 1

Determine how many milliliters of 0.626 M HClO4 will be required to neutralize 57.90 g Ca(OH)2 according to the reaction

2 HClO4(aq) +Ca(OH)2(S) =Ca(ClO4)2(aq) + 2 H2O(l)

Answer 2

57.90 g = 1 mol / 74.904 = 2 mol / 1 mol, right? :/

Answer 3

HCLO4 106 g/mol
CaOH2 74.1 g/mol

You need to find out how many moles you need. let's look at

57.9g x (1 mol CaOH2/74.1g) = 0.78 mol of CaOH2 This is how many moles you have

but you need to find out how many moles of something will react completely with this so
you find the # of moles of HCLO4 by multiplying by the molar ratio.

0.78mol CaOH2 x (2mol HClO4/1 CaOH2) = 1.56 mol. HClO4.

so 0.78 mol of CaOH2 is needed to react with 1.56 mol of HCLO4.

Answer 4

found a useful site that might help out http://www.chemteam.info/AcidBase/Titration-calc-amount-solid2.html

according to what was done there:
to find the original volume in a neutralization problem you need to do:

(x) = volume

mol/L (x) = moles

moles/(mol/L) gives you Liters required.

we have 0.626 mol/L of HClO4 and we needed 1.56 mol of that to complete the reaction.

so it's (1.56mol)/(0.626moL/L) = 2.50 L needed.