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What volume of 0.150 m hclo4 solution is needed to neutralize 60 ml 0f 8.6510-2m naoh?
Wiki User
∙ 12y ago
You MUST get the chemical equation for this question, which is:
HCL + NaOH --> H20 + NaCl
This equation is already balanced. This is a double displacement reaction with neutralization meaning water and a salt will be the products.
M = n/V (molarity = number of moles/ volume
other re-arrangements of this formula:
n = MV
V = n/M
Molarity is always moles per litre, so Its good to change all given volumes to litres then convert back to ml after if you have to.
42.0ml can be converted to litres: 42.0ml = 0.042L
You now have VOLUME and MOLARITY of NaOH, now used n = MV to get number of moles:
0.042 x 0.150 = 0.0063mol NaOH
now you know number of moles, and a BALANCED chemical equation, so you can now do a stoicheometry conversion factor to get the number of moles for HCl.
0.0063mol NaOH x1mol HCL ÷ 1mol NaOH = 0.0063 mol (moles of NaOH cancel out and now you have # of moles for HCl.
at this point you know HCL has Molarity 0.126 and 0.0063mol.
now solve for volume: V = n/M
V = 0.0063/0.126
V = 0.05L
You now know Volume of HCL is 0.05L, now convert it mL because the question is asking for it.
0.05L = 0.05 x 1000
= 50ml
Question complete!
*note* in this chemical equation, the number of moles is the same because the chemical equation is a 1:1 ratio, meaning their are no coefficients in front of an substance. is the HCl or NaOH had coefficients, then the answer would be completly different, thats why you need the stoicheometry mole to mole conversion factor that I added in.
Wiki User
∙ 11y ago
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