if i use 10mL of 0.5M HCl how much of the NaOH would i need to balance it out?
2007-01-01 11:25:01 · 5 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
I'm assuming by the way you structured your question that balance means titration to equivalence. NaOH is a strong base and HCl is a strong acid, so they dissociate completely. Therefore if you have 10 mL of 0.5M HCl, then 10 mL of 0.5M NaOH would titrate that. You never indicated the molarity of the NaOH you have available so you would have to use the equation m1v1=m2v2=Ve, where (10mL HCl)(0.5M HCl)=(x mL of NaOH)(whatever molarity is your NaOH)
2007-01-01 11:38:12 · answer #1 · answered by Terry N 2 · 0⤊ 0⤋
Well if you write out the balanced equationit would be NaOH + HCl---> NaCl + H20........so as you can see the two substances react in a one to one mole ratio. If you NaOH is also 0.5M you would also need 10ml to react together to compltely neutralize the two so they become a salt and water...(aka a neutralzation reaction)
2007-01-01 11:39:23 · answer #2 · answered by Anonymous · 0⤊ 0⤋
moles of NaOH = moles of HCl = 0.35M x 0.02435L = 8.fifty two x 10^-3 mole Mol. of NaOH x Vol. of NaOH = 0.00852 for this reason 0.00852 = mol.of NaOH x 0.0364L. Mole of NaOH = 0.00852/0.0364 = 0.23 mole
2016-10-19 08:14:20 · answer #3 · answered by ? 4 · 0⤊ 0⤋
Write an equation and balance it. You have to write the equation first and balance both sides.
NaOH + HCl --> NaCl + HOH
Is this balanced? Do all the elements on one side equal those on the other side? Plug and chug the numbers regarding the concentration and the amount that represents in terms of the amount of the other desired.
2007-01-01 11:35:13 · answer #4 · answered by Jack 7 · 0⤊ 0⤋
NaOH + HCl => NaCl + H2O
the moles of HCl 0.5 * 0.01 = 5*10^-3
the moles of NaOH needed : 5*10^-3
2007-01-01 13:05:50 · answer #5 · answered by James Chan 4 · 0⤊ 0⤋