Question

What volume of 0.115 M HClO4 solution is needed to neutralize 48.00mL of 8.90×10−2 M NaOH? just need help geting started no answer needed yet

Answer 1

I am not sure regarding this but can it be like,

if we find the no.of moles of NaOH present in 48.00mL of water and then find the volume of HClO_4 containing the no. of moles found in the earlier case.

Can such calculation work?

@SoloN8v88 what do you think? :)

Answer 2

the ratio between HClO4 and NaOH is 1:1 so, u can use the formula

HClO4 <-----> NaOH
C1 X V1 = C2 X V2
0.115 X V1 = 8.90 X 10^-2 X 48
V1 = 4.272 / 0.115 = 37.14 mL of HClO4 is required to neutralize

Answer 3

did u have to write a balanced equation first also what is the formula called

Answer 4

HClO4 + NaOH ---> NaClO4 + H2O
this is the balanced equation, and it tells the ratio i.e 1:1

Answer 5

i have open question do you think u can walk me through it without necessarily doing iy for me if thats possible

Answer 6

from balanced equation we find the mole ration between reactants, if the mole ratio is 1:1 then we can simply apply the concentration formula that is:
C1V1 = C2V2 from this formula we can calculate one parameter if we know rest of three parameters.......