Question

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If it requires 23.4 milliliters of 0.65 molar barium hydroxide to neutralize 42.5 milliliters of nitric acid, solve for the molarity of the nitric acid solution. Show all of the work used to solve this problem. Unbalanced equation: Ba(OH)2 + HNO3 Ba(NO3)2 + H2O

Answer 1

@dan815 @pooja195 @peachpi

Answer 2

@cuanchi you can't use the formula M1V1 = M2V2 then solve for molarity in this case, and converting mL to L?

Answer 3

Not really, @Photon336 that equation works when the stoiquimetry is mol to mol or 1:1, for the case of NaCl + NaOH but when you have 1:2 stoichiometry you have to add the ratio 1:2 in the formula too.

M1x V1 = (M2 V2) x2

By the way i made a mistake in the formula, now i think is fine

1) first you have to balance the equation
A Ba(OH)2 + B HNO3 -> C Ba(NO3)2 + D H2O

2) Calculate the moles of barium hydroxide in the 23.4mL of 0.65 M (convert the volume from mL to L)
molaridad Ba(OH)2= number of moles Ba(OH)2 /volume(L)Ba(OH)2 =>
number of moles Ba(OH)2= Molaridad Ba(OH)2 x volume (L) Ba(OH)2 =????

4) according to the stoichiometry of the balanced reaction in 1) calculate how many moles of HNO3 you will need to neutralize the moles of barium hydroxide calculated in 2)

number of moles HNO3 = number of moles Ba(OH)2 x (B noles of HNO3/ A moles of Ba(OH)2 = ???

5 calculate the molaridad of HNO3 with the same formula that you used in 2)
molaridad HNO3= number of moles HNO3 / volume(L) HNO3 = ???