Question

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 yields Ba(NO3)2 + H2O

Answer 1

start off by balancing the equation

Answer 2

let me know what you get

Answer 3

Ba(N03)2+2H20

Answer 4

@Vocaloid

Answer 5

not quite

Answer 6

what about the NO3 part?

Answer 7

im not sure

Answer 8

there are 2 NO3 ions on the right side and 1 on the left side

Answer 9

so we must balance them out like so:

Answer 10

Ba(OH)2 + 2HNO3 ----> Ba(NO3)2 + 2H2O

Answer 11

and then what? thank you for your help

Answer 12

we calculate the moles of barium hydroxide using

moles = concentration * volume

Answer 13

so if we have

(23.4/1000) L * 0.65 M Ba(OH)2 we have

Answer 14

0.01521 moles of barium hydroxide

Answer 15

now, if we need 2 moles of nitric acid per 1 mole of barium hydroxide, how much nitric acid do we need?

Answer 16

3 moles?

Answer 17

we have

0.01521 moles of barium hydroxide

we need twice as much nitric acid as barium hydroxide

how many moles of barium hydroxide do we need?

Answer 18

would you multiply .01521 by 2 for your answer

Answer 19

yes

Answer 20

that gives us 0.03042 moles

one last step:

Answer 21

divide that by the volume of nitric acid

Answer 22

0.03042/(42.5/1000) = your answer

Answer 23

is that the final answer ?:)

Answer 24

well, i mean, you need to actually calculate what 0.03042/(42.5/1000) is equal to

Answer 25

let me know what you get

Answer 26

.7157

Answer 27

good, now convert that to 2 sig figs

Answer 28

.71?

Answer 29

almost, 0.72

Answer 30

Medal for you !!!!!

Answer 31

THANK YOU SO MUCH