Question

What is the molarity of the H+ ion when 11.1g HNO3 are dissolved in 900 ml of H2O?

I'm not sure how to get the answer. Could someone please show me how to do this problem step-by-step?

Answer 1

first you must find mole of HNO3
mole = mass/Mr = 11.1/63 = 0.176
volume of water 900 ml = 0.9 litres
Molar = mole/volume = 0.176/0.9 = 0.196

Answer 2

then you ionized HNO3 --> H+ + NO(3-)
molarity of H+ equal to molarity of HNO3

Answer 3

sorry, where did you get the 63 from? Mr? Did you mean M?

Answer 4

Mr is realtive molecular mass
H = 1
N = 14
O = 16
Mr for HNO3 = 1x1 + 1x14 + 3x16 = 63

Answer 5

Oh okay.

Just to clarify, after you calculate everything else and you do mol/volume then that's my final answer right?

Answer 6

it depends. for this problem because only 1 ion of H+ so thats the final answer. But if there is more ion H+ you must multiply with the number of H+

Answer 7

Okay, so if it had been H2NO3 then I would multiply by 2. Got it. Thank you very much!

Answer 8

yup you r right. Ur welcome