How many grams of Cu would be needed to react with 2.0 mol HNO3?
<span>by the equation </span>
<span>3Cu + 8HNO3 --> 3Cu(NO3)2 + 2NO + 4H2O </span>
<span>2.0 mol HNO3 reacts with 3/8 ths as many moles of Cu = 0.75 moles of Cu </span>
I can help you but what is the question here?
Firstly, colligative properties focus on the NUMBER of particles in the ratio of the solute to the solvent. Finally, examples of such are: the decreasing of vapor pressure, the increasing of one's material to its boiling point, the decreasing again of one's material to its freezing point, and osmotic pressure.
Answer:- pH is 2.14.
Solution:- Nitrous acid, 
is a weak acid so first of all we solve for 
and then figure out the pH.
the equation is written as:
Initial concentration for the acid is given as 0.120 M. Let's say the change in concentration is x. Then the equilibrium concentrations would be as:
= 
=
Ka for nitrous acid is 
and the equilibrium expression for this would be written as:
![Ka=\frac{[H_3O^+][NO_2^-]}{HNO_2}](https://tex.z-dn.net/?f=Ka%3D%5Cfrac%7B%5BH_3O%5E%2B%5D%5BNO_2%5E-%5D%7D%7BHNO_2%7D)
Let's plug in the values in it.
To make the calculations easy we could ignore for the bottom and the expression becomes:
On cross multiply:
On taking square root to both sides:
So, ![[H_3O^+]=7.3*10^-^3M](https://tex.z-dn.net/?f=%5BH_3O%5E%2B%5D%3D7.3%2A10%5E-%5E3M)
Now we could calculate the pH using the pH formula:
![pH=-log[H_3O^+]](https://tex.z-dn.net/?f=pH%3D-log%5BH_3O%5E%2B%5D)
pH = 2.14
So, the pH of 0.120M nitrous acid is 2.14.
40.08 i believe would be it
