<u>Answer:</u> The pH of the solution is 11.24
<u>Explanation:</u>
We are given:
Molarity of ammonia = 0.2 M
The given chemical equation follows:
I: 0.2
C: -x +x +x
E: 0.2-x x x
The expression for equilibrium constant follows:
![K_b=\frac{[NH_4^+][OH^-]}{[NH_3]}](https://tex.z-dn.net/?f=K_b%3D%5Cfrac%7B%5BNH_4%5E%2B%5D%5BOH%5E-%5D%7D%7B%5BNH_3%5D%7D)
Putting values in above expression, we get:
Neglecting the negative value of x as concentration cannot be negative.
So, ![[OH^-]=x=1.88\times 10^{-3}M](https://tex.z-dn.net/?f=%5BOH%5E-%5D%3Dx%3D1.88%5Ctimes%2010%5E%7B-3%7DM)
pOH is defined as the negative logarithm of hydroxide ion concentration present in the solution.
![pOH=-\log [OH^-]](https://tex.z-dn.net/?f=pOH%3D-%5Clog%20%5BOH%5E-%5D)
Putting values in above equation, we get:
We know:
Hence, the pH of the solution is 11.24
Answer:
9
Explanation:
To balance the equation, we need to supply the number of missing coefficients.
There are 2 moles of aluminium on the right hand side, so automatically we need to multiply the number of moles of aluminium by 2 on the left hand side.
There are 3 sulphate ions on the right hand side so we need to multiply the number on the left by 3.
And lastly since we have 6 hydrogen molecules on the left hand side now, we need to multiply the hydrogen on the right hand side by 3 to give 6
The set of coefficients = 2 3 1 3
Adding all thus yields 9
Answer:
They both have a cell membrane, however a plant also has a cell wall.
Explanation:
The pH meter can only be used to differentiate between weak and strong acids providing that the concentrations are known. However, it is convenient to determine the concentration of an acid (or base) by titration.
