<u>Answer:</u> The concentration of 
in three significant figures will be 0.899 mol/L.
<u>Explanation:</u>
For the given reaction:
The above reaction follows zero order kinetics. The rate law equation for zero order follows:
![k=\frac{1}{t}([A_o]-[A])](https://tex.z-dn.net/?f=k%3D%5Cfrac%7B1%7D%7Bt%7D%28%5BA_o%5D-%5BA%5D%29)
where,
k = rate constant for the reaction = 
t = time taken = 10 sec
![[A_o]](https://tex.z-dn.net/?f=%5BA_o%5D)
= initial concentration of the reactant = 0.962 mol/L
[A] = concentration of reactant after some time = ?
Putting values in above equation, we get:
![6.28\times 10^{-3}=\frac{1}{10}(0.962-[A])](https://tex.z-dn.net/?f=6.28%5Ctimes%2010%5E%7B-3%7D%3D%5Cfrac%7B1%7D%7B10%7D%280.962-%5BA%5D%29)
![[A]=0.899mol/L](https://tex.z-dn.net/?f=%5BA%5D%3D0.899mol%2FL)
Hence, the concentration of in three significant figures will be 0.899 mol/L.
25 ml was used to reach the pint
D) otherwise we wouldn't be able to have water, oxygen gas, and all other compounds that have oxygen. We need at least 1 free slot to make a molecule
pH of buffer solution : 4.32
<h3>Further explanation
</h3>
A buffer solution is a solution that can maintain a good pH value due to the addition of a little acid or a little base or dilution.
The buffer solution can be acidic or basic
Acid buffer solutions consist of weak acids(H₂CO₃) and their salts.(NaHCO₃)
mol H₂CO₃
mol NaHCO₃
![\tt [H^+]=Ka\dfrac{mole~weak~acid}{mole~salt}\\\\(H^+]=1.8\times 10^{-5}\dfrac{0.008}{0.003}=4.8\times 10^{-5}\\\\pH=5-log~4.8=4.32](https://tex.z-dn.net/?f=%5Ctt%20%5BH%5E%2B%5D%3DKa%5Cdfrac%7Bmole~weak~acid%7D%7Bmole~salt%7D%5C%5C%5C%5C%28H%5E%2B%5D%3D1.8%5Ctimes%2010%5E%7B-5%7D%5Cdfrac%7B0.008%7D%7B0.003%7D%3D4.8%5Ctimes%2010%5E%7B-5%7D%5C%5C%5C%5CpH%3D5-log~4.8%3D4.32)
