The solution would be like this for this specific problem:
Given:
pH of a 0.55 M hypobromous
acid (HBrO) at 25.0 °C = 4.48
[H+] = 10^-4.48 = 3.31 x
10^-5 M = [BrO-] <span>
Ka = (3.31 x 10^-5)^2 / 0.55 = 2 x 10^-9</span>
To add, Hypobromous Acid does not require acid
adjustment, which is necessary for chlorine-based product and is stable and
effective in pH ranges of 5-9.<span>
</span>Hypobromous Acid combines with organic
compounds to form a bromamine. Chlorine also combines with the same organic
compounds to form a chloramine. <span>It is also
one of the least expensive intervention antimicrobial compounds available.</span>
The best way to determine the number of atoms of arsenic in the sample will be to multiply 2.3 by Avagadro's number.
This is because Avagadro's number is the number of particles one mole of any substance has, and its value is 6.02 x 10²³
If the number of moles of a substance are known, then multiplying by Avagadro's number will give the number of particles. In this case, this is 1.38 x 10²⁴.
When 25.6 g 
is burned, the moles of 
emitted into the atmosphere is 1.80 mol
<u>Explanation:</u>
The molar mass of octane is calculated as 8(12) +18(1) = 114 g/mol.
Where atomic mass of Carbon is C=12, and Hydrogen H=1.The sample contains 25.6 g of octane, Therefore
The combustion of octane can be written as:
The mole ratio can be represented as:
= 16:2 = 8:1.
Hence, the quantity of carbon dioxide emitted is:
= 1.80 mol
