A general formula of an acid always start with H or the hydronium ion. It has to end with an anion. As acids, these compounds are named starting with the prefix "hydro-," then adding the first syllable of the anion, then the suffix "-ic." Hope this answers the question.
<span />
You should try to strt a conversation with him or say hi introduce yourself or ask him how hes doing just talk to him i guess
Answer: The pH of the substance is 8.25. The solution is basic.
Explanation:
pH or pOH is the measure of acidity or alkalinity of a solution.
pH is calculated by taking negative logarithm of hydronium ion concentration. The acids have pH ranging from 1 to 6.9 , salts have pH of 7 and bases have pH ranging from 7.1 to 14.
![pH=-\log [H_3O^+]](https://tex.z-dn.net/?f=pH%3D-%5Clog%20%5BH_3O%5E%2B%5D)
Putting in the values:
![pH=-\log[5.6\times 10^{-9}]](https://tex.z-dn.net/?f=pH%3D-%5Clog%5B5.6%5Ctimes%2010%5E%7B-9%7D%5D)
Thus as pH is more than 7, the solution is basic.
The pH of the substance is 8.25. The solution is basic.
The number of mole of nitrogen gas, N₂, needed to produce 150 g of ammonia, NH₃ is 4.41 moles
<h3>How to determine the mole of NH₃ produced </h3>
- Mass of NH₃ = 150 g
- Molar mass of NH₃ = 14 + (3×1) = 17 g/mol
Mole = mass /molar mass
Mole of NH₃ = 150 / 17
Mole of NH₃ = 8.82 moles
<h3>How to determine the mole of N₂ needed </h3>
Balanced equation
N₂ + 3H₂ —> 2NH₃
From the balanced equation above,
2 moles of NH₃ were produced by 1 mole of N₂.
Therefore,
8.82 moles of NH₃ will be produced by = 8.82 / 2 = 4.41 moles of N₂.
Thus, 4.41 moles of N₂ is needed for the reaction.
Learn more about stoichiometry:
brainly.com/question/14735801
To minimize the sharp pH shift that occurs when a strong acid is added to a solution, IT IS PRACTICAL TO ADD A WEAK BASE.
When a strong acid is added to a solution, it usually brings about a sharp change in the pH of the concerned solution. To avoid this, one can add a weak base to the solution first. The weak base will serves as a buffer for the strong acid and prevents the solution from experiencing sharp pH variations.
