Answer:
I don't know the answer but I do really like your profile picture, it's cool. He is my favorite character from Demon Slayer
The pH of the solution is 1.38.
Mass of HCl = 614 mg = 0.614 g
Moles of HCl = 0.614g / 36.5 gmol⁻¹
Concentration of HCl :
Concentration= moles/volume of solution in liters
On adding 0.01682 moles to 400 mL of water that 0.4 L of water.
[HCl]=0.01682 mol/0.4 L= 0.04205 M
HCl (s) + H₂O (l) → H₃O⁺ (aq) +Cl⁻
1 mole of HCl gives 1 mole of hydronium ion and 1 mole of chloride ions in an aqueous solution.
Then 0.04205 mol/L of HCl will give:
1x0.04205 M= 0.04205 mol/L of hydronium ions.
[H₃O⁺]= 0.04205 M
pH= -log[H₃O⁺]
pH= -log[0.04205 M]
= 1.38
The pH of the solution is 1.38.
The complete question is- A chemist dissolves 614. mg of pure hydrochloric acid in enough water to make up 400 mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places. X 5 ?
Learn more about pH of the solution here-
brainly.com/question/11300720
#SPJ4
The paper is not clear so please ask your problem again with more clear print
Answer:
The answer to your question is -NH₂ (amino group)
Explanation:
Organic bases are proton acceptors and they most of the times have nitrogen in their structure.
Organic bases have nitrogen in their structure.
Example of bases:
Alkanamines
Imidazole
Guanidine
Pyridine
Hydroxides (they do not have nitrogen but, are organic bases=