Dude... h2o, thats why ICE FLOATS ON WATER!!!!
A mixture
having a uniform composition where the components can't be seen separately and
all components are in the same state best describes a solution.
<span>In chemistry, a </span>solution<span> is a
homogeneous mixture composed of two or more substances. In such a mixture, a
solute is a substance dissolved in another substance, known as a solvent.</span>
The correct answer between all
the choices given is the third choice or letter C. I am hoping that this answer
has satisfied your query and it will be able to help you in your endeavor, and
if you would like, feel free to ask another question.
Answer:
K(79°C) = 1.906 E7 s-1
Explanation:
Arrhenius eq:
∴ A = 5.0 E9 s-1
∴ Ea = 16.3 KJ/mol
∴ R = 8.314 E-3 KJ/K.mol
∴ T = 79°C ≅ 352 K ⇒ K = ?
⇒ K(79°C) = (5.0 E9 s-1)e∧[ - (16.3KJ/mol)/(8.314 E-3 KJ/K.mol)(352 K)]
⇒ K(79°C) = (5.0 E9 s-1)e∧(- 5.5697)
⇒ K(79°C) = (5.0 E9 s-1)*(3.811 E-3)
⇒ K(79°C) = 1.906 E7 s-1
Answer:
0.22 mol HClO, 0.11mol HBr.
0.25mol NH₄Cl, 0.12 mol HCl
Explanation:
A buffer is defined as a mixture in solution between weak acid and its conjugate base or vice versa.
Potassium hypochlorite (KClO) could be seen as conjugate base of HClO (Weak acid). That means the addition of <em>0.22 mol HClO </em>will convert the solution in a buffer. HBr reacts with KClO producing HClO, thus, <em>0.11mol HBr</em> will, also, convert the solution in a buffer. 0.23 mol HBr will react completely with KClO and in the solution you will have only HClO, no a buffering system.
Ammonia (NH₃) is a weak base and its conjugate base is NH₄⁺. That means the addition of <em>0.25mol NH₄Cl</em> will convert the solution in a buffer. Also, NH₃ reacts with HCl producing NH₄⁺. Thus, addition of<em> 0.12 mol HCl</em> will produce NH₄⁺. 0.25mol HCl consume all NH₃.
