The right answer for the question that is being asked and shown above is that: "B 1.5 X 1-^-5 ppm." A 250-mL aqueous solution contains 1.56 mc025-1.jpg 10–5 g of methanol and has a density of 1.03 g/mL. The concentration in ppm is that <span>1.5 X 1-^-5 ppm</span>
Answer:
Yes, it is.
Explanation:
A buffer is a solution in which a weak acid is in equilibrium with its conjugate base, or a weak base is in equilibrium with its conjugate acid. Because of the equilibrium, when an acid or a base is added to it, the pH remains almost unaltered.
But the buffer has a limit, generally, it works well in the range of pKa - 1 to pKa +1. The pKa value indicates the force of the acid, and it's calculated by -logKa, where Ka is the equilibrium constant of the acid. The pKa value of citric acid is 6.86, does a buffer of it can function well at pH 7.
The successive deprotonations of the acid increase the "-" charge density on the resulting anion, in this case, the carboxylate groups. This is unfavorable electrostatic repulsions between the anions which reduces the likelihood that a proton would dissociate. So, it's more favorable for the proton to remain bound to reduce unfavorable charge repulsion. Because of that, the equilibrium can be achieved.
Molar Mass: 300.0510 g/mol
Answer:
The answer to your question is 52.35 g of O₂
Explanation:
mass of oxygen = ?
mass of KClO₃ = 66.8 g
Chemical balanced reaction
KClO₃ ⇒ 2 KCl + 3O₂
Process
1.- Calculate the molar mass of KClO₃ and Oxygen
KClO₃ = 39 + 35.5 + (16 x 3) = 122.5 g
O₂ = 16 x 6 = 96 g
2.- Write proportions to solve this problem
122.5 g of KClO₃ ----------------- 96 g of O₂
66.8 g ----------------- x
x = (66.8 x 96) / 122.5
x = 6412.8/122.5
x = 52.35 g of O₂
<span>the special property of water as universal solvent is because of the existing hydrogen bonding between oxygen and hydrogen molecules. Adhesion and cohesion are one of the repercussions of hydrogen bonding. Higher temperature causes hydrogen bonds to break while lower thresholds causes them to stabilize the bonds.
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