From the calculations, the pH of the final solution is 9.04.
<h3>What is the pH of the buffer?</h3>
We can use the Henderson Hasselbach equation to obtain the final pH of the solution in terms of the pKb and the base concentration.
Number of moles of salt = 250/1000 L * 0.5 M = 0.125 moles
Number of moles of base = 150/1000 L * 0.5 M = 0.075 moles
Total volume of solution = 250ml + 150ml = 400ml or 0.4 L
Molarity of base = 0.075 moles/ 0.4 L = 0.1875 M
Molarity of salt = 0.125 moles/ 0.4 L = 0.3125 M
pOH = pKb + log[salt/base]
pKb = -log(1.8 x 10^-5) = 4.74
pOH = 4.74 + log[0.3125/0.1875 ]
pOH = 4.96
pH = 14- 4.96
pH = 9.04
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Answer:
1.59 molal
Explanation:
The <u>definition of molality</u> is:
- molality = moles solute / kg of solvent
So first <u>we calculate the moles of solute</u> (D-glucose, C₆H₁₂O₆), using its <em>molar mass</em>:
- 36.0 g C₆H₁₂O₆ ÷ 180.156 g/mol = 0.200 mol C₆H₁₂O₆
Then we<u> convert grams of water into kg</u>:
- 125.9 g H₂O *
= 0.1259 kg H₂O
Finally we <u>calculate the molality</u>:
- m = 0.200 mol / 0.1259 kg
Answer:
203 grams
Explanation:
The no. of moles of (6.3 x 10²⁴ molecules--Avagadros number) of NH₃ = (1.0 mol)(7.2 x 10²⁴ molecules)/(6.022 x 10²³ molecules) = 11.96 mol.
The no. of grams of NH₃ present = no. of moles x molar mass = (11.96 mol)(17.0 g/mol) = 203.3 g ≅ 203.0 g.
Answer:
Acetic
Explanation:
organic chemistry of, pertaining to, or producing vinegar
organic chemistry of or pertaining to acetic acid or its derivatives
Answer:
Atoms: <em>they are tiny particles that are the basic building blocks of any substance. The atoms are themselves made up of even smaller particles-protons, neutrons and electrons. </em>
Molecules: <em>it is the smallest unit of matter, which can exist independently. A molecule is formed when two or more atoms combine together.</em>
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<em>hope it helps</em>
<em>and ur welcm</em>
<em>:)</em>
