The pH of a solution which is 0.023 m in weak base and 0 037 m in the conjugate weak acid whose Ka= 7.1 × 10⁻⁶ is 4.93.
pH determines the amount of hydrogen and hydroxide ions in a solution. It is the negative logarithm of hydrogen ion concentration.
Given,
Ka= 7.1 × 10⁻⁶
Weak base = 0.023M
Acid = 0.037M
Using base dissociation constant, Ka we can calculate pKa by:
pKa = -log [Ka]
pKa = -log [7.1 × 10⁻⁶]
pKa = 5.15
A weak base and its conjugate acid are present in equal proportions in buffer solution. Using the Henderson-Hasselbalch equation, we can find out the pH of a buffer solution that constitutes a weak base and its conjugate acid.
Using Henderson-Hasselbalch equation,
pH = pKa + log [Weak base / acid]
pH = 5.15 + log [0.023 / 0.037]
pH = 5.15 + log[0.6]
pH = 5.15 - 0.22
pH = 4.93
Therefore, the pH of the solution is 4.93.
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The answer is A. Na
because it's<span /> 5,1391
The answer is 0.0171468704904. We assume you are converting between moles Mg(OH)2 and gram. This compound is also known as Magnesium Hydroxide. 1 mole<span> is equal to </span>1 moles<span> Mg(OH)2, or 58.31968 grams.</span>
The mole is an SI unit representing a specific quantity of atoms of an element or molecules of a compound. There are 6.02 x 1023 atoms in a mole of an element or 6.02 x 1023 molecules in a compound. 6.02 x 1023 is known as Avogadro's number.
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