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If a strong acid is mixed with a weak base, pH=pKa+/-1 in the buffer region.
Corrected:
If a strong base is mixed with a weak acid pOH= pKb +/-1 ( pH=(14 - pKb)+/-1) in the buffer region
[Remember: For one conjugated pair of weak acid (a = HB) AND its weak base (b = B-):
pKa + pKb = 14.0
and
pH + pOH = 14.0
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An electronic device used to determine the pH of a solution?
pH meter
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What factors determine the buffering capacity of a solution?
The concentration of the buffer (the higher the concentration, the larger the buffering capacity) and how close the pKa of the buffer is compared to the pH of the solution (the closer the greater the buffer capacity).See the Related Questions to the left for more information on buffers.
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How is the buffering of an acid different from its neutralization?
Buffering of an acid involves maintaining its pH by resisting changes when an acid or base is added, while neutralization is the reaction between an acid and a base to produce water and a salt, resulting in a pH closer to neutral (pH 7). In buffering, the acid remains relatively unchanged, while in neutralization, the acid is consumed and pH is altered.
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The body regulates pH through the buffering system, which involves substances that can accept or donate protons to help stabilize pH. The kidneys help regulate pH by excreting or conserving bicarbonate ions, while the lungs regulate pH by controlling carbon dioxide levels in the blood. Together, these systems work to maintain the body's pH within a normal range.
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In general, you can look at the pKa (or pKb) of the weak acid (base), and go 1 pH unit above and below that for relatively efficient buffering. Of course, buffer capacity of the particular buffer in use will be important also.
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