Blood is buffered by carbonic acid and the bicarbonate ion. No...

Question

Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO₃^- and 0.0012 M H₂CO₃ (pK_a1 for H₂CO₃ at body temperature is 6.1).

c. Given the volume from part (b), what mass of NaOH can be neutralized before the pH rises above 7.8?

Accepted Answer

1. The first step is to understand the concept of buffers. A buffer is a solution that can resist pH change upon the addition of an acidic or basic components. It is able to neutralize small amounts of added acid or base, thus maintaining the pH of the solution relatively stable. This is achieved by including a weak acid and its conjugate base (as in this case, $$H_{2}CO$$_{3} and HCO_{3}^{-}).. 2. The Henderson-Hasselbalch equation is used to calculate the pH of a buffer solution. The equation is: pH = pKa + log([A-]/[HA]), where [A-] is the molar concentration of the base (HCO_{3}^{-} in this case) and [HA] is the molar concentration of the acid ($$H_{2}CO$$_{3} in this case).. 3. To find the pH at which NaOH can be neutralized, we need to rearrange the Henderson-Hasselbalch equation to solve for [A-]/[HA]. This gives us: [A-]/[HA] = 10^(pH - pKa). We can then substitute the given pH (7.8) and pKa (6.1) into this equation to find the ratio of [A-] to [HA] at this pH.. 4. Once we have the ratio of [A-] to [HA], we can use it to calculate the amount of NaOH that can be neutralized. This is because the addition of NaOH will consume $$H_{2}CO$$_{3} and produce HCO_{3}^{-}, changing the ratio of [A-] to [HA]. We can set up an equation representing this reaction and solve for the amount of NaOH that can be added before the ratio of [A-] to [HA] reaches the value calculated in step 3.. 5. Finally, once we have the amount of NaOH in moles, we can convert it to mass by multiplying by the molar mass of NaOH (approximately 40 g/mol). This will give us the mass of NaOH that can be neutralized before the pH rises above 7.8.

Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO₃^- and 0.0012 M H₂CO₃ (pK_a1 for H₂CO₃ at body temperature is 6.1).
c. Given the volume from part (b), what mass of NaOH can be neutralized before the pH rises above 7.8?

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Buffer Systems

pKa and Acid-Base Equilibrium

Neutralization Reactions

Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3- and 0.0012 M H2CO3 (pKa1 for H2CO3 at body temperature is 6.1).c. Given the volume from part (b), what mass of NaOH can be neutralized before the pH rises above 7.8?