Which of the following buffers is used to maintain the $pH$ of human blood naturally?

  • A
    Hydrogen cyanide and sodium cyanide
  • B
    Copper hydroxide and copper chloride
  • C
    Carbonic acid and salt of carbonic acid
  • D
    Ammonium hydroxide and ammonium chloride

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$0.1 \ M$ $CH_3COOH$ is titrated against $0.1 \ M$ $NaOH$. What would be the difference in $pH$ between $1/4$ and $3/4$ stages of neutralization of the acid?

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The Henderson-Hasselbalch equation for an acidic buffer is given by $pH - pK_a = 5$. This condition holds true when:

$A$ buffer solution is a mixture of

$0.1 \ M$ formic acid solution is titrated against $0.1 \ M \ NaOH$ solution. What would be the difference in $pH$ between $1/5$ and $4/5$ stages of neutralization of acid?

What volume (in $mL$) of $0.10 \, M$ sodium formate is required to be added to $50 \, mL$ of $0.05 \, M$ formic acid to prepare a buffer solution with $pH = 4.0$? (Given: $pK_a$ of formic acid $= 3.7$)

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