# Henderson-Hasselbalch Equation - Video Tutorials & Practice Problems

## Henderson-Hasselbalch Equation

## Henderson-Hasselbalch Equation Example

The K_{b} of C_{6}H_{5}NH_{2} (aniline) is 3.9 × 10^{−}^{10}. Determine pH of a buffer solution made up of 500 mL of 1.4 M C_{6}H_{5}NH_{2} and 230 mL of 2.3 M C_{6}H_{5}NH_{3}^{+}.

Determine the buffer component concentration ratio (CB/WA) for a buffer with a pH of 4.7. K_{a} of boric acid (H_{3}BO_{3}) is 5.4 × 10^{−}^{10}.

^{−5}: 1

^{−5}

Calculate mass of NaN_{3} that needs be added to 1.8 L of 0.35 M HN_{3} in order to make a buffer with a pH of 6.5. K_{a} of hydrazoic acid is 1.9 × 10^{−}^{5}.

_{3}

^{−2}g NaN

_{3}

^{3}g NaN

_{3}

_{3}

## Calculating Buffer Range

## Henderson-Hasselbalch Equation Example

Which of the following weak acid-conjugate base combinations would result in an ideal buffer solution with a pH of 9.4?

a) formic acid (HCHO_{2}) and sodium formate (K_{a} = 1.8 x 10^{-4})

b) benzoic acid (HC_{7}H_{5}O_{2}) and potassium benzoate (K_{a} = 6.5 x 10^{-5})

c) hydrocyanic acid (HCN) and lithium cyanide (K_{a} = 4.9 x 10^{-10})

d) iodic acid (HIO_{3}) and sodium iodate (K_{a} = 1.7 x 10^{-1})

_{2}) and sodium formate (K

_{a}= 1.8 x 10

^{-4})

_{7}H

_{5}O

_{2}) and potassium benzoate (K

_{a}= 6.5 x 10

^{-5})

_{a}= 4.9 x 10

^{-10})

_{3}) and sodium iodate (K

_{a}= 1.7 x 10

^{-4})

## Do you want more practice?

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