What is the pH of a buffer that consists of 0.100 M $H C O O H$ $HCOOH$ and 0.540 M $H C O O N a$ $HCOONa$ ?

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What is the pH of a buffer that consists of 0.100 M $H C O O H$ $HCOOH$ and 0.540 M $H C O O N a$ $HCOONa$ ?

The $p K_{a}$ $pK_a$ of formic acid is 3.74.

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Answer 1 · 2016-04-21T18:14:03

$p H$ $pH$ $>$ $>$ $3.74$ $3.74$

Explanation:

$pH=pKa+log10{[A_][HA]}$ $pH = pK_a + log_10{[[A^_]]/[[HA]]}$

$p H = 3.74 + {log}_{10} {\frac{0.540 \cdot m o l \cdot L^{- 1}}{0.100 \cdot m o l \cdot L^{- 1}}}$ $pH = 3.74 + log_10{[0.540*mol*L^-1]/[0.100*mol*L^-1]}$

You'll have to do the calculation.

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What is the pH of a buffer that consists of 0.100 M $H C O O H$ $HCOOH$ and 0.540 M $H C O O N a$ $HCOONa$ ?

The $p K_{a}$ $pK_a$ of formic acid is 3.74.

1 Answer

Explanation:

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What is the pH of a buffer that consists of 0.100 M HCOOHHCOOH and 0.540 M HCOONaHCOONa?

The pKapK_a of formic acid is 3.74.

1 Answer

Explanation:

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Impact of this question

What is the pH of a buffer that consists of 0.100 M $H C O O H$ $HCOOH$ and 0.540 M $H C O O N a$ $HCOONa$ ?

The $p K_{a}$ $pK_a$ of formic acid is 3.74.