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Byju's Answer

Standard IX

Chemistry

pH of a Solution

A Student pla...

Question

A Student planned an experiment that would use $0.10 M$ propionic acid, $C H_{3} C H_{2} C O O H$ . Calculate the value of $[H^{+}]$ and the $p H$ for this solution. For propionic acid, $K_{a} = 1.34 \times 10^{- 5}$ .

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Solution

$[H^{+}] = \sqrt{C K_{a}}$
$[H^{+}] = \sqrt{0.10 \times 1.34 \times 10^{- 5}}$
$[H^{+}] = 0.001158 M$
$p H = - l o g_{10} [H^{+}]$
$p H = - l o g_{10} 0.001158$
$p H = 2.94$

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Similar questions

Q. The

K_{a}

of propionic add is

1.34 \times 10 - 5

. What is the

p H

of a solution containing

0.5

M propionic acid and

0.5

M sodium propionate?

Q. What will be the new

p H

0.01 m o l

H C l

is added to a

1 L

buffer solution that is

0.02 M

in propionic acid

(C H_{3} C H_{2} C O O H)

and

0.015 M

in sodium propionate

(C H_{3} C H_{2} C O O N a)

?
Dissociation constant

K_{a}

of propionic acid at

25^{\circ} C

1.34 \times 10^{- 5}

(Take

l o g (1.34) = 0.13

)

Q. A buffer solution was prepared by dissoving

0.02

mol propionic acid and

0.015

mol sodium propionate in enough water to make

1.00 L

of solution.

(K_{a}

for propoinic acid is

1.34 \times 10^{- 5}

). What is the

p H

of the buffer?

Q. How many moles of sodium propionate

(C H_{3} C H_{2} C O O N a)

should be added to one litre of an aqueous solution containing 0.02 mole of propionic acid

(C H_{3} C H_{2} C O O H)

to obtain a buffer solution of

p H = 5.87

?
Dissociation constant of propionic acid

K_{a}

25^{\circ} C

1.34 \times 10^{- 5}

Take

l o g (1.34) = 0.13

Q. How many moles of sodium propionate

(C H_{3} C H_{2} C O O N a)

should be added to one litre of an aqueous solution containing 0.02 mole of propionic acid

(C H_{3} C H_{2} C O O H)

to obtain a buffer solution of

p H = 5.87

?
Dissociation constant of propionic acid

K_{a}

25^{\circ} C

1.34 \times 10^{- 5}

Take

l o g (1.34) = 0.13

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A Student planned an experiment that would use 0.10 M propionic acid, CH3CH2COOH. Calculate the value of [H+] and the pH for this solution. For propionic acid, Ka=1.34×10−5.

[H+]=√CKa[H+]=√0.10×1.34×10−5[H+]=0.001158 MpH=−log10[H+]pH=−log100.001158pH=2.94

A Student planned an experiment that would use $0.10 M$ propionic acid, $C H_{3} C H_{2} C O O H$ . Calculate the value of $[H^{+}]$ and the $p H$ for this solution. For propionic acid, $K_{a} = 1.34 \times 10^{- 5}$ .

$[H^{+}] = \sqrt{C K_{a}}$
$[H^{+}] = \sqrt{0.10 \times 1.34 \times 10^{- 5}}$
$[H^{+}] = 0.001158 M$
$p H = - l o g_{10} [H^{+}]$
$p H = - l o g_{10} 0.001158$
$p H = 2.94$