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Arrhenius Acid

When 10 ml of...

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When 10 ml of 0.1 M acetic acid (pK_a =5.0) is titrated against 10 ml of 0.1 M ammonia solution (pK_b =5.0) , the equivalence point occurs at pH- (1) 5.0 (2) 6.0 (3) 7.0 (4) 9.0

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10 m L

0.1 M

p K_{a} = 5.0

) is titrated against

10 m L

0.1 M

ammonia solution

(p K_{b} = 5.0)

, the equivalence point occurs at pH:

Q. When 10 mL of 0.1 M acetic acid

(p K_{a} = 5.0)

is titrated against 10 mL of 0.1 M ammonia solution

(p K_{b} = 5.0)

the equivalence point occurs at pH of:

5.0 m L

0.1 M N a O H

solution is added to

50 m L

0.1 M

acetic acid solution. Calculate the

p H

of the resulting acetic acid solution.

(K a = 1.8 \times 10^{- 5})

Q. A solution of weak acid

H A

was titrated with base

N a O H

. The equivalent point was reached when

40 m L

0.1 M N a O H

has been added. Now

20 m L

0.1 M H C l

were added to titraded solution, the

p H

was found to be

5.0

. What will be the

p H

of the solution obtained by mixing

20 m L

0.2 M N a O H

20 m L

0.2 M H A

O H^{-}

concentration at the equivalent point when a solution of

0.1 M

acetic acid is titrated with a solution of

0.1 M

K_{2}

= 1.9 \times 10^{- 3}

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