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Basic Buffer Action

71 Calculate ...

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71 Calculate the amount of (NH4)2SO4 which must be added to 500 ml of 0.2 (M) NH3 to yield asolution of pH = 9.35. (pKb(NH4OH) = 4.74 )

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Q. Calculate the amount of

(N H_{4})_{2} S O_{4}

in g which must be added to

500

0.2

N H_{3}

to yield a solution of

p H = 9.35

K_{b}

N H_{3} = 4.7

Q. Calculate the weight of

(N H_{4})_{2} S O_{4}

which must be added to 500 mL of 0.2 M

N H_{3}

to yield a solution of pH = 9.35,

K_{b}

N H_{3} = 1.78 \times 10^{- 5}

Q. Calculate the weight of

(N H_{4})_{2} S O_{4}

which must be added to 500 mL of 0.2 M

N H_{3}

to yield a solution of pH = 9.35,

K_{b}

N H_{3} = 1.78 \times 10^{- 5}

(in gm)(Write answer nearest integer)

Q. What will be the amount of

(N H_{4})_{2} S O_{4}

(in g) which must be added to 500 mL of 0.2 M

N H_{4} O H

to yield a solution of pH 9.35? [Given,

p K_{a}

N H_{4}^{+}

p K_{b} (N H_{3})

p K_{a} (N H_{4}^{+})

]

Q. The amount of

(N H_{2})_{4} S O_{4}

g

, which must be added to

500 mL

0.2 M

N H_{3}

to yield a solution of

p H = 9.35

K_{b}

N H_{3}

\times

10^{- 5}

will be:( Give your answer upto two decimal only.)
(Given,

log 1.6 = 0.2, log 70 = 1.85

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