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Question

What is the mass of the precipitate formed when $$50$$mL of $$16.9$$% solution of $$AgNO_3$$ is mixed with 
$$50$$ mL of $$5.8$$% $$NaCl$$ solution ?
(Ag = $$107.8$$, N =$$14$$, O = $$16$$, Na = $$23$$, $$Cl = 35.5$$)


A
7 g
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B
14 g
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C
28 g
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D
3.5 g
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Solution

The correct option is A $$7$$ g
$$50mL\,\, 16.9\%\,AgNO_3=\dfrac{50\times 16.9}{100\times 169}=0.5mol\,AgNO_3$$

$$50mL\,\,15.8\%\,NaCl=\dfrac{50\times 5.8}{100\times 5.8}=0.05mol\, NaCl.$$

$$AgNO_3\underset{aq}{+}NaCl\underset{aq}{\rightarrow} AgCl\downarrow +NaNO_3(aq)$$
   $$ 0.05$$             $$0.05$$            -                   -
        -                   -             $$0.05$$             $$0.05$$

molecular mass of $$AgCl$$=143.3

mass of ppt$$(AgCl)$$ =$$0.05\times 143.3$$
                     $$=7.1gm$$

Hence, option $$A$$ is correct.

Chemistry

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