Question

To what extent must a given solution containing 40 mg AgNO3 per mL be diluted to yield a solution containing 16 mg AgNO3 per mL:

Answer 1

Answer:

AgNO

3(aq]

+

HCl

(aq]

→

AgCl

(s]

⏐

↓

+

HNO

3(aq]

The net ionic equation, which you get after removing the spectator ions, looks like this

Ag

+

(aq]

+

Cl

−

(aq]

→

AgCl

(s]

⏐

⏐

↓

Notice that the reactants take part in the reaction in a  

1

:

1

mole ratio, which means that the reaction will consume equal numbers of moles of silver nitrate and hydrochloric acid, which produce silver cations,  

Ag

+

, and chloride anions,  

Cl

−

, respectively.

Your goal now is to figure out how many moles of each reactant you're mixing together.

For starters, use silver nitrate's molar mass to determine how many moles you get in that  

1.40-g

sample of silver nitrate

1.40

g

⋅

1 mole AgNO

3

169.87

g

=

0.008242 moles AgNO

3

Explanation:

Answer 2

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