Verified Answer :

The solution to the problem is as follows:

The weight of solute required = Molarity x Molecular mass x Volume of solution in mL /1000 =0.15 x 170 x 175 / 1000 = 4.4625g 

Take 4.4625g of AgNO3 and disolve in certain quantity of water(<175 mL) and finally make up the solution to 175mL with water.

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Answer: Therefore, we need to dissolve 4.5 g of [tx]AgNO_3[/tex] and make the volume upto 175 ml.

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution

\(Molarity=\frac{n\times 1000}{V_s}\)

where,

n= moles of solute

\(V_s\) = volume of solution in ml = 175.0 ml

\(moles of solute =\frac{\text {given mass}}{\times {\text {molar mass}}=\frac{x}{170g/mol}\)

Now put all the given values in the formula of molarity, we get

\(0.150M=\frac{x\times 1000}{170\times 175.0ml}\)

\(x=4.5g\)

Therefore, we need to dissolve 4.5 g of [tx]AgNO_3[/tex] and make the volume upto 175 ml.

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