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Chapter 4: Problem 38

If \(10 .\) g of AgNO \(_{3}\) is available, what volume of 0.25$M \mathrm{AgNO}_{3}$ solution can be prepared?

Short Answer

Expert verified
The volume of the 0.25M AgNO3 solution that can be prepared from 10g of AgNO3 is 0.2356 Liters.

Step by step solution

01

Calculate the molar mass of AgNO3

To calculate the molar mass of AgNO3, we add the molar masses of the elements that make up AgNO3: silver (Ag), nitrogen (N), and oxygen (O). Molar mass of AgNO3 = (molar mass of Ag) + (molar mass of N) + (3 × molar mass of O) The molar masses of each element are: Ag = 107.87 g/mol N = 14.01 g/mol O = 16.00 g/mol Molar mass of AgNO3 = (107.87 g/mol) + (14.01 g/mol) + (3 × 16.00 g/mol) = 169.87 g/mol
02

Convert mass of AgNO3 to moles

10 grams of AgNO3 is given. To find the moles of AgNO3, we can use the formula: moles = mass (g) / molar mass (g/mol) moles = 10 g / 169.87 g/mol = 0.0589 mol So, we have 0.0589 moles of AgNO3.
03

Use the molarity equation to find the volume of the solution

Now that we have the number of moles of AgNO3, we can use the molarity equation: Molarity (M) = moles of solute / volume of solution (in Liters) We want the solution's molarity to be 0.25M, and we have 0.0589 moles of AgNO3. Now we can solve for the volume: 0.25 M = 0.0589 mol / volume (L) volume (L) = 0.0589 mol / 0.25 M = 0.2356 L The volume of the 0.25M AgNO3 solution can be prepared from 10g of AgNO3 is 0.2356 Liters.

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Most popular questions from this chapter

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