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Chapter 4: Problem 79

What mass of \(\mathrm{KCl}\) is needed to precipitate the silver ions from \(15.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{AgNO}_{3}\) solution?

Short Answer

Expert verified
The mass of KCl required to precipitate the silver ions from \(15.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{AgNO}_{3}\) solution is approximately \(0.224 \mathrm{g}\).

Step by step solution

01

List the given information and identify the target variable

We have the following information: - Volume of AgNO鈧� solution = 15.0 mL - Concentration of AgNO鈧� solution = 0.200 M - KCl needed to precipitate the silver ions Our target variable is the mass of KCl.
02

Convert volume to liters

Convert the volume of the AgNO鈧� solution from mL to L: \(15.0 \mathrm{~mL} = 15.0 \times 10^{-3} \mathrm{~L}\)
03

Calculate moles of AgNO鈧�

Using the given concentration, calculate the moles of AgNO鈧�: Moles of AgNO鈧� = Concentration 脳 Volume = (0.200 M) 脳 (15.0 脳 10鈦宦� L) Moles of AgNO鈧� = 3.0 脳 10鈦宦� mol
04

Determine stoichiometric ratio

According to the balanced chemical equation, the stoichiometric ratio between AgNO鈧� and KCl is 1:1.
05

Calculate moles of KCl

Since the stoichiometric ratio is 1:1, the moles of KCl required will be equal to the moles of AgNO鈧�. Moles of KCl = Moles of AgNO鈧� = 3.0 脳 10鈦宦� mol
06

Calculate mass of KCl

Using the molar mass of KCl (39.10 g/mol for K and 35.45 g/mol for Cl), find the mass of KCl required: Mass of KCl = Moles of KCl 脳 Molar mass of KCl Mass of KCl = (3.0 脳 10鈦宦� mol) 脳 (39.10 g/mol + 35.45 g/mol) Mass of KCl = (3.0 脳 10鈦宦� mol) 脳 (74.55 g/mol) Mass of KCl 鈮� 0.224 g The mass of KCl required to precipitate the silver ions from 15.0 mL of 0.200 M AgNO鈧� solution is approximately 0.224 g.

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Most popular questions from this chapter

(a) You have a stock solution of \(14.8 \mathrm{M} \mathrm{NH}_{3}\). How many milliliters of this solution should you dilute to make \(1000.0 \mathrm{~mL}\) of \(0.250 \mathrm{M} \mathrm{NH}_{3} ?\) (b) If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of \(0.500 \mathrm{~L}\), what will be the concentration of the final solution?

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