Chapter 4.6, Problem 1RCF

Interpretation Introduction

Interpretation:

Mass of $AgBr$ formed in the solution containing $6g$ of $KBr$ when treated with excess of $AgN{O}_3$ has to be calculated.

Concept introduction:

The mass of the precipitate is depends on the reactant masses.

Mole:

The mole of the solute is calculated by multiplication of concentration of solution and volume of the solution and it is,

$\text{Mole}\text{=}\text{Concentration}\text{(M)×}\text{volume}\text{(L)}$

$\text{Molarity = }\frac{\text{No}\text{. of moles of solute}}{\text{Volume of solution in L}}$

Mass:

The mass of solute present in the solution is given by multiplication of mole and molar mass of the solute.

$\text{Mass}\text{=}\text{Mole}\text{×}\text{Molar}\text{mass}$

$Masspercent=\frac{Massofsolute}{Massofsolution}\times 100\%$