91Ó°ÊÓ

• The amount of a material in a given volume of solution is measured in molarity (M).
• The mole of a solute per litre of a solution is known as molarity.
• The molar concentration of a solution is also known as molarity.

It is necessary to compute the mass of each species in a given mixture.

The ratio of moles of solute (in grammes) to the volume of the solution is known as molarity (in litres). The formula for calculating a solution's molarity is:

The mass of each species in a given mixture is to be calculated.

Given,

1.000MHCI

The reaction that takes place in a solid mixture is

$$\begin{gathered} {\mathrm{K}}_2{\mathrm{CO}}_3+2\mathrm{HCI}→2{\mathrm{KCI}}_{\left(\mathrm{aq}\right)}+{\mathrm{H}}_2\mathrm{O}+{\mathrm{CO}}_2 \\ {\mathrm{KHCO}}_3+\mathrm{HCI}→{\mathrm{KCI}}_{\left(\mathrm{aq}\right)}+{\mathrm{KCI}}_{\left(\mathrm{aq}\right)}+{\mathrm{H}}_2\mathrm{O}+{\mathrm{CO}}_2 \end{gathered}$$

The number of moles in the

$$\begin{gathered} \mathrm{HCI}=0.015\mathrm{L}×1.000\mathrm{M} \\ =0.015\mathrm{molHCI} \end{gathered}$$

The vast majority of ${\mathrm{K}}_2{\mathrm{CO}}_3\mathrm{and}{\mathrm{KHCO}}_3$

The mass of a given combination is ${\mathrm{K}}_2{\mathrm{CO}}_3$+ mass of ${\mathrm{KHCO}}_3=2.000\mathrm{g}$

$2\left(\mathrm{molof}{\mathrm{K}}_2{\mathrm{CO}}_3\right)+\left(\mathrm{mol}\mathrm{of}{\mathrm{KHCO}}_3\right)=0.015\mathrm{mol}$

It obtain by substituting y in the previous equation.

$\mathrm{x}=1.811\mathrm{g}\mathrm{and}\mathrm{y}=0.189\mathrm{g}$

Each species' weight in a specific mixture was calculated.

The burden of ${\mathrm{K}}_2{\mathrm{CO}}_3$is present in the given mixture 1.811 g .

The burden of ${\mathrm{KHCO}}_3$in given mixture is 0.189 g.