Question

30 mL of 0.100 M HCL and 10.0 mL of 0.470 M HCLH+Cl-

Answer 1

Let us first define what the molarity of a substance corresponds to. This is defined as the moles of solute (n) per liter of solution (V), so we will have the following equation:

`M=(n_T)/(V_T)`

Where,

nT is the total number of moles

VT is the total volume in liters

M is the molarity of the solution

When we have a mixture we must add the total moles and the total volume as follows:

`M=(n_A+n_B)/(V_A+V_B)`

Now, the moles of each solution can be found by clearing the moles of the first equation.

But first, we have two solutions, we will call them solution a and solution b, the conditions are.

Solution a

Va=30mL=0.030L

Ma=0.100M

Solution b

Vb=10.0mL = 0.0100L

Mb=0.470M

Now for each solution, we have the following equation to find the number of moles:

`\begin{gathered} n_A=M_A* V_A \\ n_B=M_B* V_B \end{gathered}`

If we replace this equation into the second equation we will have:

`M=(M_AV_A+M_BV_B)/(V_A+V_B)`

We replace the known data:

`\begin{gathered} M=(0.100M*0.030L+0.470M*0.010L)/(0.030L+0.010L) \\ M=0.19M \end{gathered}`

Since both ions are in the same concentration, that is to one ion per molecule, the concentration will be the same.

H+ = 0.19M

Cl- =0.19M