Question

Two different bromide solutions are mixed with each other: Solution 1 is an aqueous solution of 4.85 g aluminum bromidein 150. ml water and solution 2 has a volume of 175 ml and contains 7.75 g of zinc bromide. You mix the two solutions together in a large beaker. What is the bromide concentration in moles/L in the mixture

Answer 1

M=0.380 M.

Step-by-step explanation:

Hello there!

In this case, given those two solutions of aluminum bromide and zinc bromide, it is firstly necessary to compute the moles of bromide ions in each solution as shown below:

`n_(Br^-)^(in\ AlBr_3)=4.85 gAlBr_3*(1molAlBr_3)/(266.69gAlBr_3)*(3molBr^-)/(1molAlBr_3) =0.05456molBr^-\\\\n_(Br^-)^(in\ ZnBr_2)=7.75gZnBr_2*(1molZnBr_2)/(225.22gZnBr_2)*(2molBr^-)/(1molZnBr_2) =0.06882molBr^-`

Now, we compute the total moles of bromide:

`n_(Br^-)=0.05456mol+0.06882mol\\\\n_(Br^-)=0.12338mol`

Then, the total volume in liters:

`150mL+175mL=325mL*(1L)/(1000mL) \\\\=0.325L`

Therefore, the concentration of total bromide is:

`M=(0.12338mol)/(0.325L)\\\\M=0.380M`

Best regards!