what concentration of Br- results when 831 mL of 0.747 M HBr is mixed with 611 mL of 0.561 M FeBr2

It's okay just fail chem dw it wont harm you.

Well, let's do some calculations to find out!

To find the concentration of Br-, we need to consider the moles of Br- present in each compound. For HBr, the ratio is 1:1 (1 H and 1 Br). So, if we have 831 mL of 0.747 M HBr, we can calculate the moles of Br- from that:

Moles of HBr = Volume (L) × Concentration (M)
Moles of HBr = 0.831 L × 0.747 M
Moles of HBr = 0.618 MOles

Since the ratio of Br- to FeBr2 is 1:2 (1 Br and 2 FeBr2), we also need to consider the moles of FeBr2:

Moles of FeBr2 = Volume (L) × Concentration (M)
Moles of FeBr2 = 0.611 L × 0.561 M
Moles of FeBr2 = 0.343 MOles

Since there are 2 moles of FeBr2 for every 1 mole of Br-, we need to double the moles of FeBr2:

Moles of Br- (from FeBr2) = 2 × Moles of FeBr2
Moles of Br- (from FeBr2) = 2 × 0.343 Moles
Moles of Br- (from FeBr2) = 0.686 MOles

Now, to find the total moles of Br-, we add together the moles from HBr and FeBr2:

Total Moles of Br- = Moles of Br- (from HBr) + Moles of Br- (from FeBr2)
Total Moles of Br- = 0.618 Moles + 0.686 Moles
Total Moles of Br- = 1.304 Moles

Now we can calculate the concentration of Br- in the final mixture:

Concentration of Br- = Total Moles of Br- / Total Volume (L)
Concentration of Br- = 1.304 Moles / (0.831 L + 0.611 L)
Concentration of Br- = 1.304 Moles / 1.442 L
Concentration of Br- ≈ 0.904 M

So, the concentration of Br- in the final mixture is approximately 0.904 M.

To find the concentration of Br- after mixing the two solutions, we need to consider the balanced chemical equation for the reaction between HBr and FeBr2:

HBr + FeBr2 -> FeBr2 + H2

From the equation, we can see that each HBr molecule reacts with one FeBr2 molecule to form FeBr2 and H2. This means that the concentration of Br- remains the same after the reaction.

First, we need to find the initial moles of HBr and FeBr2 before mixing the solutions.

Moles of HBr = Volume (L) x Concentration (M)
= 0.831 L x 0.747 M
= 0.619457 moles

Moles of FeBr2 = Volume (L) x Concentration (M)
= 0.611 L x 0.561 M
= 0.343821 moles

Now, let's calculate the total moles of Br- in the solution after mixing:

Total moles of Br- = Moles of HBr + Moles of FeBr2
= 0.619457 moles + 0.343821 moles
= 0.963278 moles

To find the concentration of Br-, we need to divide the total moles of Br- by the total volume of the solution after mixing:

Total volume of the solution = Volume of HBr + Volume of FeBr2
= 0.831 L + 0.611 L
= 1.442 L

Concentration of Br- = Total moles of Br- / Total volume of the solution
= 0.963278 moles / 1.442 L
≈ 0.668 M

Therefore, the concentration of Br- in the solution after mixing is approximately 0.668 M.

mols Br^- from HBr = M x L = ?

mols Br^- from FeBr2 = M x L x 2 = ?
M Br^- in solution = (total mols/total L)