Question

Suppose 0.0263 g of ammonium bromide is dissolved in 50 mL of a 19.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the ammonium bromide is dissolved in it.

Answer 1

To calculate the final molarity of bromide anion in the solution, divide the number of moles of bromide anion by the volume of the solution. In this case, the final molarity of bromide anion is 0.0054 M.

Step-by-step explanation:

To calculate the final molarity of bromide anion in the solution, we need to determine the number of moles of ammonium bromide and the volume of the solution. First, calculate the number of moles of ammonium bromide by dividing the given mass (0.0263 g) by its molar mass (97.0 g/mol). This gives us 0.00027 mol.

Next, calculate the number of moles of bromide anion by dividing the number of moles of ammonium bromide by its stoichiometric coefficient. Ammonium bromide has one bromide anion per formula unit, so the number of moles of bromide anion is also 0.00027 mol.

Finally, calculate the final molarity of bromide anion by dividing the number of moles of bromide anion by the volume of the solution in liters. The volume is given as 50 mL, which is equivalent to 0.050 L. Dividing 0.00027 mol by 0.050 L gives a final molarity of 0.0054 M for bromide anion.