The final molarity of potassium cation in the solution is 6.70 × 10⁻⁵ M.
Step 1: Calculate the moles of potassium chloride
moles of potassium chloride = grams of potassium chloride / molar mass of potassium chloride
moles of potassium chloride = 1.75 g / 74.55 g/mol
moles of potassium chloride = 0.0235 mol
Step 2: Calculate the total volume of the solution
total volume of solution = volume of ammonium sulfate solution + volume of potassium chloride solution
total volume of solution = 350.0 mL + 0.0 mL
total volume of solution = 350.0 mL
Step 3: Calculate the final molarity of potassium cation
final molarity of potassium cation = moles of potassium chloride / total volume of solution
final molarity of potassium cation = 0.0235 mol / 350.0 mL
final molarity of potassium cation = 0.000067 M
Round to 3 significant digits:
final molarity of potassium cation = 6.70 × 10⁻⁵ M.
Question
Suppose 1.75g of potassium chloride is dissolved in 350.mL of a 54.0 mM aqueous solution of ammonium sulfate. Calculate the final molarity of potassium cation in the solution. You can assume the volume of the solution doesn't change when the potassium chloride is dissolved in it. Round your answer to 3 significant digits.