What is the final resulting molarity when mL of a solution is homogeneously mixed with mL of a solut — Redox Reactions and Volumetric Analysis Chemistry Question
Question
What is the final resulting molarity when $150$ mL of a $6.00 M$ $H_2SO_4$ solution is homogeneously mixed with $250$ mL of a $3.00 M$ $H_2SO_4$ solution?
Answer: A
💡 Solution & Explanation
When mixing two non-reacting solutions of the exact same solute, the final molarity formula is $M_f = (M_1V_1 + M_2V_2) / (V_1 + V_2)$ . Calculating the total millimoles = $(150 \times 6.00) + (250 \times 3.00) = 900 + 750 = 1650$ millimoles. Total combined volume = $150 + 250 = 400$ mL. Final molarity = $1650 / 400 = 16.5 / 4 = 4.125 M$ .
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