A scientist measures the concentration of a solution at 0.5 M. She dilutes the solution by adding 200 mL of water to 300 mL of the original solution. What is the new concentration of the solution?
["Title: How to Calculate New Concentration After Dilution – A Practical Guide", "---", "When working in a chemistry lab, accurately measuring and adjusting solution concentrations is essential for reliable results. A common scenario involves diluting a stock solution to achieve a desired concentration. In this article, we explore how a scientist measures a solution at 0.5 M and dilutes it by adding 200 mL of water to 300 mL of the original solution. We’ll walk through the dilution formula and calculate the new concentration step by step.", "---", "### Understanding the Initial Concentration", "The scientist begins with a 0.5 M (molar) solution, meaning there are 0.5 moles of solute dissolved in every liter of solution. Initially, she uses 300 mL (which equals 0.3 L) of this solution. The amount of solute remains constant during dilution—only the total volume changes.", "---", "### Applying the Dilution Formula", "To find the new concentration after dilution, scientists use the fundamental dilution equation:", "[\nC_1 \ imes V_1 = C_2 \ imes V_2\n]", "Where:\n- ( C_1 ) = initial concentration = 0.5 M\n- ( V_1 ) = initial volume = 0.3 L\n- ( C_2 ) = final concentration (what we want to find)\n- ( V_2 ) = final volume after dilution = 300 mL + 200 mL = 500 mL = 0.5 L", "---", "### Step-by-Step Calculation", "1. Plug values into the formula:", "[\n0.5, \ ext{M} \ imes 0.3, \ ext{L} = C_2 \ imes 0.5, \ ext{L}\n]", "2. Calculate left-hand side:", "[\n0.15, \ ext{mol} = C_2 \ imes 0.5, \ ext{L}\n]", "3. Solve for ( C_2 ):", "[\nC_2 = \frac{0.15, \ ext{mol}}{0.5, \ ext{L}} = 0.3, \ ext{M}\n]", "---", "### Final Result", "After adding 200 mL of water to 300 mL of a 0.5 M solution, the new concentration is 0.3 M. This means dilution by volume change increases the volume while reducing solute concentration proportionally, as predicted by the dilution law.", "---", "### Why This Matters in Real Science", "Accurate concentration adjustments are critical in experiments like titrations, enzyme assays, and biochemical analyses. Understanding dilution ensures precise control over reactant ratios, avoiding errors in data and reproducibility issues.", "---", "### Summary", "- Starting concentration: 0.5 M\n- Volume used: 300 mL (0.3 L)\n- Volume of water added: 200 mL (0.2 L)\n- Total volume after dilution: 500 mL (0.5 L)\n- New concentration: 0.3 M", "By applying basic chemistry principles, scientists reliably change solution concentrations—an essential skill in any laboratory setting.", "---", "Keywords: Dilution calculation, concentration formula, Molarity, solution dilution, chemistry lab, scientist calculation, 0.5 M solution, water dilution, molarity simplification."]
