This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Hey, good to see you again. Step 1: Write the balanced chemical equation for the neutralization reaction. Sulfuric acid (H_2SO_4) is a diprotic acid, meaning it releases two H^+ ions. Sodium hydroxide (NaOH) is a monoprotic base, releasing one OH^- ion. H_2SO_4(aq) + 2NaOH(aq) Na_2SO_4(aq) + 2H_2O(l) From the balanced equation, 1 mole of H_2SO_4 reacts with 2 moles of NaOH. Step 2: List the given values. Concentration of acid (M_a) = 0.100 M Volume of acid (V_a) = 25.00 mL = 0.02500 L Volume of base (V_b) = 34.36 mL = 0.03436 L Concentration of base (M_b) = ? Step 3: Use the titration formula. At the equivalence point of a neutralization reaction, the moles of acid and base are related by their stoichiometric coefficients: (M_a V_a)/(n_a) = (M_b V_b)/(n_b) Where n_a is the stoichiometric coefficient of the acid (1 for H_2SO_4) and n_b is the stoichiometric coefficient of the base (2 for NaOH). Step 4: Substitute the values and solve for M_b. (0.100 M)(0.02500 L)1 = M_b (0.03436 L)2 0.002500 mol = M_b (0.03436 L)2 Multiply both sides by 2: 2 × 0.002500 mol = M_b (0.03436 L) 0.005000 mol = M_b (0.03436 L) Solve for M_b: M_b = 0.005000 mol0.03436 L M_b ≈ 0.1455179 M Step 5: Round to the correct number of significant figures. The concentration of the acid (0.100 M) has 3 significant figures. The volumes (25.00 mL and 34.36 mL) have 4 significant figures. The result should be rounded to 3 significant figures. M_b = 0.146 M The concentration of the base solution is 0.146 M. Send me the next one 📸