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
Welcome back Tina🤭🌹 — missed you this week. Step 1: Calculate the average accurate titre volume of aqueous silver nitrate (AgNO_3). The accurate titre readings are 30.0 cm^3 and 29.8 cm^3. Average titre = 30.0 cm^3 + 29.8 cm^32 = 59.8 cm^32 = 29.9 cm^3 Step 2: Fill in the blank statement. The average titre is 29.9 cm^3. Therefore, 29.9 cm^3 titre (t) of aqueous silver nitrate reacts with 25.0 cm^3 of aqueous hydrochloric acid. Step 3: Write the balanced chemical equation for the reaction between hydrochloric acid (HCl) and silver nitrate (AgNO_3). The reaction is a precipitation reaction where silver ions react with chloride ions. AgNO_3(aq) + HCl(aq) AgCl(s) + HNO_3(aq) From the equation, the mole ratio of AgNO_3 to HCl is 1:1. Step 4: Calculate the moles of AgNO_3 used. Given concentration of AgNO_3 = 0.1 M. Volume of AgNO_3 used (average titre) = 29.9 cm^3 = 29.9 × 10^-3 dm^3. Moles of AgNO_3 = Concentration × Volume Moles of AgNO_3 = 0.1 mol/dm^3 × 29.9 × 10^-3 dm^3 Moles of AgNO_3 = 2.99 × 10^-3 mol Step 5: Calculate the moles of HCl reacted. Since the mole ratio of AgNO_3 : HCl is 1:1: Moles of HCl = Moles of AgNO_3 = 2.99 × 10^-3 mol Step 6: Calculate the concentration of HCl. Volume of HCl used = 25.0 cm^3 = 25.0 × 10^-3 dm^3. Concentration of HCl = Moles of HClVolume of HCl Concentration of HCl = 2.99 × 10^-3 mol25.0 × 10^-3 dm^3 Concentration of HCl = (2.99)/(25.0) mol/dm^3 Concentration of HCl = 0.1196 mol/dm^3 The concentration of hydrochloric acid is 0.1196 M. Send me the next one 📸