Question

Consider the titration involving the equation: Ba(OH)2 + 2HNO3 -> Ba(NO3)2 + 2H 20 The equivalent point is reached when 19.65 mLof 0.200 M HNO 3 is titrated into 25.00 mL of the Ba(OH)2. Calculate the molarity of BalOH) 2. a. 0.0935 M b. 0.0894 M c. 0.0786 M d. 0.0900 M

Answer 1

Acid for is and bose combine salt and water. called Neutralisation togeener to a This reaction reaction, BacoH)2 + 2HNOz BalN03)2 + 2H2O. Imole of BacOH)2 reacts wille zuole ot HNO2 to form limole of Ba(NO) and a mole of H₂O. 19165 ml ct 0.200 M HNO3 solution = Molarity of no afmoles of soleite vollerne af solutiaine as Molarity & Lolerue inc no of moles of HNO3 = : 0-200 made s9o* = 0.00 393 mole. 25.00 mL of BacoHl. Let the Molarity Balottla be: X M, no at moles at Ba(OH)2 = 8 (25) mole of → Imole of Bacolth 2 mole of HNO3 I required, 0.00393 mole at HNO3 → ?? no of moles of Bacota resuired 2 0.00393 x 1

This is equal to 25x 1000 25 X a (000 = 0.00 393 > 50 x = 0.00393 X 1000 x X x= 3-93 50 0.0786 D ri Molarity at Balohl= 0.0186 m option © correct -