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* 10.111 moles H250, 13. 13.50ml of barium chloride solution is required to react completely with 9.50ml of a 0.200M silver nitrate solution. The unbalanced reaction is: BaCl2laq) + 2AgNO3(4) ► 2AgCl) + Ba(NO3)2(aq). What is the molarity of the barium chloride solution? (0.200 moles AgNO) 1 Rac 9 50y10malar Rac

Answer 1

13A:- Given a balanced reaction: Balta + 2 Ag Nos aq) → z Agu (g) + Ba(NOB) q 6a). It is the balanced quation. from the given Equation, we observe that mole of Balle Requires 2 moles of AgNO₃. a [1:2 Ratio. Given volume of barium chloride solution - 13.50mL = 0.01350 L Volume of silver nitrate solution = 9.50m2 = 0.00950 L Molarity of silver nitrate = 0.200M we know, Molarity = no. of moles Volume of solution () silver nitrate - Molarity of silverenitrate & * no of moles of volume of silver nitrate = (0.200 M) X(0.00950L) I B = 0.001916 woles Of Silve x nitrate from the given balanced reaction, and Ratio of moles of Bal to moles of AgNO3. og 0.001916 moles of AgNO3 required t(0.001916) moles of Bo С, 0.001916 moles of Agno, 0.000958 moles of Bach Then, Molarity of Ball, = no. of moles Molarity of Balla = = 0.000958 Volume (L) - - 0.01350 = 0.0709 Mail ('. Molarity of Balg = 0.0709 mol/L = 0.0709M]

& water 12A - Given Reaction: Potassium hydroxide & sulphuric acid potassium sulphate KOH + H₂ Sou Kęsou + H₂O. > Balancing the reaction, we get: 4 KOH + 2H₂SO4 - 2k₂ sou + 4H₂O. from the above reaction, we can observe that: koH requires & moles of H₂sou for complete 4 moles of reaction . 4 moles of KOH : q moles of He sou Given volume of KoH = 95.0mb = 0.025 L Malarity of KOH = 0.0525M. given molarity of H₂SO4 = 0.1lIM. →no. of moles of KOH - Molarity of KoH) x volume of KOH) = (0.0525 M) x (0.025L) 0.0013125 moles of KOH. no. of moles of Ho sou required = les of koH) (0.0013125) 20.00065625 moles of Hesoy > Volume of Hasou required no of Moles Molarity of H₂ sou solution 0.00065625 0-11 = 0.005912 Litre (OY) 5.912 mi 5.912 ml (or) 0.005912 litres of h₂sou is required.