Answer :
Mass of AgBr is formed when 35.5 ml of 0.184 m agno3 is treated with an excess of aqueous hydrobromic acid is 1.23g.
What is Stoichiometric?
We may calculate reactant and product amounts using balanced chemical equations thanks to the fundamental concept of stoichiometry. The balanced equation's ratios are used in this instance. Generally speaking, how a reaction will behave depends on the amount of substance present.
Equation formed:
AgNO₃(aq) + HBr(aq) ⇒ AgBr(s) + HNO₃(aq)
Calculate the amount of AgNO3 consumed throughout the reaction.
based on molarity (a 1000 ml solution of AgNO3 comprises 0.184 moles).
AgNO₃ moles in 35.5 ml solution = [tex]\frac{(0.184mol) . (35.5ml)}{1000ml}[/tex]
∴ Moles of AgNO₃ = 0.006532 moles
Moles of AgBr formed by 0.006532 moles of AgNO₃
From balanced reaction eq.,
Moles ratio of AgNO₃ : AgBr = 1 : 1 (AgNO₃ = AgBr)
∴ Moles of AgBr = 0.006532 moles
Mass of 0.006532 moles of AgBr,
Molar mass of AgBr = 187.77g/ml
∵ Mass (AgBr) = 187.77 × 0.006532
Mass of AgBr = 1.23g
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