염화바륨 시약의 순도 계산. 4.36 g barium chloride

염화바륨 시약의 순도 계산. 4.36 g barium chloride

 

 

An impure sample of barium chloride with a mass of 4.36 g is added to an aqueous solution of sodium sulfate. After the reaction is complete, the precipitate is filtered and dried. Its mass is found to be 2.62 g. What is the percentage purity of the original barium chloride?

 

 

An impure sample of barium chloride with a mass of 4.36 g is added to an aqueous solution of sodium sulfate. After the reaction is complete, the mass of the solid barium sulfate is found to be 2.62 g. What is the percentage purity of the original barium chloride?

BaCl2(s) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)

 

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BaCl2(aq) + Na2SO4(aq) → BaSO4(s) + 2NaCl(aq)

 

 

BaSO4의 몰질량 = 233.39 g/mol 이므로,

2.62 g / (233.39 g/mol) = 0.0112 mol BaSO4

( 계산 참고 https://ywpop.tistory.com/7738 )

 

 

BaCl2 : BaSO4 = 1 : 1 계수비(= 몰수비) 이므로,

반응한 BaCl2의 몰수 = 0.0112 mol

 

 

BaCl2의 몰질량 = 208.23 g/mol 이므로,

0.0112 mol BaCl2의 질량을 계산하면,

0.0112 mol × (208.23 g/mol) = 2.33 g BaCl2

 

 

BaCl2의 순도를 계산하면,

(2.33 g / 4.36 g) × 100 = 53.4%

 

 

 

[참고] 한 번에 계산하면,

[(2.62 / 233.39 × 208.23) / 4.36] × 100 = 53.6%

 

 

 

[키워드] BaCl2 + Na2SO4 + BaCl2, BaSO4 침전 기준문서