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【武大】三价铁、铋离子混合液中各组分含量的测定

【武大】三价铁、铋离子混合液中各组分含量的测定
【武大】三价铁、铋离子混合液中各组分含量的测定

Bi3+-Fe3+混合溶液各组分含量的测定

孙阳勇

(武汉大学化学与分子科学学院湖北武汉430072)

摘要:对于Bi3+和Fe3+与EDTA形成稳定络合物,它们的稳定常数分别为lgK

=27.94、lgK Fe

BiY

=25.1.由于Δlg K=2.84〈5,故不能直接用EDTA进行分部滴定,考虑到Fe2+与EDTA形(Ⅲ)Y

成的络合物的稳定常数为14.32,这时对于Bi3+和Fe2+与EDTA形成的络合物,有ΔlgK=13.62﹥5.故可考虑使用还原剂来还原Fe3+,从而可以滴定Bi3+的含量。实验时首先加入抗坏血酸还原Fe3+,以二甲酚橙为指示剂,在氨基乙酸-HCl缓冲体系中,以二甲酚橙为指示剂,用EDTA标准溶液滴定Bi3+的含量,之后加入六亚甲基四胺-HCl缓冲溶液,用EDTA标准溶液滴定Fe2+的含量,通过两次滴定可分别求出Bi3+与Fe3+的浓度。

关键词:Bi3+-Fe3+混合溶液二甲酚橙抗坏血酸氧化还原掩蔽法

引言:络合滴定又称为配位滴定,是以络合反应为基础的滴定分析法。络合反应也是路易斯酸碱反应(金属离子是路易斯酸,可接受路易斯碱所提供的未成键电子对而形成化学键),对于提高络合滴定选择性的途径有:络合掩蔽法、沉淀掩蔽法、氧化还原掩蔽法等。当某种价态的共存离子对滴定有干扰时,利用氧化还原反应改变干扰离子的价态以消除干扰的方法,称之为氧化还原掩蔽法。

试剂及仪器:纯锌片,乙二胺四乙酸二钠盐(Na

H2Y·2H2O,相对分子质量372.2)(AR),

2

2g/L二甲酚橙水溶液,抗坏血酸溶液,蒸馏水,50mL烧杯,六亚甲基四胺溶液,甘氨酸固体,200mL烧杯,25mL移液管,表面皿,250mL锥形瓶,聚乙烯塑料瓶,酸式滴定管,玻璃棒,250mL容量瓶(2个),电子天平

实验部分

1.实验原理:

1.1.当为单一离子测定时,由于lgK’

=lgK MY-lgαY(H)- lgαM(OH),在高酸度下,可忽略lgαM(OH),

MY

因此有lgαY(H)= lgK MY-lgK’MY,对于C M=0.01mol/L,当ΔpM’=±0.2,Et=±0.1%,有lg K’MY≥8,因此对于Fe3+的滴定有最高酸度为lgαY(H)=25.1-8=17.1时,对应pH=1.2,其最低酸度为Fe3+不水解时,有此时[OH-]=1.59*10-12 mol/L,那么此时pH=2.2,故滴定Fe3+时应该控制pH=1.2-2.2。同理对于滴定Bi3+时应该控制pH=0.7-4.53,滴定Fe2+时应该使pH=5.1-7.46,由于滴定时均是

在酸性条件下,故用二甲酚橙作指示剂,其作用范围pH﹤6,其中XO在pH>6.3时,它呈现红色;pH<6.3时,呈现黄色;pH=p K a=6.3时,呈现中间颜色,二甲酚橙与金属离子形成的配合物都是紫红色。但是Fe3+对XO有封闭作用,用抗坏血酸掩蔽Fe3+即可解决,此时为

Bi3+-Fe2+的混合液,最高酸度时为lgαY(H)=lgαY(Fe2+)=12.32,此时最高酸度为pH=2.4,最低酸度为Bi3+不水解时pH=4.53,那么在Bi3+-Fe2+混合液中滴定Bi3+使pH=2.4―4.53。

1.2.对于Bi3+和Fe3+与EDTA形成稳定络合物,它们的稳定常数分别为lgK

=27.94、lgK Fe

BiY

=25.1.当ΔpM’=±0.2,Et=±0.3%由于ΔlgK=2.84〈5,故不能直接用EDTA进行分部滴定,(Ⅲ)Y

但是可以用EDTA一次滴定出Bi3+和Fe3+的总量(但是要注意三价铁离子对指示剂的封闭作用,结果误差较大);利用抗坏血酸的还原性可将Fe3+还原成Fe2+,由于lgK Fe(Ⅱ)Y=14.32,此时对于Bi3+和Fe2+与EDTA形成的络合物,有ΔlgK=13.62﹥5,故可准确滴定Bi3+而Fe2+不干扰。对于Bi3+-Fe2+体系,当C(Bi3+)=0.01mol/L时,到达滴定终点时,有pBi ep=5.4,pBi sp=1/2*(p C Bi sp+lgK’BiY),而lgK’BiY =lgK BiY-lg(αY(H)+ αY(N)-1)-lgαBi=27.94-12.62-1.4=13.92,故有pBi sp=7.96,因此有ΔpBi=-2.56,那么有终点误差为Et=-0.04%,表示可以准确滴定。

1.3.维生素C(Vitamin C ,Ascorbic Acid)又叫L-抗坏血酸,具有较强的还原性,加热或在溶液中易氧化分解,在碱性条件下更易被氧化,为己糖衍生物,可还原三价铁离子。

2.实验步骤:

2.1.配制Zn2+标准溶液:在分析天平上准确称取0.15-0.25g基准锌片于干净的50mL烧杯中,加入6mL 6mol/L的HCl溶液,立即盖上表面皿,待完全溶解后用蒸馏水冲洗表面皿,之后转移至250mL容量瓶中,定容至250mL,摇匀,计算Zn2+标准溶液的浓度。

2.1.稀释混合液:用专用移液管移取混合液25.00mL于250mL容量瓶中,加入一定量的盐酸防止Bi3+的水解,之后加蒸馏水稀释至刻度,摇匀。

2.3.配制EDTA溶液:在微量天平上称取1.8-2.5g乙二胺四乙酸二钠盐于200mL烧杯中,加入蒸馏水溶解后倒入聚乙烯塑料瓶中,加水约至500mL,摇匀。

2.4.标定EDTA溶液:用移液管吸取25.00mL Zn2+标准溶液于锥形瓶中,加2滴2g/L 的二甲酚橙指示剂,之后滴加200g/L六亚甲基四胺至溶液呈现稳定的紫红色,再加入5mL六亚甲基四胺溶液,然后用EDTA溶液滴定至溶液由紫红色刚变成黄色,记下EDTA的体积。平行滴定三份,计算EDTA的浓度。

2.5.混合液中Bi3+浓度的测定:用移液管移取25.00mL混合溶液于锥形瓶中,加入5ml抗坏血酸溶液,摇匀后放置2分钟,再加入2滴XO指示剂,用氨基乙酸-HCl缓冲溶液调节溶液为紫红色。用上述EDTA标准溶液进行滴定,溶液由紫红色变为亮黄色且半分钟内不褪色即为终点,记录消耗EDTA溶液的体积,平行滴定三次。

2.5.混合液中Fe3+浓度的测定:向上述溶液中再加入2滴XO指示剂,加入约40mL 200g/L六亚甲基四胺至溶液呈现稳定的紫红色,用上述EDTA标准溶液进行滴定,溶液由紫红色变为亮黄色且半分钟内不褪色即为终点,记录消耗EDTA溶液的体积,平行滴定三次。结果与讨论:

实验称取基准锌片0.2464g,所得Zn2+标准溶液浓度为:0.01507 mol/L

表一: Zn2+标准溶液标定EDTA(XO作指示剂)

表二:EDTA滴定混合液中Bi3+浓度(XO作指示剂)

表三:EDTA滴定混合液中Fe3+的浓度(XO作指示剂)

实验时用EDTA滴定混合液中Bi3+和Fe3+的总浓度,所用EDTA为48.95mL,而滴定Bi3+浓度时用EDTA为20.95mL,因此滴定Fe3+的浓度用EDTA为28.00mL,造成测定Fe3+的测定有较大误差,原因就是三价铁离子对XO较强的封闭作用,使变色延后。而后由于实验条件受限,未有氨基乙酸-HCl缓冲溶液,取而代之的是在25mL混合液中加入抗坏血酸还原Fe3+,之后加入20.95mL EDTA与Bi3+络合后,再在六亚甲基四胺-HCl缓冲体系中滴定剩余的二价铁离子,使得实验衔接不上,因此滴定二价铁离子时相对偏差较大。

滴定Bi3+至滴定终点时,有pBi sp=1/2*(p C Bi sp+lgK’BiY),而lgK’BiY =lgK BiY-lg(αY(H)+ αY(N)-1)-lgαBi=27.94-12.50-1.4=14.04,那么有pBi sp=1/2*(2.32+14.04)=8.18,pBi ep=5.4,有ΔpBi=-2.78,那么有终点误差为Et=-0.07%,表示可以准确滴定。同理滴定Fe2+时终点误差较小。

结论:实验测得混合液中Bi3+浓度为:0.01038mol/L , Fe3+浓度为:0.01058mol/L,那么原瓶中Bi3+浓度为:0.1038mol/L , Fe3+浓度为:0.1058mol/L。

致谢:感谢分析实验指导老师谢敏,感谢分析实验预备室的老师。

参考文献:

[1]分析化学实验:第五版上册.武汉大学主编.北京:高等教育出版社,2012,124-125

[2]分析化学:第五版上册.武汉大学主编.北京:高等教育出版社,188-211

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