Question #114575
a 1.0g sample of a mixture which contains only NaCl and KCl have a precipitate of AgCl which weighed 2.0 g. what are the percentage of Na and K in the mixture?
1
Expert's answer
2020-05-08T14:12:02-0400

Solution.

n(AgCl)=mM=2.0143.32=0.014 moln(AgCl) = \frac{m}{M} = \frac{2.0}{143.32} = 0.014 \ mol

Cl+Ag+=AgClCl^- + Ag^+ = AgCl

x = n(NaCl)

y = n(KCl)

1)x+y=0.0141) x + y = 0.014

2)58.44×x+74.55×y=1.02) 58.44 \times x + 74.55 \times y = 1.0

x = n(NaCl) = 0.003 mol

y = n(KCl) = 0.011 mol

m(NaCl)=n(NaCl)×M(NaCl)=0.180 gm(NaCl) = n(NaCl) \times M(NaCl) = 0.180 \ g

m(KCl)=n(KCl)×M(KCl)=0.820 gm(KCl) = n(KCl) \times M(KCl) = 0.820 \ g

w(NaCl)=18%w(NaCl) = 18 \%

w(KCl)=82%w(KCl) = 82 \%

m(Na)=m(NaCl)×w(Na in NaCl)100%m(Na) = \frac{m(NaCl) \times w(Na \ in \ NaCl)}{100 \%}

m(K)=m(KCl)×w(K in KCl)100%m(K) = \frac{m(KCl) \times w(K \ in \ KCl)}{100 \%}

m(Na) = 0.071 g

m(K) = 0.430 g

w(Na in mix)=m(Na)m(mix.)=7.10%w(Na \ in \ mix) = \frac{m(Na)}{m(mix.)} = 7.10 \%

w(K in mix)=m(K)m(mix.)=43.00%w(K \ in \ mix) = \frac{m(K)}{m(mix.)} = 43.00 \%

Answer:

w(Na in mix) = 7.10 %

w(K in mix) = 43.00 %


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