Indium (atomic weight = 114.82) has two naturally occurring isotopes, the predominant one form has isotopic weight 114.9041 and abundance of 95.72%. Which of the following isotopic weights is the most likely for the other isotope?

112.94

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115.9

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113.9

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114.9

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Solution

The correct option is A 112.94
Solution:- (A) $112.94 g$
Abundance of first isotope $= 95.72 %$
Abundance of other isotope $= 100 - 95.72 = 4.28 %$
Let $x$ be the mass other isotope.
Therefore,
$(114.9041 \times 0.9572) + (x \times 0.0428) = 114.82$
$\Rightarrow x = \frac{114.82 - 109.986}{0.0428} = 112.94 g$
Hence the mass of other isotope is $112.94 g$ .

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Indium (atomic weight = 114.82) has two naturally occurring isotopes, the predominant one form has isotopic weight 114.9041 and abundance of 95.72%. Which of the following isotopic weights is the most likely for the other isotope?

The correct option is A 112.94Solution:- (A) 112.94gAbundance of first isotope =95.72%Abundance of other isotope =100−95.72=4.28%Let x be the mass other isotope.Therefore,(114.9041×0.9572)+(x×0.0428)=114.82⇒x=114.82−109.9860.0428=112.94gHence the mass of other isotope is 112.94g.