A sample of a tin ore weighing 0.2407 g was dissolved in an acid solution and al
ID: 722040 • Letter: A
Question
A sample of a tin ore weighing 0.2407 g was dissolved in an acid solution and all the tin in the sample was changed to tin(II). In a titration, 8.75 mL of 0.0428 M KMnO4 solution was required to oxidize the tin(II) to tin(IV).(a) What is the balanced net ionic equation for the reaction in the titration?
(b) How many grams of tin were in the sample?
(c) What was the percentage by mass of tin in the sample?
(d) If the tin in the sample had been present in the compound SnO2, what would have been the percentage by mass of SnO2 in the sample?
Explanation / Answer
the balanced net ionic equation for the reaction in the titration 5