I have a question regarding solution for problem 143 chapter 3from McMurry Fay Chemistry sixth edition text book. In step 2/4there is a section where the solution divides (98 * .353)/80 Iunderstand that 98 is the grams of H2SO4 per mole and .353 is thegrams of NaOH used to neautrilize H2SO4, but I dont understandwhere the 80 comes from. Can you please exaplain where they 80comes from. The question in case you cant access the specific sixthedition text book is:
A 1.268 g sample of a metal carbonate (MCO3) was treated with100.00 mL of .1083 M sulfuric acid (H2SO4), yielding CO2 gas and anaqueous solution of the metal sulfate (MS)4). The solution wasbioled to remove all the disolved CO2 and was then titrated with.1241 M NaOH. A 71.02 mL volume of NaOH was required to neutralizethe excess H2SO4. (a) what is the identiy of the metal M? (b) howmany liters of CO2 gas were produced if the density of CO2 is 1.799g/L?
I have a question regarding solution for problem 143 chapter 3from McMurry Fay Chemistry sixth edition text book. In step 2/4there is a section where the solution divides (98 * .353)/80 Iunderstand that 98 is the grams of H2SO4 per mole and .353 is thegrams of NaOH used to neautrilize H2SO4, but I dont understandwhere the 80 comes from. Can you please exaplain where they 80comes from. The question in case you cant access the specific sixthedition text book is:
A 1.268 g sample of a metal carbonate (MCO3) was treated with100.00 mL of .1083 M sulfuric acid (H2SO4), yielding CO2 gas and anaqueous solution of the metal sulfate (MS)4). The solution wasbioled to remove all the disolved CO2 and was then titrated with.1241 M NaOH. A 71.02 mL volume of NaOH was required to neutralizethe excess H2SO4. (a) what is the identiy of the metal M? (b) howmany liters of CO2 gas were produced if the density of CO2 is 1.799g/L?
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