The amount of ${BaSO}_4$ formed upon mixing $100 {~mL}$ of $20.8 \% \,{BaCl}_2$ solution with $50 {~mL}$ of $9.8 \% {H}_2 {SO}_4$ solution with $50 {~mL}$ of $9.8 \%\,$ ${H}_2 {SO}_4$ solution will be: $ ({Ba}=137, {Cl}=35.5, {~S}=32, {H}=1 \text { and } {O}=16 \text { ) } $

JEE CHEMISTRY MCQ: SOME BASIC CONCEPTS OF CHEMISTRY

1 Hard

1 of 1

Application +4 | -1

The amount of

{BaSO}_4

formed upon mixing

100 {~mL}

20.8 \% \,{BaCl}_2

solution with

50 {~mL}

9.8 \% {H}_2 {SO}_4

solution with

50 {~mL}

9.8 \%\,

{H}_2 {SO}_4

solution will be:

({Ba}=137, {Cl}=35.5, {~S}=32, {H}=1 \text { and } {O}=16 \text { ) }

View answer and explanation

Correct option: A

23.3 {~g}

Option A (

23.3 {~g}

) is correct because it is the mass of

{BaSO}_4

formed based on the stoichiometry of the reaction between

{BaCl}_2

and

{H}_2 {SO}_4