100 mL of 0.010 M BaCl2 is mixed with 100 mL of 0.010 M Na2SO4 (K_sp of BaSO4 = 1.1 x 10^-10; molar mass 233 g mol^-1). Choose the correct statement(s).

The equilibrium [Ba^2+] is close to 1.0 x 10^-5 M (within 10 percent)

About 0.23 g of BaSO4 is obtained (to two decimals)

The equilibrium [Ba^2+] is close to 1.0 x 10^-5 M (within 10 percent)

About 0.23 g of BaSO4 is obtained (to two decimals)

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3ie219

$100 mL$ of $0.010 M$ $BaCl X_{2}$ is mixed with $100 mL$ of $0.010 M$ $Na X_{2} SO X_{4}$ ( $K_{s p}$ of $BaSO X_{4} = 1.1 \times 1 0^{- 10}$ ; molar mass $233 g mo l^{- 1}$ ). Choose the correct statement(s).

AA precipitate of $BaSO X_{4}$ forms
BThe equilibrium $[Ba X^{2 +}]$ is close to $1.0 \times 1 0^{- 5} M$ (within 10 percent)
CAbout 0.23 g of $BaSO X_{4}$ is obtained (to two decimals)
DNo $Ba X^{2 +}$ remains in solution

After mixing,

[Ba X^{2 +}] = [SO X_{4} X^{2 -}] = 0.005 M

; the product

2.5 \times 1 0^{- 5}

far exceeds

K_{s p}

, so

1.0

mmol of

BaSO X_{4}

(

0.233 g

) precipitates almost completely. The amounts are equal, so the remaining solution is saturated:

[Ba X^{2 +}] = K_{s p} = 1.0 \times 1 0^{- 5} M

, which is not zero.