Ksp for BaSO4 at 25^° C is 1.1 × 10^{-10}. To make the new solubility equal to 1.1 × 10^{-8}, it is necessary to use the solution of Na2SO4 of what concentration? Show detailed solution

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Q. Find the solubility of a sparingly soluble salt,

B a S O_{4}

0.02 M

N a_{2} S O_{4}

solution ?

(K_{s p}

for

B a S O_{4} = 1.1 \times 10^{- 10})

Q. Calculate the solubility of a sparingly soluble salt,

B a S O_{4}

0.01 M

N a_{2} S O_{4}

solution ?

(K_{s p}

for

B a S O_{4} = 1.1 \times 10^{- 10})

Q. An aqueous solution contains an unknown concentration of

B a^{2 +}

. When 50 mL of 1 M solution of

N a_{2} S O_{4}

is added,

B a S O_{4}

just begins to precipitate. The final volume is 500 mL. The solubility product of

B a S O_{4}

1 \times 10^{- 10}

. What is the original concentration of

B a^{2 +}

The solubility product of $B a S O_{4}$ at $25^{\circ} C$ is $1.0 \times 10^{- 9}$ . What would be

the concentration of $H_{2} S O_{4}$ necessary to precipitate $B a S O_{4}$ from a solution

of $0.01 M$ $B a^{2 +}$ ions ?

The $K_{s p}$ of $A g_{2} C r O_{4}$ is $1.1 \times 10^{- 12}$ at 298K. The solubility (in mol/L) of $A g_{2} C r O_{4}$ in 0.1M $A g N O_{3}$ solution is:

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