314918 A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution \(\left(\mathrm{Q}_{\mathrm{sp}}\right)\) becomes greater than its solubility product. If the solubility of \(\mathrm{BaSO}_{4}\) in water is \({\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 4}}}}{\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}\) Its solubility in 0.01 \({\text{mol d}}{{\text{m}}^{ - 3}}\) of \({{\text{H}}_2}{\text{S}}{{\text{O}}_4}\) in \({\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}{\text{?}}\)
314919
Specify if addition of the second substance in each of the following increases (i) or decreases (D),
the solubility of the first substance.
(I) \(\mathrm{Al}(\mathrm{OH})_{3}, \mathrm{NaOH}\)
(II) \(\mathrm{PbCl}_{2}, \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\)
(III) \(\mathrm{CuSO}_{4}, \mathrm{NH}_{3}\)
314921 Solubility product of a salt \({\text{AB}}\) is \({\text{1}} \times {\text{1}}{{\text{0}}^{{\text{ - 8}}}}{\text{ }}{{\text{M}}^{\text{2}}}\) in a solution in which the concentration of \(\mathrm{A}^{+}\)ions is \({10^{ - 3}}{\text{ M}}\). The salt will precipitate when the concentration of \(\mathrm{B}^{-}\) ions is kept
314918 A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution \(\left(\mathrm{Q}_{\mathrm{sp}}\right)\) becomes greater than its solubility product. If the solubility of \(\mathrm{BaSO}_{4}\) in water is \({\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 4}}}}{\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}\) Its solubility in 0.01 \({\text{mol d}}{{\text{m}}^{ - 3}}\) of \({{\text{H}}_2}{\text{S}}{{\text{O}}_4}\) in \({\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}{\text{?}}\)
314919
Specify if addition of the second substance in each of the following increases (i) or decreases (D),
the solubility of the first substance.
(I) \(\mathrm{Al}(\mathrm{OH})_{3}, \mathrm{NaOH}\)
(II) \(\mathrm{PbCl}_{2}, \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\)
(III) \(\mathrm{CuSO}_{4}, \mathrm{NH}_{3}\)
314921 Solubility product of a salt \({\text{AB}}\) is \({\text{1}} \times {\text{1}}{{\text{0}}^{{\text{ - 8}}}}{\text{ }}{{\text{M}}^{\text{2}}}\) in a solution in which the concentration of \(\mathrm{A}^{+}\)ions is \({10^{ - 3}}{\text{ M}}\). The salt will precipitate when the concentration of \(\mathrm{B}^{-}\) ions is kept
314918 A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution \(\left(\mathrm{Q}_{\mathrm{sp}}\right)\) becomes greater than its solubility product. If the solubility of \(\mathrm{BaSO}_{4}\) in water is \({\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 4}}}}{\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}\) Its solubility in 0.01 \({\text{mol d}}{{\text{m}}^{ - 3}}\) of \({{\text{H}}_2}{\text{S}}{{\text{O}}_4}\) in \({\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}{\text{?}}\)
314919
Specify if addition of the second substance in each of the following increases (i) or decreases (D),
the solubility of the first substance.
(I) \(\mathrm{Al}(\mathrm{OH})_{3}, \mathrm{NaOH}\)
(II) \(\mathrm{PbCl}_{2}, \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\)
(III) \(\mathrm{CuSO}_{4}, \mathrm{NH}_{3}\)
314921 Solubility product of a salt \({\text{AB}}\) is \({\text{1}} \times {\text{1}}{{\text{0}}^{{\text{ - 8}}}}{\text{ }}{{\text{M}}^{\text{2}}}\) in a solution in which the concentration of \(\mathrm{A}^{+}\)ions is \({10^{ - 3}}{\text{ M}}\). The salt will precipitate when the concentration of \(\mathrm{B}^{-}\) ions is kept
314918 A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution \(\left(\mathrm{Q}_{\mathrm{sp}}\right)\) becomes greater than its solubility product. If the solubility of \(\mathrm{BaSO}_{4}\) in water is \({\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 4}}}}{\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}\) Its solubility in 0.01 \({\text{mol d}}{{\text{m}}^{ - 3}}\) of \({{\text{H}}_2}{\text{S}}{{\text{O}}_4}\) in \({\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}{\text{?}}\)
314919
Specify if addition of the second substance in each of the following increases (i) or decreases (D),
the solubility of the first substance.
(I) \(\mathrm{Al}(\mathrm{OH})_{3}, \mathrm{NaOH}\)
(II) \(\mathrm{PbCl}_{2}, \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\)
(III) \(\mathrm{CuSO}_{4}, \mathrm{NH}_{3}\)
314921 Solubility product of a salt \({\text{AB}}\) is \({\text{1}} \times {\text{1}}{{\text{0}}^{{\text{ - 8}}}}{\text{ }}{{\text{M}}^{\text{2}}}\) in a solution in which the concentration of \(\mathrm{A}^{+}\)ions is \({10^{ - 3}}{\text{ M}}\). The salt will precipitate when the concentration of \(\mathrm{B}^{-}\) ions is kept
314918 A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution \(\left(\mathrm{Q}_{\mathrm{sp}}\right)\) becomes greater than its solubility product. If the solubility of \(\mathrm{BaSO}_{4}\) in water is \({\text{8}} \times {\text{1}}{{\text{0}}^{{\text{ - 4}}}}{\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}\) Its solubility in 0.01 \({\text{mol d}}{{\text{m}}^{ - 3}}\) of \({{\text{H}}_2}{\text{S}}{{\text{O}}_4}\) in \({\text{mol d}}{{\text{m}}^{{\text{ - 3}}}}{\text{?}}\)
314919
Specify if addition of the second substance in each of the following increases (i) or decreases (D),
the solubility of the first substance.
(I) \(\mathrm{Al}(\mathrm{OH})_{3}, \mathrm{NaOH}\)
(II) \(\mathrm{PbCl}_{2}, \mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\)
(III) \(\mathrm{CuSO}_{4}, \mathrm{NH}_{3}\)
314921 Solubility product of a salt \({\text{AB}}\) is \({\text{1}} \times {\text{1}}{{\text{0}}^{{\text{ - 8}}}}{\text{ }}{{\text{M}}^{\text{2}}}\) in a solution in which the concentration of \(\mathrm{A}^{+}\)ions is \({10^{ - 3}}{\text{ M}}\). The salt will precipitate when the concentration of \(\mathrm{B}^{-}\) ions is kept