Suppose 22.5 nickel(II) iodide is dissolved in 250 mL of a 0.50 M aqueous solution of...
Suppose 22.5 nickel(II) iodide is dissolved in 250 mL of a 0.50 M aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the nickel(II) iodide is dissolved in it.
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Suppose 22.5 nickel(II) iodide is dissolved in 250 mL of a 0.50
M aqueous solution of...
Suppose 15.2 g of nickel(II) iodide is dissolved in 200. mL of a 0.50 M aqueous solution of potassium carbonate.
Suppose 15.2 g of nickel(II) iodide is dissolved in 200. mL of a 0.50 M aqueous solution of potassium carbonate. Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) iodide is dissolved in it. Be sure your answer has the correct number of significant digits.
Suppose 16.6g of nickel(II) iodide is dissolved in 250.mL of a 0.80M aqueous solution of potassium...
Suppose 16.6g of nickel(II) iodide is dissolved in 250.mL of a 0.80M aqueous solution of potassium carbonate. Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) iodide is dissolved in it. Be sure your answer has the correct number of significant digits.
Suppose 3.63g of nickel(II) iodide is dissolved in 350.mL of a 75.0mM aqueous solution of potassium...
Suppose 3.63g of nickel(II) iodide is dissolved in 350.mL of a 75.0mM aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the nickel(II) iodide is dissolved in it. Be sure your answer has the correct number of significant digits. (M)
Suppose 3.81g of nickel(II) chloride is dissolved in 250.mL of a 69.0m M aqueous solution of...
Suppose 3.81g of nickel(II) chloride is dissolved in 250.mL of a 69.0m M aqueous solution of potassium carbonate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the nickel(II) chloride is dissolved in it. Round your answer to 3 significant digits.
Suppose 0.522g of zinc iodide is dissolved in 100.mL of a 63.0mM aqueous solution of potassium...
Suppose 0.522g of zinc iodide is dissolved in 100.mL of a 63.0mM aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it. Round your answer to 3 significant digits.
Suppose 0.509 g of nickel(II) chloride is dissolved in 100. mL of a 23.0 mM aqueous...
Suppose 0.509 g of nickel(II) chloride is dissolved in 100. mL of a 23.0 mM aqueous solution of potassium carbonate. Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits. (M)
Suppose 29.0 g of zinc iodide is dissolved in 250 mL of a 0.60 Maqueous solution...
Suppose 29.0 g of zinc iodide is dissolved in 250 mL of a 0.60 Maqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it. Be sure your answek has the correct number of significant digits. X 5 ?
Suppose 0.591 g of zinc iodide is dissolved in 50. mL of a 57.0 m M...
Suppose 0.591 g of zinc iodide is dissolved in 50. mL of a 57.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it Round your answer to 2 significant digits. M M10 ? X
Suppose 0.232 g of nickel(II) bromide is dissolved in 50. mL of a 24.0 m M...
Suppose 0.232 g of nickel(II) bromide is dissolved in 50. mL of a 24.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) bromide is dissolved in it. Be sure your answer has the correct number of significant digits. | Ом x 6 ?
Suppose 1.38g of potassium iodide is dissolved in 300.mL of a 18.0mM aqueous solution of silver nitrate. Calculate the f...
Suppose 1.38g of potassium iodide is dissolved in 300.mL of a 18.0mM aqueous solution of silver nitrate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the potassium iodide is dissolved in it. Round your answer to 3 significant digits.
Suppose 29.0 g of zinc iodide is dissolved in 250 mL of a 0.60 Maqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it. Be sure your answek has the correct number of significant digits. X 5 ?
Suppose 0.591 g of zinc iodide is dissolved in 50. mL of a 57.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it Round your answer to 2 significant digits. M M10 ? X
Suppose 0.232 g of nickel(II) bromide is dissolved in 50. mL of a 24.0 m M aqueous solution of potassium carbonate. Calculate the final molarity of nickel(II) cation in the solution. You can assume the volume of the solution doesn't change when the nickel(II) bromide is dissolved in it. Be sure your answer has the correct number of significant digits. | Ом x 6 ?
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