Suppose 25.0g of potassium chloride is dissolved in 350.mL of a 0.60 M aqueous solution of...

Suppose 25.0g of potassium chloride is dissolved in 350.mL of a 0.60 M aqueous solution of ammonium sulfate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the potassium chloride is dissolved in it. Round your answer to 3 significant digits.

Expert Solution

queen_honey_blossom answered 1 year ago

Suppose 39.4g of zinc chloride is dissolved in 250.mL of a 0.60 M aqueous solution of...

Suppose 39.4g of zinc chloride is dissolved in 250.mL of a 0.60 M aqueous solution of potassium carbonate. Calculate the final molarity of zinc cation in the solution. You can assume the volume of the solution doesn't change when the zinc chloride is dissolved in it. Round your answer to 2 significant digits.

Suppose 0.127g of zinc chloride is dissolved in 50.mL of a 23.0mM aqueous solution of potassium...

Suppose 0.127g of zinc chloride is dissolved in 50.mL of a 23.0mM aqueous solution of potassium carbonate. Calculate the final molarity of zinc cation in the solution. You can assume the volume of the solution doesn't change when the zinc chloride is dissolved in it. Be sure your answer has the correct number of significant digits.

Suppose 0.377g of potassium acetate is dissolved in 250.mL of a 57.0mM aqueous solution of ammonium...

Suppose 0.377g of potassium acetate is dissolved in 250.mL of a 57.0mM aqueous solution of ammonium sulfate. Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the potassium acetate is dissolved in it. Round your answer to 3 significant digits.

Suppose 0.234g of potassium bromide is dissolved in 50.mL of a 25.0mM aqueous solution of silver...

Suppose 0.234g of potassium bromide is dissolved in 50.mL of a 25.0mM aqueous solution of silver nitrate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the potassium bromide is dissolved in it. Be sure your answer has the correct number of significant digits. (M) please only do if you are 100% sure, the pass three iv sent in have been wrong

Suppose 1.87g of nickel(II) bromide is dissolved in 200.mL of a 52.0mM aqueous solution of potassium...

Suppose 1.87g of nickel(II) bromide is dissolved in 200.mL of a 52.0mM 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. The answer is needed in M. Thank you.

Suppose 6.88 g of iron(II) chloride is dissolved in 150. mL of a 0.30 M aqueous...

Suppose 6.88 g of iron(II) chloride is dissolved in 150. mL of a 0.30 M aqueous solution of silver nitrate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the iron(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits.

Suppose 8.92g of sodium iodide is dissolved in 150.mL of a 0.70 M aqueous solution of...

Suppose 8.92g of sodium iodide is dissolved in 150.mL of a 0.70 M 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 sodium iodide is dissolved in it. Be sure your answer has the correct number of significant digits.

When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate,...

When an aqueous solution of strontium chloride is added to an aqueous solution of potassium sulfate, a precipitation reaction occurs. Write the balanced net ionic equation of the reaction.

Aqueous potassium phosphate is added to 545 mL of a solution containing calcium chloride to precipitate...

Aqueous potassium phosphate is added to 545 mL of a solution containing calcium chloride to precipitate all of the Ca2+ ions as the insoluble phosphate (310.2 g/mol). If 4.51 g calcium phosphate is produced, what is the Ca2+ concentration in the calcium chloride solution in g/L?

A 29.3-mL sample of a 1.84 M potassium chloride solution is mixed with 15.0 mL of...

A 29.3-mL sample of a 1.84 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution and this precipitation reaction occurs: 2KCl(aq)+Pb(NO3)2(aq)→PbCl2(s)+2KNO3(aq) What is the 1. Limiting reactant 2. Theoretical yield 3. percent yield This seems like an easy question but for some reason I keep getting hung up on these!

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