What mass of NaCl is needed to precipitate all the silver ions from 20.0 mL of 0.100 M AgNO3 solution?

185 mL of 0.355 M NaCl is added to a 0.500 L volumetric flask and the flask is filled with water. Calculate the [Na⁺] concentration in the diluted solution.

How many moles of solute particles are present in 3.9 mL of 0.665 M (NH4)3PO4?

When 50.0 mL of a 0.3000 M AgNO3 solution is added to (4.65x10^1) mL of a solution of MgCl₂, an AgCl precipitate forms immediately. The precipitate is then filtered from the solution, dried, and weighed. If the recovered AgCl is found to have a mass of (1.2x10^-1) g. what was the concentration in molarity of chloride ions in the original MgCl₂ solution? 2AgNO3(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO3)2(aq) Use the correct number of significant figures and type in the unit abbreviation for the answer. Answer: 8.0x10^-1 M.

If a 10.0mL volumetric flask is used to prepare the dilution, what volume of 0.50 M cobalt (II) nitrate is needed to prepare a 0.15 M standard solution?

0.3456 g of a solid acid is dissolved in 50 mL of water in a flask  and a few drops of phenolphthalein are added to the solution.  A buret containing 0.2545 M NaOH is prepared with an initial volume of 10.50 mL.  The acid is accidentally titrated with the base beyond the end point, so 1.52 mL of 0.187 M HCl are added to the flask. The titration with the base is continued to a final volume reading of  40.55 mL.  Calculate the molar mass of the solid acid.

All the chloride in a 5.00 g sample of an unknown metal chloride is precipitated as AgCl with 70.9 mL of 0.2010 M AgNO3. What is the percentage of chloride in the sample?

Suppose 3.32g of nickel(II) iodide is dissolved in 50mL of a 0.40 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.

A researcher has a sample of potassium chloride that is contaminated with magnesium chloride. They weigh 5.00 g of the sample, dissolve it in 1.00 L of water, and determine the chloride ion concentration to be 0.0708 M. What mass (in g) of the 5.00 g sample was magnesium chloride?

A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 52.50 mL of 1.500 M NaCl, and the PbCl₂ precipitate is filtered from the solution. Then 200.0 mL of 3.000 M NaBr is added to the remaining solution, and the PbBr₂ precipitate is also collected and dried. What is the mass (in grams) of the PbBr₂ precipitate, assuming the yield in each precipitation step is 100%?