What is the molarity of a solution made by dissolving 37.2 g Fe(NO3)3 in enough water to make 200.0 mL of solution? How many grams of Fe(NO3)3

A 2.85 g sample of NaCl and CaCl2 was dissolved in water, and an excess of AgNO3 was added to precipitate all of the chloride ions.The AgCl was collected and dried, and weighed to give 7.20 g of AgCl. How much NaCl and CaCl2 was in the sample? i g NaCl g CaCl2

What volume in liters of a 7.5 M Fe(NO3)3 solution can be diluted to prepare 201.2 mL of a solution with a concentration of 3.1 M?

Water "softeners" remove metal ions such as Ca2+ and Fe3+ by replacing them with enough Na+ ions to maintain the same number of positive charges in the solution. If  7.33  ×  102 L  of "hard" water is 0.0766 M Ca2+ and 0.00462 M Fe3+, how many moles of Na+ are needed to replace these ions?

-3 What is the mass of solute, in grams, in 100. mL of a 1.263 × 10-³ M solution of Na3PO4? Mass of solute = g 3- What are the molar concentrations of the Na+ and PO4³- ions? Molar concentration Na+ 3- Molar concentration PO4³ = = M M

40.00 mL of a solution of MgCl2 with a molar volume concentration of 0.933 mol/L is mixed with 100.0 mL of a solution of AlCl3 with a molar volume concentration of 0.211 mol/L.  What is the final molar volume concentration of chloride ions (Cl-) in the mixture in mol/L? Note: The density of pure water is 1.000 g/mL.

A.) If 11.3 g of KBr (MM = 119.00 g/mol) are added to a 500.0 mL volumetric flask, and water is added to fill the flask, what is the concentration of KBr in the resulting solution? B) If 25.0 mL of a 7.90 M HCl solution is diluted to 2.00 L, what is the molarity of the new solution? C) What quantity in moles of KBr are there in 225.0 mL of 0.155 M KBr?

1.) What mass of NaCl (in g) is necessary for 5.25 L of a 1.25 M solution? 2.) You have measured out 75.00 g of MgCl2 (formula weight: 58.33 g/mol) to make a solution.  What must your final volume be (in L) if you want a solution made from this mass of MgCl2 to have concentration of 0.175 M? 3.) You have a concentrated solution  of 5.00 M NaOH.  If you dilute 365.2 mL of this solution with water to a final volume of 2.00 L, what is the molarity of the diluted solution? 4.) What volume (in mL) of 5.00 M HCl must diluted to a final volume of 1.50 L to make a solution with a final concentration of 0.470 M?

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC8H4O4. This is often written in shorthand notation as KHP. How many grams of KHP are needed to exactly neutralize 20.5 mL of a 0.381 M barium hydroxide solution? Mass = grams KHC, H4O4

In the reaction below, how many grams of chlorine gas (Cl₂) are needed to react with 5.393 x 1023 molecules of sodium hydroxide? Cl₂(g) + NaOH(aq) → NaCl(aq) + NaClO3(aq) + H₂O(l) What volume (in L) of 0.125 mol/L Ba(OH)2 solution is needed to react completely with 0.200 L of a 0.300 mol/L HNO3 solution according to the following reaction: Ba(OH)2(aq) + HNO3(aq) → Ba(NO3)2(aq) + H₂O(l) ->>