What is the iron(II) ion concentration in a solution prepared by mixing 329 mL of 0.411M iron(II) nitrate with 421 mL of 0.249 M sodium hydroxide? The Kg of iron(II) hydroxide is 4.87 x 10 17. [Fe²*] = M

A student weighs out a 11.1 g sample of CuSO4, transfers it to a 500. mL volumetric flask, adds enough water to dissolve it and then adds water to the 500. mL tick mark. What is the molarity of copper(II) sulfate in the resulting solution? Molarity = M

A 30.00-mL volume of aqueous sulfuric acid, H2SO4, is titrated using 0.200 M NaOH and an indicator that turns color only after all the sulfuric acid protons have reacted with OH- ions. The solution turns color when 48.32 mL of base has been added. What is the molar concentration of the sulfuric acid?

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 2.50 g sample of KCl is dissolved in 17.0 mL of water. The resulting solution is then added to 79.0 mL of a 0.150 M CaCl2 (aq) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K+ ions М Concentration of Ca+ ions = M

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It had the unwieldy formula of KHC8H4O4 . This is offen written in shorthand notation of KHP. How many grams of KHP are needed to exactly neutralize 21.0 mL of a 0.197 M barium hydroxide solution?

A mixture of bases can sometimes be the active ingredientin antacid tablets. If 0.4826 g of a mixture of Al(OH)₃ and Mg(OH)₂ is neutralized with 17.30 mL of 1.000 MHNO₃, what is the mass % of Al(OH)₃ in the mixture?

Phosphoric acid, H3PO4, in a solution was neutralized by titration with a barium hydroxide,  Ba(OH)2 solution. If 16.2 mL of phosphoric acid solution required 46.1 mL of 0.100 M Ba(OH)2 for neutralization, what was the molarity of the phosphoric acid in the original solution?

Acetylsalicylic acid (C₂H8O4) is a monoprotic acid commonly known as aspirin. A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took 5.10 mL of 0.1466 M NaOH to neutralize the solution. Calculate the number of grains of aspirin in the tablet. (One grain = 0.0648 g and the molar mass of aspirin = 180.15.) mol Round your answer to 3 significant digits. grains ☐ ☐x10

A certain rust remover containing phosphoric acid has a density of 1.685 g/mL. Titration of a 59.3 mL sample of the rust remover requires 640 mL of 1.86 M NaOH to completely react with the acid to form sodium phosphate. What is the mass percent H3PO4 (98.0 g/mol) in the rust remover? Oa, 19.8% Ob. 14.6% Oc. 69.7% Od.85.1% Oe. 39.1%