Exactly 0.2220 g of pure Na2CO3 was dissolved in 100.0 mL of 0.0731 M HCl.   (a) What mass in grams of CO2 was evolved?   (b) What was the molar concentration of the excess reactant (HCl or Na2CO3)?

Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom. oxidation state of highlighted atom species Na (aq) H30"(aq) co? (aq) Cl,(9)

How many grams of Ni(OH)2Ni(OH)2 are produced from the reaction of 27.0 mLmL of a 1.95  M NaOH M NaOH solution and excess NiCl2NiCl2?

3. A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO2 produced was collected in 3% H₂O₂. Reaction: SO2(g) + H₂O2 → H₂SO4. A 25.00-mL portion of 0.00873 M NaOH was introduced into the solution of H₂SO4, following which the excess base was back-titrated with 15.17 mL of 0.01102 M HCI. Calculate the sulfur concentration in the sample in parts per million.

A 9.835-gram sample of cobalt(II) chloride hexahydrate (CoCl2•6H2O; molar mass = 237.9 g/mol) is dissolved in 150.0 mL of solution. What is the molarity of CoCl2 in the solution? (A) 0.04134 M (B) 0.06557 M (C) 0.2756 M (D) 2.756 x 10–4 M

50.0 mL of a 0.4230 M solution of Na3PO, was mixed with 100.0 mL of 0.5151 M HgNO3 and allowed to react: Na3PO4 (aq) + HgNO3(aq) → 3 NaNO3(aq) + Hg3PO4 (s) - Answer the following questions: What mass of precipitate was formed? What is the molarity of the unreacted reactant after the reaction is complete? Check 9 M

3. Assume that 2.1429 g of Cr(NO3)3 is dissolved in enough water to make 50.00 mL of solution. (a) What is the molarity of Cr(NO3)3? (b) What is the molarity of the chromium(III) cation? (c) What is the molarity of the nitrate anion? The molar mass of Cr(NO3)3 is 238.011 g/mol.

1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? | c) Which of the reactants is the limiting reagent? Justify your answer. d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction? f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?

Suppose that a solution prepared by dissolving 0.554 g of MgCl2 in about 30 mL of water is mixed with a solution that contains excess K2CO3 dissolved in about 30 mL of water.   What is the theoretical yield (in grams) of MgCO3 in the precipitation reaction that occurs?

when 100.0 mL of a 2.00 M solution of KOH(aq) is added to 100.0 mL of a 2.00 M solution of Mg(NO3)2 what is the mass of the precipitate(s) that form?