Which reaction is an example of both a precipitation and a neutralization? (A) H3PO4(aq) + 3 KOH(aq) –→ K3PO4(aq) + 3 H2O(I) (B) FeC13(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCI(aq) (C) (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H20(1) (D) H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2 H2O(1) (E) 2 C(s) + 02(g) → 2 CO(g) (11) * All of the statements regarding redox reactions are true except (A) a reducing agent causes another substance to be reduced. (B) halogens usually behave as oxidizing agents because they readily gain electrons. (C) metal ions are produced when pure metals are oxidized. (D) when a substance is oxidized its charge (or oxidation number) decreases. (E) alkali metals often behave as reducing agents because they readily lose electrons. (12) * In a typical oxidation-reduction reaction the electrons are transferred (A) from the oxidizing agent to the reducing agent. (B) from what is being oxidized to the substance being reduced. (C) from what is being reduced to the substance being oxidized. (D) from what is being oxidized to the reducing agent. (E) none of these.

After 10.0 mL of a 0.020 M Ba(OH)2 (aq) are mixed with 15.0 mL of a 0.020 M KOH(aq), what is the molarity of [OH-]?

Write the ionic and net ionic equation for each reaction. Al(OH)3(s) + NaOH(aq) -----> Na[Al(OH)4](aq) Pb(NO3)2(aq) + KI(aq) -----> PbI2(s) + KNO3(aq)

Which of the below represents the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of iron(II) nitrate and potassium sulfide are mixed? Group of answer choices Fe2+(aq) + S2-(aq) → FeS(s) K+(aq) + NO3-(aq) → KNO3(s) 2 K+(aq) + S2-(aq) + Fe2+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) No reaction occurs. 2 K+(aq) + S2-(aq) + Fe2+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq)

Consider the neutralization reaction  2HNO3(aq) + Ba(OH)2(aq) yields to 2H2O(L) + Ba(NO3)2(aq) A 0.100 L sample of an unknow HNO3 solution required 49.3 mL of 0.100 M Ba(OH)2 for complete neutralization. What is the concentration of the HNO3 solution?

A student tries to determine experimentally the molar mass of aspirin (HAsp).She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is:HAsp(aq) + OH-(aq) ----> Asp-(aq) + H2O(l) What is the molar mass of aspirin?

What is made by adding solutions of Ba( NO3)2(aq) and NH4)2S(aq)?

A certain brand of vinegar is analyzed for its acetic acid content by titration with 0.2 moles/liter NaOH. The neutralization reaction is:CH3COOH(aq) + NaOH(aq) --> NaCH3COO(aq) + H2O(l)Here 6ml of the vinegar required 45 ml of the 0.2 moles/liter NaOH to be neutralized. Assume that the density of the vinegar is 1.15 g/ml. What is the % by mass of CH3COOH in the vinegar

A 10.00-mL sample of sulfuric acid, H2SO4, is titrated with 0.2760 M NaOH solution. If the titration requires 32.50 mL of the NaOH solution, what is the molar concentration of the H2SO4 solution? The acid-base reaction occurs as follows:             H2SO4(aq)  +  2NaOH(aq)  -->  Na2SO4(aq)  +  2H2O(l)

If 28.96 mL of 0.376 M barium hydroxide are needed to titrate 27.89 mL of nitric acid, what is the molarity of the acid? 2HNO, (aq) + Ba(OH);(aq) - Ba(NO)a(aq) + 2H,0) O0.521 M O 0.390 M O 0.260 M O 1.562 M O 0.781 M • Previous No new data to save. Last checke MacBook Air 234 80 F6 F7 F5