Which of the following reactions is a precipitation reaction? A) HNO:(aq) + NaOH(aq) → NaNO:(aq) + H:O(1) B) 2C2H:OH(I) + 70:(g) → 4CO:(g) + 6H2O(I) C) 2H:O2(1) → 2H:O(1) + O:(g) D) FeSO:(aq) + K:S(aq) → FeS(s) + K:SO:(aq)

Determine net ionic equations, if any, occuring when aqueous solutions of the following reactants are mixed. Nickel(II) chloride and lead(II) nitrate; Pb2+(aq) + 2Cl-(aq) -> PbCl2(s) Ammonium sulfate and barium nitrate; Ba2+(aq) + SO42-(aq) -> BaSO4(s) Copper(II) sulfate and ammonium carbonate; No reaction occurs. Sodium bromide and hydrochloric acid; Na+(aq) + Cl-(aq) -> NaCl(s) Calcium acetate and sodium carbonate; Ca2+(aq) + CO32-(aq)  CaCO3(s)

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)

Which of the following reactions are redox reactions?    i)   2 C6H6 (l)   +   15 O2 (g)     ->     12 CO2 (g)   +    6 H2O (g)                                    ii)   Pb(NO3) 2 (aq)    +    2 KCl  (aq)    -->    PbCl2 (s)    +   2 KNO3(aq)                     iii)   3 Mg (s)    +   2 FeCl3 (aq)    -->    3 MgCl2 (aq)   +   2 Fe (s)

For the reaction that occurs when the following solutions are mixed, write (i) the balanced molecularequation including states of matter of all products, (ii) the complete/full ionic equation, (iii) the net ionic equation AND (iv) the names of all reactants.

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg .   Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 111. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 0-2 X 5

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?

Which one(s) of the following reactions is(are) redox reactions? (a) Na (s) + H2O (l) → NaOH (aq) + H2 (g) (b) NaOH (aq) + HCl (aq) → NaCl (aq) + H2O (l) (c) H2O (l) → O2 (g) + H2 (g) (d) Ag+ (aq) + Cl- (aq) → AgCl (s)

|A 500-g sample of Al, (SO, ); is reacted with 450 g of Ca(OH),. A total of 596 g of CaSO, is produced. Al, (SO4)3(ag) + 3Ca(OH) 2(aq) →2AI(OH) 3(s) + 3CaSO (s) Determine the following: