Include s, aq, l, etc. Consider the reaction when aqueous solutions of aluminum chloride and ammonium...

Include s, aq, l, etc.

Consider the reaction when aqueous solutions of aluminum chloride and ammonium nitrate are combined.

Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hypochlorous acid are combined.

Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrobromic acid and ammonia are combined.

Write a net ionic equation for the reaction that occurs when aqueous solutions of perchloric acid and barium hydroxide are combined.

(Use H⁺ instead of H₃O⁺.)

Write a net ionic equation for the reaction that occurs when aqueous solutions of sodium hydroxide and hypochlorous acid are combined.

Write a net ionic equation for the overall reaction that occurs when aqueous solutions of hydrosulfuric acid and potassium hydroxide are combined. Assume excess base.

Solutions

Expert Solution

Consider the reaction when aqueous solutions of aluminum chloride and ammonium nitrate are combined.

AlCl3 (aq) + 3 NH4NO3 (aq) -------------> Al(NO3)3 (aq) + 3 NH4Cl (aq)

Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and hypochlorous acid are combined.

Net ionic : NH3 (aq) + HClO (aq) ------------> NH4+ (aq) + ClO- (aq)

Write a net ionic equation for the reaction that occurs when aqueous solutions of hydrobromic acid and ammonia are combined.

Net ionic : H+ (aq) + NH3 (aq) -----------> NH4+ (aq)

Write a net ionic equation for the reaction that occurs when aqueous solutions of perchloric acid and barium hydroxide are combined.

Net ionic : H+ (aq) + OH- (aq) -------------> H2O (l)

Write a net ionic equation for the reaction that occurs when aqueous solutions of sodium hydroxide and hypochlorous acid are combined.

Net ionic : HClO (aq) + OH- (aq) ----------> ClO- (aq) + H2O (l)

Write a net ionic equation for the overall reaction that occurs when aqueous solutions of hydrosulfuric acid and potassium hydroxide are combined. Assume excess base.

Net ionic : H2S (aq) + OH- (aq) -------------> HS- (aq) + H2O (l)

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

When aqueous solutions of ammonium carbonate and aluminum iodide are combined, solid aluminum carbonate and a...

When aqueous solutions of ammonium carbonate and aluminum iodide are combined, solid aluminum carbonate and a solution of ammonium iodide are formed. The net ionic equation for this reaction is:

Activity 4: Equilibrium of solid ammonium chloride with ammonium chloride in aqueous solution. NH4Cl(s) +H2O(l) ...

Activity 4: Equilibrium of solid ammonium chloride with ammonium chloride in aqueous solution. NH4Cl(s) +H2O(l)  NH4+(aq) + Cl-(aq) (ammonium chloride) (ammonium ion) Procedure * Pour about 75 mL of tap water into a 150-mL beaker and heat to boiling on a hot plate. * While waiting for the water to boil, place approx. 1 mL of a saturated NH4Cl solution into a small, clean, dry test tube. *To this test tube, add concentrated HCl solution one drop at a...

consider the reaction between Mg(s) and HCl(aq) to producer aqueous magnesium chloride and hydrogen gas. How...

consider the reaction between Mg(s) and HCl(aq) to producer aqueous magnesium chloride and hydrogen gas. How many liters of hydrogen gas at STP will be produced when 12.15 g of magnesium reacts with an excess of hydrochloric acid?

Consider the following reaction in aqueous solution: 5Br-(aq) + BrO3-(aq) + 6H+(aq) →3Br2(aq) + 3H2O(l) If...

Consider the following reaction in aqueous solution: 5Br-(aq) + BrO3-(aq) + 6H+(aq) →3Br2(aq) + 3H2O(l) If the rate of appearance of Br2(aq) at a particular moment during the reaction is 5.5x10-5M/s, what is the rate of disappearance of Br-(aq) at that moment?

Solid Aluminum nitrite reacts with solid ammonium chloride to form aluminum chloride, nitrogen gas, and water....

Solid Aluminum nitrite reacts with solid ammonium chloride to form aluminum chloride, nitrogen gas, and water. What is the maximum possible mass of gas produced when 61.5g of aluminum nitrite and 49.6g of ammonium chloride are allowed to react completely.? Please show al steps so I can understand it. Thank you.

Consider the reaction of 1.35g aluminum and 100. ml of 1.20 M HBr 2Al(s) + 6HBr(aq)---->2AlBr3(aq)...

Consider the reaction of 1.35g aluminum and 100. ml of 1.20 M HBr 2Al(s) + 6HBr(aq)---->2AlBr3(aq) + 3 H2(g) Employ an Ice Table in calculating these find what amount of excess reagent will remain unreacted Find the mass of AlBr3 should be collected if the reactions run at a 75% yield

10.5 mL of 0.100M ammonium chloride aqueous solution is titrated with 0.100 M NaOH(aq). What type...

10.5 mL of 0.100M ammonium chloride aqueous solution is titrated with 0.100 M NaOH(aq). What type of solution is present when VNaOH = 2.00 mL? Select one: a. strong acid b. strong base c. weak acid d. weak base e. buffered

Consider the ionization of aqueous ammonia: NH3(aq) + H2O(l) ⇌ NH4 + (aq) + OH- (aq)...

Consider the ionization of aqueous ammonia: NH3(aq) + H2O(l) ⇌ NH4 + (aq) + OH- (aq) a)Using the thermodynamic data from the textbook (Appendix C), calculate the values of ∆H°rxn, ∆G°rxn, and ∆S°rxn for this process at 25o C. b)Calculate the value of Kb (with 2 sig figs) at 25o C from the value of ∆G°rxn. c) The value of ∆G°rxn you obtain (if your calculations are correct) must be positive, indicating that the reaction in question is non-spontaneous. Why...

Consider the given reaction. MgCO3(s) + 2 HCl(aq) — MgCl2(aq) + H2O(l) + CO2(g)

Consider the given reaction. MgCO3(s) + 2 HCl(aq) — MgCl2(aq) + H2O(l) + CO2(g) Calculate the atom economy of this reaction to form carbon dioxide assuming that no other reactions are occurring. atom economy = _______ %

Reaction 1: NaOH(s)--> NaOH (aq) Reaction 2: NaOH(s) + HCl (aq)--> NaCl(aq)+H2O(l) Reaction 3: NaOH(aq) +HCl...

Reaction 1: NaOH(s)--> NaOH (aq) Reaction 2: NaOH(s) + HCl (aq)--> NaCl(aq)+H2O(l) Reaction 3: NaOH(aq) +HCl (aq) --> NaCl (aq) + H2O (L) 1) Describe each reaction as endothermic or exothermic and explain your reasoning. 2) Examine the chemical equations for the three reactions. Determine their relationship in a way that is consistent with Hess's Law. (i.e. verify that Hess's Law is upheld. Reaction 3 is the target equation). 3) Why is heat a stoichiometric quality? 4) Just what IS...

Subjects