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Consider the following acid-neutralization reactions involving the strong base NaOH(aq):
HNO3(aq) + NaOH(aq) NaNO3(aq) + H2O(l)
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
NH4+(aq) + NaOH(aq) NH3(aq) + Na+(aq) + H2O(l)

(a) By using data in Appendix C, calculate ∆H° for each of the reactions. (b) As we saw in Section 4.3, nitric acid and hydrochloric acid are strong acids. Write net ionic equations for the neutralization of these acids. (c) Compare the values of ∆H° for the first two reactions. What can you conclude? (d) In the third equation NH4+ (aq) is acting as an acid. Based on the value of ∆H° for this reaction, do you think it is a strong or a weak acid? Explain.

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Collen Von
Collen VonLv2
29 May 2020

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Related questions

Write (1) a balanced molecular equation, (2) a total ionic equation, and (3) a net ionic equation that would describe a predicted reaction. Please pay attention to details such as charges (e.g. Ba2+ vs. Ba) and states (i.e. (aq), (s), (l), or (g) as appropriate). If a reaction is not predicted to occur (soluble salts on both sides of the equation), only the balanced molecular equation is needed.

 

sodium carbonate + sulfuric acid

Na2CO3 (aq)+ H2SO4(aq) -> Na2SO4(aq) + CO2 (g)+ H2O(l)

Na+(aq)+CO3^2−(aq)+2H+(aq)+SO4^2−(aq) ->H2O(l)+CO2(g)+2Na+(aq)+SO4^2−(aq)

CO3^2−(aq)+2H+(aq) -> H2O(l)+CO2(g)

 

sodiumcarbonate + hydrochloric acid

Na2CO3(aq) + HCl (aq)-> NaCl (aq)+ H2O (l)+ CO2(g)

Na+(aq) + CO3^-2 (aq)

 

potassium chloride + sodium carbonate

KCl (aq)+ Na2CO3 (aq)-> K2CO3 (aq)+ 2NaCl(aq)

 

potassium chloride + silver nitrate

KCl (aq)+ AgNO3 (aq) -> KNO3 (aq)+ AgCl (s)

 

potassium chloride + sodium nitrate

KCl (aq)+ NaNO3 (aq) ->  KNO3 (aq)+ NaCl(aq)

 

nickel chloride + silver nitrate

NiCl2 (aq)+ 2AgNO3(aq) ->  Ni (NO3)2(aq) + 2AgCl (s)

 

nickel chloride + sodium carbonate

KCl (aq)+ Na2CO3(aq) -> K2CO3 (aq)+ 2NaCl(aq)

 

hydrochloric acid + sodium hydroxide

HCl (aq)+ NaOH(aq) ->  NaCl(aq) + H2O(l)

 

Ammonium chloride + sodium hydroxide

NH4Cl(aq) + NaOH(aq) ->  NaCl(aq) + H2O (l)+ NH3(g)

 

sodium acetate + hydrochloric acid

CH3COONa (aq)+HCl (aq) ->  CH3COOH(aq) +NaCl(aq)

 

lead nitrate + sulfuric acid

Pb(NO3)2 (aq)+ H2SO4(aq) -> PbSO4 (aq)+ HNO3(aq)

 

  1. You will investigate three reactions in this experiment. In thespace provided below, write the balanced molecular and net ionicequations from the descriptions of the reactions. Use the table ofstandard heats of formation in your text (or another approvedresource) to calculate the molar enthalpies of the reactions.
  • Reaction 1: An aqueous solution of sodium hydroxide reacts withan aqueous solution of hydrochloric acid, yielding water.

  • Reaction 2: An aqueous solution of sodium hydroxide reacts withan aqueous solution of ammonium chloride, yielding aqueous ammonia,NH3, and water.

  • Reaction 3: An aqueous solution of hydrochloric acid reacts withaqueous ammonia, NH3, yielding aqueous ammonium chloride.

Reaction

Balanced Reaction Equation

?H (KJ)

1

NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l)

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

2

NaOH(aq) + NH4Cl(aq) -> NaCl(aq) + NH3(g) + H2O(l)

Net ionic: NH4+ (aq) + OH- (aq) -> NH3(g) + H2O(l)

3

HCl(aq) + NH3(aq) -> NH4+ + Cl-

Net ionic: H+ (aq) + NH3 (aq) -> NH4+
  1. For each reaction you perform, you will mix together 50.0 mL of2.00 M acid and 2.00 M base. What are the resulting concentrationsof the reactants upon mixing?
  2. How many moles of each reactant are present in each trial?
  3. What is the total volume of the solutions upon mixing? Assuminga density of 1.03 g/mL for the solution, find the total mass ofeach reaction mixture.

Hello, I have what I think are the right balanced equations butI can't figure out how to calculate the enthalpy (delta H) and I'munsure of how to do questions 1, 2, and 3 after the table.

1. Which of the following equations represents the proper net ionicequation for the precipitation of an insoluble carbonate compoundfrom Pb(NO3)2 (aq) and Na2CO3 (aq)?

Na2CO3 (aq) + Pb(NO3)2 (aq) ----> 2 NaNO3 (aq) + PbCO3 (s)
Pb2+ (aq) + CO32- (aq) ----> PbCO3 (s)
Na2CO3 (aq) + 2 NO3- (aq) ----> 2 NaNO3 (s) + CO32- (aq)
NO3- (aq) + Na+ (aq) ----> NaNO3 (s)
CO32- (aq) + Pb(NO3)2 (aq) ----> PbCO3 (s) + 2 NO3- (aq)
3 CO32-(aq) + 2 Pb3+(aq) ----> Pb2(CO3)3(s)
Na2+ (aq) + (NO3)2- (aq) ----> Na2(NO3)2 (s)
Na2CO3 (aq) + Pb(NO3)2(aq) ----> Na2(NO3)2 (aq) + PbCO3(s)
Pb+(aq) + CO3-(aq) ----> PbCO3 (s)


2. Which of the following equations represents the proper net ionicequation for the complete neutralization reaction between thestrong base, LiOH (aq) and the weak acid H2SO3 (aq) ?

H2SO3 (aq) + 2 OH-(aq) ---> 2 H2O (l) + SO32-(aq)
H2SO3 (aq) + 2 LiOH (aq)---->2 H2O (l) + Li2SO3 (aq)
SO32- (aq)+ 2 Li+(aq)----> Li2 SO 3 (aq)
H2+ (aq) + 2 OH- (aq) ----> 2 H2O (l)
H+ (aq) + OH- (aq) ----> H2O (l)
H+ (aq) + LiOH (aq) ----> H2O (l) + Li+ (aq)
H+ (aq) + Li+ (aq) ----> HLi (aq)
SO32- (aq) + OH- (aq) ----> HSO4 (aq)

3. What are the spectator ions in the solution after completelyprecipitating an insoluble sulfide compound when mixing Na2S (aq)and ZnBr2 (aq)?

Na+ , S2- , Zn2+ , and Br-
S2- and Zn2+
Br- and S2-
S2- and Na+
Na+ and Zn2+
Br- and Zn2+
Zn2+
Br-
Na+ and Br-
Na+

4. What are the spectator ions in the solution after the completeneutralization reaction occurs when mixing the weak acid HCN (aq)and the strong base NaOH (aq)?

H+ , CN-, Na+ , and OH-
OH- and Na+
H+ and OH-
Na+
OH- and CN-
Na+ and CN-
Na+ and H+
CN- and H+
CN-

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