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13 Dec 2019

1. Which net ionic equation best represents the reaction thatoccurs when an aqueous solution of barium chloride is mixed with anaqueous solution of sulfuric acid?


[A] BaCl2 + H2SO4 -> BaSO4 + 2HCL


[B] 2H+ (aq)+2Cl-(aq)-> HCl(g)


[C] Ba(2+)(aq) + SO4(2-)(aq) -> BaSO4 (s)


[D] Ba(2+)(aq)+2Cl-(aq)+2H+(aq)+SO4(2-)(aq)->BaSO4(s)+2HCl(g)


[E] No net reaction occurs.


2. What is the net ionic equation for the acid-base reactionthat occurs when acetic acid and sodium hydroxide solutions aremixed?


[A]H+(aq)+OH-(aq) -> H2O(l)


[B]H3O+(aq)+OH-(aq)->2H2O(l)


[C]HC2H3O2(aq)+NaOH(aq)->NaC2H3O2(aq)+ H2O(l)


[D]C2H3O2-(aq) + H+(aq) Na+(aq) +OH-(aq) ->Na+(aq) + C2H3O2-(aq) + H2O(l)


[E] HC2H3O2(aq) + OH- (aq) -> C2H3O2-(aq) + H2O (l)

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Beverley Smith
Beverley SmithLv2
17 Dec 2019

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Related questions

1. This experiment involves the reaction of Ba(OH)2 with H2SO4. Which of the following gives the balanced chemical reaction used in the experiment?

a. Ba(OH)2(aq) + H2SO4(aq) → H2Ba(s) + SO4(OH)2(l)
 
b. Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + H2O(l)
 
c. BaSO4(s) + 2H2O(l) → Ba(OH)2(aq) + H2SO4(aq)
 
d. Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + 2H2O(l)
 
2) Which of the following gives the net ionic reaction for the reaction used in this experiment?
 
a. H+(aq) + OH-(aq) → H2O(l)
 
b. no net reaction
 
c. Ba2+(aq) + SO42-(aq) → BaSO4(s)
 

d. Ba2+(aq) + 2OH-(aq) + 2H+(aq) + SO42-(aq) → BaSO4(s) + 2H2O(l)

3) Ranjit titrates a sample 10.00 mL of Ba(OH)2 solution to the endpoint using 12.58 mL of 0.1023 M H2SO4.

Based on this data, calculate the concentration of the barium hydroxide solution.

[Ba(OH)2] = ___ M

4) Xianming runs a titration and collects, dries, and weighs the BaSO4(s) produced in the experiment. He reports a mass of 0.2989 g  Ba2SO4. Based on this, calculate the concentration of Ba(OH)2 solution.

[Ba(OH)2] = ___ M

 

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)

 

What is the hydroxide concentration, [OH-], in a 3.85 M NaC2H3O2 solution? Consider the following information to help you answer this question: Sodium acetate is a water-soluble salt. Like all water-soluble ionic compounds, it dissociates completely when dissolved in water: H2O NaC2H3O2(s) ---------------> Na+(aq) + C2H3O2-(aq) Since the Na+ ion is the conjugate acid of a strong base (NaOH) it is too weak of an acid to react with water: Na+(aq) + H2O(l) ---------> N.R. Note: N.R. means “No Reaction”. However, the C2H3O2- ion is the conjugate base of a weak acid (HC2H3O2). Therefore, it is a strong enough base to react with water: C2H3O2-(aq) + H2O(l) <----------> HC2H3O2(aq) + OH-(aq) The above equilibrium reaction is the one for which you need to set up and solve an ICE table. However, the Kb value for C2H3O2- is normally not published in tables. It doesn’t need to be, because you can get it from two other values that are published: the Ka for HC2H3O2 and KW for the ionization of water. HC2H3O2(aq) + H2O(l) <----------> H3O+(aq) + C2H3O2-(aq) Ka = 1.8 x 10-5 2H2O(l) <----------> H3O+(aq) + OH-(aq) KW = 1.0 x 10-14 By combining the above two equations in the appropriate way, you can produce the reaction for which the equilibrium constant is desired. Once you have the required equilibrium constant, you can set up the ICE table in the usual way. Note that the initial concentration of C2H3O2- is the concentration given for NaC2H3O2. This is because the reaction proceeds to 100% completion, and the reaction has one-to-one stoichiometry. For every mole of NaC2H3O2, you get a mole of C2H3O2- (and a mole of Na+).

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