Consider the following titration: 20.0 mL of 0.060 MHClO4(in the flask) is titrated with 0.040 M NaOH (inburet).What is the overall reaction occurring in the titration? (Note thatHClO4is a strong acid) a)HClO4(aq)+ H2O----> H3O+(aq)+ ClO4-(aq) b) HClO4(aq)+ NaOH(aq) ----> H2O+ NaCl(aq) + 2 O2(g) c) HClO4(aq)+ NaOH(aq) -----> NaClO4(aq)+ H2O d) NaOH(aq) + H2O-----> H2O+ OH-(aq)+ Na+(aq)

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13 Dec 2019

Consider the following titration: 20.0 mL of 0.060 MHClO₄(in the flask) is titrated with 0.040 M NaOH (inburet).
What is the overall reaction occurring in the titration? (Note thatHClO₄is a strong acid)

a)HClO₄(aq)+ H₂O----> H₃O⁺(aq)+ ClO₄^-(aq)

b) HClO₄(aq)+ NaOH(aq) ----> H₂O+ NaCl(aq) + 2 O₂(g)

c) HClO₄(aq)+ NaOH(aq) -----> NaClO₄(aq)+ H₂O

d) NaOH(aq) + H₂O-----> H₂O+ OH^-(aq)+ Na⁺(aq)

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In the acid-base titration experiment, volume of base is measured as

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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+

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?
How many moles of each reactant are present in each trial?
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.

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 âNo Reactionâ. 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 doesnât 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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