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13 Dec 2019

In an experiment, 700 mL of 0.5 M hydrochloric acid (HCl) is added to 600 mL of 0.5 M sodium hydroxide (NaOH) solution. The acid and base neutralize each other according to the equation: HCl + NaOH ---> NaCl + H2O

How many moles of acid and base were there originally?

The answer is 0.35 mole of HCl and 0.3 mole of NaOH

but, I can't seem to get that answer when I calculate it, so I'm not sure where I am going wrong.

Update: I figured it out.

.5 M x .7L = .35 mole of HCl

.5 M x .6L = .3 mole of NaOH

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Related questions

1.) Watch the animation, and observe the titration process using a standard 0.100 M sodium hydroxide solution to titrate 50.0 mL of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titrations are correct

Drag items A-F to: Before equivalence point, At equivalence point, After equivalence point

A.) The pH of the solution is close to 2

B.) The pH of the solution is close to 12

C.) The pH of the solution is 7

D.) The color of the solution is pink

E.) The color of the solution is blue

F.) The pH changes most rapidly

2.) Consider the balanced equation for the titration of an acid, HCl, with a base, NaOH:

HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(aq)

According to the balanced equation, to neutralize one mole of the acid (HCl) you will have to add one mole of the base (NaOH). Based on the number of moles of HCl and NaOH at a particular stage of titration, the progress of the reaction with respect to the equivalence point can be decided, as shown in the following table:

You can use the following equation to determine the number of moles in a given solution or volume of titrant: number of moles=molarity (mol/L)×volume (in liters)

A volume of 100 mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the equivalence point, or after the equivalence point.

Drag items A-F to Before equivalence point, At equivalence point, After equivalence point

A.) 50.0 mL of 1.00 M NaOH

B.) 150 mL of 1.00 M NaOH

C.) 200 mL of 1.00 M NaOH

D.) 10.0 mL of 1.00 M NaOH

E.) 5.00 mL of 1.00 M NaOH

F.) 100 mL of 1.00 M NaOH

The titration of the 5.00mL aliquot using the sodium hydroxide solution determines the total acid content. However, remember that you used .10M HCl to more quickly establish the hydrolysis equilibrium. The titration with the sodium hydroxide determines the total acid content of the aliquot,

NaOH + HCl -> H2O + Na + Cl
NaOH + CH3COOH -> H2O + Na + CH3COO

and so to determine the number of moles of acetic acid present in this aliquot, you have to first subtract out the amount of sodium hydroxide that reacts with the HCl.

I know that Total mols = mols of HCl added at the beginning + mols of acetic acid produced

I am assuming that the mols of HCl added at the begining is 0.005 mols because (0.05 L) x (0.10 M)

We added 50.0 mL of 0.1 M HCl and 3.00 mL of neat methyl acetate and let it set for a couple of days.

I then transfered 5.00 mL of the acid aliqout into a beaker.

We then titrated and used 18.5 mL of 0.2 NaOH to neutralize 5.00 mL of the acid aliquot.

Can someone help me find the total mols of acid in the aliquot? (I tried solving it and i got 0.004 mols but I think its wrong)

  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.

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