CHM 1711 Study Guide - Quiz Guide: Dune, Titration, Sodium Hydroxide

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19 Dec 2015

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Tableau 1 : pr paration d"une solution de naoh par dilution. Volume de la solution de naoh concentr e (ml) Concentration de la solution de naoh originale (m) Volume de la solution de base apr s dilution (ml) Concentration approximative de la solution de base dilu e (m) Tableau 2 : talonnage de la solution dilu e de naoh. Concentration moyenne de la solution dilu e de naoh (m) Tableau 3 : d termination de la concentration d"un acide inconnu. La solution de naoh avant et apr s la dilution est incolore et inodore. La solution de hcl avant la dilution est incolore et inodore. La solution de l"acide inconnu no2 avant la dilution est incolore et inodore. La solution du jus inconnu no2 avant la dilution est incolore et inodore. La ph nolphtal ine d gage une forte odeur et est incolore. L"ajout de la ph nolphtal ine dans chacune des solutions ne cause aucune variation de couleur.

Related Questions

1)Calculate the final concentration of each of the following:

2.6 L of a 5.0 M HCl solution is added to water so that the final volume is 7.0 L . Cfinal = ? M

Water is added to 0.40 L of a 12 M NaOH solution to make 4.0 L of a diluted NaOH solution. Cfinal = ?M

A15.0 âmL sample of a 16 % (m/v) KOH solution is diluted with water so that the final volume is 120.0 mL . Cfinal = % (m/v)

A 75.0 âmL sample of a 18 % (m/v) H2SO4 solution is added to water to give a final volume of 410 mL . Cfinal = % (m/v) 3)

2)Calculate the final concentration of the solution when water is added to prepare each of the following solutions.

17.0 mL of a 15.0 %(m/v)

K2SO4 solution is diluted to 80.0 mL Answer should be in % (m/v) 80.0 mL of a 6.00 M NaOH solution is diluted to 235 mL Answer should be in M

Number of trials	Trial 1
volume of standard oxalic acid solution (mL)	25.00
molarity of standard H2C2O4 solution (M)	0.072
number of moles of H2C2O4 (mol)	?
Initial buret reading (mL)	0.00
final buret reading (mL)	31.40
volume or titrant (base) (mL)	31.40
number of moles NaOH (mol)	?
molarity of NaOH (M)	?

1. What is the number of moles of H2C2O4 ?

2. What is the number of moles NaOH?

3. What is the molarity of NaOH?

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)âNaCl(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)Ãvolume (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

CHM 1711 Study Guide - Quiz Guide: Dune, Titration, Sodium Hydroxide

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