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All properties of acids are due to

Neutralization Reaction. All properties of acids are due to. H +. All properties of bases are due to. OH-. When H + meet OH-, water is created. H +. H 2 O. OH-. Since there are no more H + or OH-, the solution is neither acidic nor basic.

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All properties of acids are due to

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  1. Neutralization Reaction All properties of acids are due to H+ All properties of bases are due to OH- When H+ meet OH-, water is created. H+ H2O OH- Since there are no more H+ or OH-, the solution is neither acidic nor basic In order to completely neutralize a solution, we need the exact same number of H+ from acids and OH- from bases Too many H+ , still acidic. Too many OH-, still basic H2O Neutral Acidic Basic H2O H2O H+ H2O OH- H+ H+ H+ OH- OH- OH- OH-

  2. C. Titration of Acids and Bases Titration Method of calculating the concentration of an acid or base solution Based on the fact that for every H+, we need one OH- in order to cancel it out 2 types of questions 1. Finding moles of acid or base For every mole of H+, we will need one mole of OH- to neutralize it Examples 1. If we have 3.0 moles of hydroxides in solution, how many moles of hydrogen ions are needed to neutralize them? 3.0 moles of OH- So need 3.0 moles of H+

  3. 2. If we had 200.0 ml of a 0.80 M solution of HCl, how many moles of OH- would we need to neutralize this? Need to find the moles of HCl Which is the same as moles of H+ Use the MOLARITY formula Molarity = moles Liters 0.80 M = ___x___ 0.200 L X = 0.16 moles of H+ So we need 0.16 moles of OH- 3. If we needed to neutralize 150.0 ml of a 3.0 M NaOH solution, how many moles of H+ would we need? Molarity = moles Liters 3.0 M = ___x___ 0.150 L X = 0.45moles of OH- So we need 0.45 moles of H+

  4. 2. Finding Volumes or Molarity Since M = moles liter If we multiply the molarity x the volume of an acid Ma x Va = moles of H+ If we multiply the molarity x the volume of a base Mb x Vb = moles of OH- When we neutralize the acid and base, moles of H+ must equal moles of OH- so Ma x Va = Mb x Vb Example -1. How many milliliters of 1.0 M HCl are needed to neutralize 200.0 ml of a 2.0 M NaOH solution? Ma x Va = Mb x Vb 1.0 x x = 2.0 x 200.0 ml x= 400.0 400 ml = Va

  5. 2. How much 0.10 M HCl is needed to neutralize 200.0 ml of a 0.30 M NaOH solution? Ma x Va = Mb x Vb 0.10 M x Va = 0.30 M x 200.0 ml Va = 600 ml 3. If H+ and OH- Do Not Match Up HCl creates only one H+ NaOH creates only one OH- Since these two match up, we can use the simple formula. On rare occasions, the H+ in the acid will not equal the OH- of the base. H2SO4 Creates 2 H+ LiOH Creates only 1 OH- We would need 2 LiOH to neutralize one H2SO4 In this case, we need to use a special formula na xMa x Va = nb x Mb x Vb nb = number of OH- in the base na = number of H+ in the acid

  6. Examples 1. What is the concentration of HCl if 30.0 ml of the acid are neutralized by 50.0 ml of a 3.0 M Ca(OH)2 solution? na xMa x Va = nb x Mb x Vb 1 x Ma x 30.0 = 2 x 3.0 x 50.0 Ma = 10. M 2. How many ml of 0.50 M H2SO4 is needed to neutralize 100.0 ml of a 2.5 M KOH solution? na xMa x Va = nb x Mb x Vb 2 x 0.50 x Va = 1 x 2.5 x 100.0 Va = 250 ml

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